no grades until jan 10

isn't that the best news?

merry christmas boys

hope you have a great holiday!

Lab 2: Chemica; Properties of Magnesium

for your notes

Bonus

find me power points for the following chapters: 13, 21, 22, 23

Bonus

find me power points for the following chapters: 13, 21, 22, 23

Any Final Questions

if you have any final question, please ask by 3:45 p.m.

Sample Exam EP 5 December 2009

EP 4 Sample Exam December 2009

Matching

Match each item with the correct statement below.
a. molar volume
b. molar mass
c. atomic mass


____ 1. the number of grams of an element that is numerically equal to the atomic mass of the element in amu

____ 2. the mass of a mole of any element or compound

____ 3. the volume occupied by a mole of any gas at STP

Match each item with the correct statement below.
a. representative particle d. percent composition
b. mole e. standard temperature and pressure
c. Avogadro's number f. empirical formula


____ 4. the number of representative particles of a substance present in 1 mole of that substance

____ 5. an atom, an ion, or a molecule, depending upon the way a substance commonly exists

____ 6. the SI unit used to measure amount of substance

____ 7. 0 C and 1 atm

____ 8. the percent by mass of each element in a compound

____ 9. the smallest whole number ratio of the atoms in a compound

Match each item with the correct statement below.
a. product d. balanced equation
b. reactant e. skeleton equation
c. chemical equation


____ 10. a chemical equation that does not indicate relative amounts of reactants and products

____ 11. a new substance formed in a chemical reaction

____ 12. a starting substance in a chemical reaction

____ 13. a concise representation of a chemical reaction

____ 14. an equation in which each side has the same number of atoms of each element

Match each item with the correct statement below.
a. activity series of metals c. combustion reaction
b. single-replacement reaction d. decomposition reaction


____ 15. a reaction in which a single compound is broken down into simpler substances

____ 16. a reaction in which oxygen reacts with another substance, often producing heat or light

____ 17. a reaction in which the atoms of one element replace the atoms of a second element in a compound

____ 18. a list of metals in order of decreasing reactivity

Match each item with the correct statement below.
a. actual yield e. limiting reagent
b. percent yield f. mass
c. theoretical yield g. number of molecules
d. excess reagent h. volume


____ 19. This quantity can always be used in the same way as moles when interpreting balanced chemical equations.

____ 20. This is conserved only in reactions where the temperature is constant and the number of moles of gaseous reactants is the same as that of gaseous products.

____ 21. This is conserved in every ordinary chemical reaction.

____ 22. the reactant that determines the amount of product that can be formed in a reaction

____ 23. the maximum amount of product that could be formed from given amounts of reactants

____ 24. the reactant that is not completely used up in a reaction

____ 25. the amount of product formed when a reaction is carried out in the laboratory

____ 26. the ratio of the actual yield to the theoretical yield

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 27. What SI unit is used to measure the number of representative particles in a substance?
a. kilogram c. kelvin
b. ampere d. mole


____ 28. How many atoms are in 3.5 moles of arsenic atoms?
a. 5.8 10 atoms c. 2.1 10 atoms
b. 7.5 10 atoms d. 1.7 10 atoms


____ 29. What is true about the molar mass of chlorine gas?
a. The molar mass is 35.5 g.
b. The molar mass is 71.0 g.
c. The molar mass is equal to the mass of one mole of chlorine atoms.
d. none of the above


____ 30. What is the mass of silver in 3.4 g AgNO ?
a. 0.025 g c. 2.2 g
b. 0.64 g d. 3.0 g


____ 31. What is the percent by mass of carbon in acetone, C H O?
a. 20.7% c. 1.61%
b. 62.1% d. 30.0%


____ 32. Which expression represents the percent by mass of nitrogen in NH4NO3?
a. 14 g N/80 g NH NO 100% c. 80 g NH NO /14 g N 100%
b. 28 g N/80 g NH NO 100% d. 80 g NH NO /28 g N 100%


____ 33. Which of the following compounds has the highest oxygen content, by weight?
a. Na O c. BaO
b. CO d. H O


____ 34. What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?
a. C HN c. C H N
b. C H N d. CH N


____ 35. The ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of dicyclohexyl maleate is 4 to 6 to 1. What is its molecular formula if its molar mass is 280 g?
a. C H O c. C H O
b. C H O d. C H O


____ 36. Which of the following is NOT true about empirical and molecular formulas?
a. The molecular formula of a compound can be the same as its empirical formula.
b. The molecular formula of a compound can be some whole-number multiple of its empirical formula.
c. Several compounds can have the same empirical formula, but have different molecular formulas.
d. The empirical formula of a compound can be triple its molecular formula.


____ 37. Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a. PbO Pb 2O c. Pb O 2Pb O
b. PbO Pb O d. PbO Pb O


____ 38. What are the correct formulas and coefficients for the products of the following double-replacement reaction?
RbOH H PO
a. Rb(PO ) H O c. Rb PO 3H O
b. RbPO 2H O d. H Rb PO OH


____ 39. How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s)  3Fe(s) + Al O (s)
a. 1.2 mol c. 1.6 mol
b. 0.8 mol d. 2.4 mol


____ 40. Calculate the number of moles of Al O that are produced when 0.60 mol of Fe is produced in the following reaction.
2Al(s) + 3FeO(s) 3Fe(s) + Al O (s)
a. 0.20 mol c. 0.60 mol
b. 0.40 mol d. 0.90 mol


EP 4 Sample Exam December 2009
Answer Section

MATCHING

1. ANS: C DIF: L1 REF: p. 294 OBJ: 10.1.3

2. ANS: B DIF: L1 REF: p. 294, p. 295
OBJ: 10.1.3, 10.1.4

3. ANS: A DIF: L1 REF: p. 300 OBJ: 10.2.2

4. ANS: C DIF: L1 REF: p. 290 OBJ: 10.1.2

5. ANS: A DIF: L1 REF: p. 290 OBJ: 10.1.2

6. ANS: B DIF: L1 REF: p. 290 OBJ: 10.2.1

7. ANS: E DIF: L1 REF: p. 300 OBJ: 10.2.2

8. ANS: D DIF: L1 REF: p. 305 OBJ: 10.3.1

9. ANS: F DIF: L1 REF: p. 309 OBJ: 10.3.2

10. ANS: E DIF: L1 REF: p. 323 OBJ: 11.1.2

11. ANS: A DIF: L1 REF: p. 323 OBJ: 11.1.2

12. ANS: B DIF: L1 REF: p. 323 OBJ: 11.1.2

13. ANS: C DIF: L1 REF: p. 323 OBJ: 11.1.3

14. ANS: D DIF: L1 REF: p. 325 OBJ: 11.1.3

15. ANS: D DIF: L1 REF: p. 332 OBJ: 11.2.1

16. ANS: C DIF: L1 REF: p. 336, p. 337
OBJ: 11.2.1

17. ANS: B DIF: L1 REF: p. 333 OBJ: 11.2.1

18. ANS: A DIF: L1 REF: p. 333 OBJ: 11.2.2

19. ANS: G DIF: L1 REF: p. 356 OBJ: 12.1.2

20. ANS: H DIF: L1 REF: p. 357 OBJ: 12.1.2

21. ANS: F DIF: L1 REF: p. 357 OBJ: 12.1.2

22. ANS: E DIF: L1 REF: p. 369 OBJ: 12.3.1

23. ANS: C DIF: L1 REF: p. 369 OBJ: 12.3.1

24. ANS: D DIF: L1 REF: p. 372 OBJ: 12.3.2

25. ANS: A DIF: L1 REF: p. 372 OBJ: 12.3.2

26. ANS: B DIF: L1 REF: p. 372 OBJ: 12.3.2

MULTIPLE CHOICE

27. ANS: D DIF: L1 REF: p. 290 OBJ: 10.1.2

28. ANS: C DIF: L2 REF: p. 291, p. 292
OBJ: 10.1.2

29. ANS: B DIF: L2 REF: p. 294 OBJ: 10.1.3

30. ANS: C DIF: L2 REF: p. 298 OBJ: 10.2.1

31. ANS: B DIF: L2 REF: p. 307 OBJ: 10.3.1

32. ANS: B DIF: L2 REF: p. 307 OBJ: 10.3.1

33. ANS: D DIF: L3 REF: p. 307 OBJ: 10.3.1

34. ANS: C DIF: L2 REF: p. 310 OBJ: 10.3.2

35. ANS: D DIF: L3 REF: p. 310 OBJ: 10.3.2

36. ANS: D DIF: L1 REF: p. 311 OBJ: 10.3.3

37. ANS: B DIF: L2 REF: p. 332 OBJ: 11.2.1

38. ANS: C DIF: L2 REF: p. 334, p. 335
OBJ: 11.2.1

39. ANS: B DIF: L1 REF: p. 359, p. 360
OBJ: 12.2.1

40. ANS: A DIF: L1 REF: p. 359, p. 360
OBJ: 12.2.1

EP 5 Sample Midterm December 2009

EP 5 Sample Exam December 2009

Matching

Match each item with the correct statement below.
a. activated complex d. activation energy
b. reaction rate e. free energy
c. inhibitor


____ 1. the minimum energy colliding particles must have in order to react

____ 2. arrangement of atoms at the peak of an energy barrier

____ 3. the number of atoms, ions, or molecules that react in a given time to form products

____ 4. a substance that interferes with a catalyst

____ 5. energy available to do work

Match each item with the correct statement below.
a. spontaneous reaction d. reaction mechanism
b. entropy e. elementary reaction
c. chemical equilibrium


____ 6. when the forward and reverse reactions take place at the same rate

____ 7. a reaction that releases free energy

____ 8. the measure of disorder

____ 9. Reactants are converted to products in a single step.

____ 10. includes all elementary reactions of a complex reaction

Match each item with the correct statement below.
a. acid dissociation constant d. Lewis acid
b. diprotic acid e. pH
c. hydrogen-ion donor


____ 11. can accept an electron pair

____ 12. acid with two ionizable protons

____ 13. Brønsted-Lowry acid

____ 14. negative logarithm of the hydrogen ion concentration

____ 15. ratio of the concentration of the dissociated to the undissociated form

Match each item with the correct statement below.
a. salt hydrolysis d. equivalence point
b. end point e. buffer capacity
c. titration


____ 16. process of adding a known amount of solution of known concentration to determine the concentration of another solution

____ 17. The number of moles of hydrogen ions equals the number of moles of hydroxide ions.

____ 18. Indicator changes color.

____ 19. Cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water.

____ 20. the amount of acid or base that can be added to a buffer solution before a significant change in pH occurs

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 21. Which expression represents a reaction rate?
a. time/mass c. energy/time
b. number/time d. time/energy


____ 22. Activation energy is ____.
a. the heat released in a reaction
b. an energy barrier between reactants and products
c. the energy given off when reactants collide
d. generally very high for a reaction that takes place rapidly


____ 23. Why does a catalyst cause a reaction to proceed faster?
a. There are more collisions per second only.
b. The collisions occur with greater energy only.
c. The activation energy is lowered only.
d. There are more collisions per second and the collisions are of greater energy.


____ 24. If a reaction is reversible, what are the relative amounts of reactant and product at the end of the reaction?
a. no reactant; all product
b. no product; all reactant
c. some product; some reactant
d. The relationship between reactants and products cannot be determined.


____ 25. What happens to a reaction at equilibrium when more reactant is added to the system?
a. The reaction makes more products. c. The reaction is unchanged.
b. The reaction makes more reactants. d. The answer cannot be determined.


____ 26. Which of the following statements is true?
a. All spontaneous processes are exothermic.
b. All nonspontaneous processes are endothermic.
c. All spontaneous processes release free energy.
d. Entropy always increases in a spontaneous process.


____ 27. What determines whether or not a reaction is spontaneous?
a. change in molar volume and heat change
b. change in enthalpy only
c. enthalpy change and entropy change
d. change in entropy only


____ 28. Which variable is NOT required to calculate the Gibbs free-energy change for a chemical reaction?
a. change in enthalpy c. temperature in kelvins
b. temperature in C d. change in entropy


____ 29. What is the order of the following reaction? A + 2B  C + D
a. zero c. second
b. first d. third


____ 30. What information is NOT given by an overall equation for a chemical reaction?
a. the relative numbers of molecules used
b. the probable order of the reaction
c. the number of atoms participating in the reaction
d. the reaction mechanism


____ 31. Which of the following reactions illustrates amphoterism?
a. H O + H O H O + OH c. HCl + H O H O + Cl
b. NaCl Na + OH d. NaOH Na + OH


____ 32. What is the charge on the hydronium ion?
a. 2– c. 0
b. 2– d. 1+


____ 33. The products of self-ionization of water are ____.
a. H O and H O c. OH and H
b. OH and OH d. OH and H


____ 34. Which type of solution is one with a pH of 8?
a. acidic
b. basic
c. neutral
d. The type varies, depending on the solution.


____ 35. Which of these solutions is the most basic?
a. [H ] = 1 10 M c. [H ] = 1 10 M
b. [OH ] = 1 10 M d. [OH ] = 1 10 M


EP 5 Sample Exam December 2009
Answer Section

MATCHING

1. ANS: D DIF: L1 REF: p. 543 OBJ: 18.1.1

2. ANS: A DIF: L1 REF: p. 544 OBJ: 18.1.1

3. ANS: B DIF: L1 REF: p. 542 OBJ: 18.1.1

4. ANS: C DIF: L1 REF: p. 547 OBJ: 18.1.2

5. ANS: E DIF: L1 REF: p. 566 OBJ: 18.4.1

6. ANS: C DIF: L1 REF: p. 550 OBJ: 18.2.1

7. ANS: A DIF: L1 REF: p. 567 OBJ: 18.4.1

8. ANS: B DIF: L1 REF: p. 569 OBJ: 18.4.2

9. ANS: E DIF: L1 REF: p. 578 OBJ: 18.5.2

10. ANS: D DIF: L1 REF: p. 578 OBJ: 18.5.2

11. ANS: D DIF: L1 REF: p. 592 OBJ: 19.1.2

12. ANS: B DIF: L1 REF: p. 588 OBJ: 19.1.2

13. ANS: C DIF: L1 REF: p. 590 OBJ: 19.1.2

14. ANS: E DIF: L1 REF: p. 596 OBJ: 19.2.2

15. ANS: A DIF: L1 REF: p. 606 OBJ: 19.3.1

16. ANS: C DIF: L1 REF: p. 613, p. 614, p. 615
OBJ: 19.4.1

17. ANS: D DIF: L1 REF: p. 613 OBJ: 19.4.2

18. ANS: B DIF: L1 REF: p. 615 OBJ: 19.4.2

19. ANS: A DIF: L1 REF: p. 619 OBJ: 19.5.1

20. ANS: E DIF: L1 REF: p. 621 OBJ: 19.5.2

MULTIPLE CHOICE

21. ANS: B DIF: L1 REF: p. 542 OBJ: 18.1.1

22. ANS: B DIF: L1 REF: p. 543 OBJ: 18.1.1

23. ANS: C DIF: L1 REF: p. 546, p. 547
OBJ: 18.1.2

24. ANS: C DIF: L1 REF: p. 549, p. 550
OBJ: 18.2.1

25. ANS: A DIF: L2 REF: p. 552, p. 553
OBJ: 18.2.2

26. ANS: C DIF: L1 REF: p. 571 OBJ: 18.4.3

27. ANS: C DIF: L2 REF: p. 572 OBJ: 18.4.3

28. ANS: B DIF: L2 REF: p. 572 OBJ: 18.4.4

29. ANS: D DIF: L2 REF: p. 577 OBJ: 18.5.1

30. ANS: D DIF: L2 REF: p. 578 OBJ: 18.5.2

31. ANS: A DIF: L2 REF: p. 592 OBJ: 19.1.2

32. ANS: D DIF: L1 REF: p. 594 OBJ: 19.2.1

33. ANS: D DIF: L1 REF: p. 594 OBJ: 19.2.1

34. ANS: B DIF: L1 REF: p. 597 OBJ: 19.2.2

35. ANS: C DIF: L2 REF: p. 597, p. 598
OBJ: 19.2.2

Sample Exam EP 6 December 2009 Midterm

ep 6 review dec 2009

Matching

Match each item with the correct statement below.
a. oxidation number c. oxidizing agent
b. half-reaction d. reducing agent


____ 1. substance that accepts electrons

____ 2. substance that donates electrons

____ 3. integer related to the number of electrons under an atom's control

____ 4. reaction showing either the reduction or the oxidation reaction

Match each item with the correct statement below.
a. Choose coefficients to make the change in oxidation number equal to 0.
b. Make the electron changes of both half-reactions equal.
c. Assign oxidation numbers to all the atoms.
d. Write the equation showing ions separately.


____ 5. the first step in balancing a redox reaction by the oxidation-number-change method

____ 6. the next-to-the-last step in balancing a redox reaction by the oxidation-number-change method

____ 7. the first step in balancing a redox reaction by the half-reaction method

____ 8. the next-to-the-last step in balancing a redox reaction by the half-reaction method


Match each item with the correct statement below.
a. anode d. half-cell
b. battery e. cathode
c. fuel cell


____ 9. the electrode at which oxidation occurs

____ 10. one part of a voltaic cell in which either oxidation or reduction occurs

____ 11. the electrode at which reduction occurs

____ 12. a group of cells that are connected together

____ 13. a voltaic cell in which a fuel substance undergoes oxidation and from which electrical energy is obtained continuously

Match each item with the correct statement below.
a. electrode d. voltaic cell
b. electrolysis e. dry cell
c. salt bridge


____ 14. a tube containing a conducting solution

____ 15. a conductor in a circuit that carries electrons to or from a substance other than a metal

____ 16. an electrochemical cell that is used to convert chemical energy to electrical energy

____ 17. a voltaic cell in which the electrolyte is a paste

____ 18. a process in which electrical energy is used to bring about a chemical change

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 19. When iron oxide becomes iron, what type of reaction occurs?
a. oxidation c. neutralization
b. reduction d. combination


____ 20. Which statement is true about the following reaction?
S + Cl SCl
(Hint: Chlorine is the more electronegative element.)
a. Sulfur is reduced to SCl . c. Chlorine is oxidized to SCl .
b. Chlorine is reduced to SCl . d. Sulfur is the oxidizing agent.


____ 21. What is defined as the charge an atom would have in a compound if its bonding electrons were assigned to the more electronegative atom?
a. reduction number c. valence
b. oxidation number d. electropositivity


____ 22. Which atom has a change in oxidation number of –3 in the following redox reaction?
K Cr O + H O + S KOH + Cr O + SO
a. K c. O
b. Cr d. S


____ 23. In the following unbalanced reaction, which atom is oxidized?
HNO + HBr NO + Br + H O
a. hydrogen c. oxygen
b. nitrogen d. bromine


____ 24. Which element decreases its oxidation number in the following reaction?
BiCl + Na SO 2NaCl + BiSO
a. bismuth
b. chlorine
c. oxygen
d. No element decreases its oxidation number.


____ 25. Which element decreases its oxidation number in the following reaction?
I + 2KCl 2KI + Cl
a. iodine
b. potassium
c. chlorine
d. No element decreases its oxidation number.


____ 26. What is the oxidation half-reaction for the following unbalanced redox equation?
Cr O + Fe Cr + Fe
a. Cr Cr O c. Fe Fe
b. Fe Fe d. Cr O Cr


____ 27. What is shown by a half-reaction?
a. oxidation or reduction of an element c. decomposition of an ion or molecule
b. neutralization of an ion or molecule d. none of the above


____ 28. What is the ionic form of the following unbalanced equation?
MnO + HNO Mn(NO ) + H O
a. MnO + HNO Mn + NO + H O
b. MnO + H + NO MnNO + H O
c. MnO + H + NO Mn + NO + H O
d. Mn + O + H + NO Mn + NO + H O


____ 29. Identify the pair of metals that lists the more easily oxidized metal on the left.
a. Ag, Na c. Ca, Al
b. Fe, K d. K, Li


____ 30. At which electrode does oxidation occur in a voltaic cell?
a. anode only
b. cathode only
c. both anode and cathode
d. either anode or cathode, depending on the metal


____ 31. Which electrode is labeled as positive in a voltaic cell?
a. anode only c. both anode and cathode
b. cathode only d. neither anode nor cathode


____ 32. What is the electrode in the center of the most common dry cell made of?
a. copper c. iron
b. zinc d. graphite


____ 33. What metal is oxidized in the most common dry cell?
a. copper c. iron
b. zinc d. carbon


____ 34. What is reduced in the most common dry cell?
a. copper c. manganese dioxide
b. zinc d. carbon


____ 35. When a lead storage battery discharges, the concentration of ____.
a. sulfuric acid increases
b. sulfuric acid decreases
c. lead sulfate in the battery decreases
d. lead sulfate in the battery remains constant


____ 36. What is the electrolyte in the hydrogen-oxygen fuel cell?
a. sulfuric acid c. potassium hydroxide
b. hydrochloric acid d. sodium hydroxide


____ 37. What standard reduction electrode has a half-cell potential of 0.00 V?
a. oxygen c. lithium
b. hydrogen d. fluorine


____ 38. At which electrode (anode or cathode) does oxidation occur in an electrolytic cell?
a. anode c. both
b. cathode d. neither


ep 6 review dec 2009
Answer Section

MATCHING

1. ANS: C DIF: L1 REF: p. 634 OBJ: 20.1.1

2. ANS: D DIF: L1 REF: p. 634 OBJ: 20.1.2

3. ANS: A DIF: L1 REF: p. 639 OBJ: 20.2.1

4. ANS: B DIF: L1 REF: p. 650 OBJ: 20.3.1

5. ANS: C DIF: L1 REF: p. 648, p. 649
OBJ: 20.3.1

6. ANS: A DIF: L1 REF: p. 648, p. 649
OBJ: 20.3.1

7. ANS: D DIF: L1 REF: p. 650, p. 651
OBJ: 20.3.2

8. ANS: B DIF: L1 REF: p. 650, p. 651
OBJ: 20.3.2

9. ANS: A DIF: L1 REF: p. 665 OBJ: 21.1.2

10. ANS: D DIF: L1 REF: p. 665 OBJ: 21.1.2

11. ANS: E DIF: L1 REF: p. 665 OBJ: 21.1.2

12. ANS: B DIF: L1 REF: p. 668 OBJ: 21.1.4

13. ANS: C DIF: L1 REF: p. 669 OBJ: 21.1.5

14. ANS: C DIF: L1 REF: p. 665 OBJ: 21.1.2

15. ANS: A DIF: L1 REF: p. 665 OBJ: 21.1.2

16. ANS: D DIF: L1 REF: p. 665 OBJ: 21.1.2

17. ANS: E DIF: L1 REF: p. 667 OBJ: 21.1.3

18. ANS: B DIF: L1 REF: p. 678 OBJ: 21.3.1

MULTIPLE CHOICE

19. ANS: B DIF: L1 REF: p. 632 OBJ: 20.1.1

20. ANS: B DIF: L2 REF: p. 633, p. 634
OBJ: 20.1.2

21. ANS: B DIF: L1 REF: p. 639 OBJ: 20.2.1

22. ANS: B DIF: L1 REF: p. 643 OBJ: 20.2.2

23. ANS: D DIF: L2 REF: p. 643 OBJ: 20.2.2

24. ANS: D DIF: L2 REF: p. 643 OBJ: 20.2.2

25. ANS: A DIF: L2 REF: p. 643 OBJ: 20.2.2

26. ANS: B DIF: L2 REF: p. 650, p. 651
OBJ: 20.3.2

27. ANS: A DIF: L1 REF: p. 650 OBJ: 20.3.2

28. ANS: C DIF: L3 REF: p. 650, p. 651
OBJ: 20.3.2

29. ANS: C DIF: L2 REF: p. 664 OBJ: 21.1.1

30. ANS: A DIF: L1 REF: p. 665 OBJ: 21.1.2

31. ANS: B DIF: L1 REF: p. 665 OBJ: 21.1.2

32. ANS: D DIF: L1 REF: p. 667 OBJ: 21.1.3

33. ANS: B DIF: L1 REF: p. 667 OBJ: 21.1.3

34. ANS: C DIF: L1 REF: p. 667 OBJ: 21.1.3

35. ANS: B DIF: L2 REF: p. 668 OBJ: 21.1.4

36. ANS: C DIF: L1 REF: p. 669 OBJ: 21.1.5

37. ANS: B DIF: L1 REF: p. 672 OBJ: 21.2.2

38. ANS: A DIF: L2 REF: p. 679 OBJ: 21.3.1

notebook check due wednesday last day

if i haven't checked it, that's the drop dead date.

Stroke Information

-- PASSING SOME INFO ALONG!

INFORMATION EVERYONE SHOULD KNOW........................

Blood Clots / Stroke - They Now Have a Fourth Indicator,

the Tongue












I will continue to forward this every time it comes around!



STROKE: Remember the 1st Three Letters.... S. T. R.



STROKE IDENTIFICATION:



During a BBQ, a friend stumbled and took a little fall - she assured everyone that she was fine (they offered to call paramedics) .she said she had just tripped over a brick because of her new shoes.



They got her cleaned up and got her a new plate of food. While she appeared a bit shaken up, Ingrid went about enjoying herself the rest of the evening



Ingrid's husband called later telling everyone that his wife had been taken to the hospital - (at 6:00 pm Ingrid passed away.) She had suffered a stroke at the BBQ. Had they known how to identify the signs of a stroke, perhaps Ingrid would be with us today.
Some don't die. they end up in a helpless, hopeless condition instead.



It only takes a minute to read this...



A neurologist says that if he can get to a stroke vic tim within 3 hours he can totally reverse the effects of a stroke...totally. He said the trick was getting a stroke recognized, diagnosed, and then getting the patient medically cared for within 3 hours, which is tough.



RECOGNIZING A STROKE



Thank God for the sense to remember the '3' steps, STR.
Read and Learn!



Sometimes symptoms of a stroke are difficult to identify. Unfortunately, the lack of awareness spells disaster. The stroke vic tim may suffer severe brain damage when people nearby fail to recognize the symptoms of a stroke.



Now doctors say a bystander can recognize a stroke by asking three simple questions:



S *Ask the individual to SMILE.

T *Ask the person to TALK and SPEAK A SIMPLE SENTENCE (Coherently)

(i.e. It is sunny out today.)

R *Ask him or her to RAISE BOTH ARMS.



If he or she has trouble with ANY ONE of these tasks, call emergency number immediately and describe the symptoms to the dispatcher.



New Sign of a Stroke -------- Stick out Your Tongue



NOTE: Another 'sign' of a stroke is this: Ask the person to 'stick' out his tongue..
If the tongue is 'crooked', if it goes to one side or the other,
that is also an indication of a stroke.



A cardiologist says if everyone who gets this e-mail sends it to 10 people;
you can bet that at least one life will be saved.



I have done my part. Will you?

Debate News

Chula USA will be in January. Interested people please talk to me

Congratulations to AC 1

Putter Jakkrapat 6/1, Jay Montri 6/1, and Gun Satthawut came in second in the First Annual Assumption College Academic Day Challenge losing a close one in the final 5-2. They came away with a beautiful trophy and prize money

FIGHT ON! Go AC

hope to see you at the stadium :D

Bonus video

write a summary in your notebook with 10 definitions from the videob

Debate Video Highlights

Exam Content for Summative

EXAMINATION CONTENT FOR SUMMATIVE AND FINAL TEST

Semester: 2 Academic Year: 2009

Code: SC40102 Subject: Foundation Science (Chemistry) EP-M 4/1-2

No. Prentice Hall Chemistry
Contents / Chapters
Page(s)
Periods Exams
Sum Final
Ch 10 Chemical Quantities
10.1 The Mole: A Measurement of Matter
10.2 Mole-Mass and Mole-Volume Relatoinships
10.3 Percent Composition and Chemical Formulas Pages: 286-319 6 ü


Ch 11 Chemical Reactions
11.1 Describing Chemical Reactions
11.2 Types of Chemical Reactions
11.3 Reactions in Aqueous Solution Pages: 320-351 6 ü


Ch 12 Stoichemistry
12.1 The Arithmetic of Equations
12.2 Chemical Calculations
12.3 Limiting Reagent and Percent Yield Pages: 352-383 6 ü


Ch 13 States of Matter
13.1 The Nature of Gases
13.2 The Nature of Liquids
13.3 The Nature of Solids
13.4 Changes of State Pages: 384-411 6 ü





Ch 14 The Behavior of Gases
14.1 Properties of Gases
14.2 The Gas Laws
14.3 Ideal Gases
14.4 Gases: Mixtures and MOvement Pages: 412-443 6 ü



Mr. Gary Sakuma


EXAMINATION CONTENT FOR SUMMATIVE AND FINAL TEST

Semester: 2 Academic Year: 2009
Code: Sc40222 Subject: Chemistry EP-M 5/1-2
No. Prentice Hall Chemistry
Contents / Chapters
Pages
Periods Exams
Sum Final
Ch 18 Reaction Rates and Equilbrium
18.1 Rates of Reaction
18.2 Reversible Reactions and Equilibrium
18.3 Solubility Equilibrium
18.4 Entropy and Free Energy
18.5 The Progress of Chemical Reactions Pages: 540-585 15 ü

Ch 19 Acids, Bases, and Salts
19.1 Acid-Base Theories
19.2 Hydrogen Ions and Acidity
19.3 Strengths of Acids and Bases
19.4 Neutralization Reactions
10.5 Salts in Solution Pages: 586-629 15 ü











Ch. 20 Oxidation-Reduction Reactions
20.1 The Meaning of Oxidation and Reduction
20.2 Oxidation Numbers
20.3 Balancing Redox Equations Pages: 630-661 12 ü

Ch 21 Electrochemistry
21.1 Electrochemical Cells
21.2 Half-Cells and Cell Potentials
21.3 Electrolytic Cells Pages: 662-691 9 ü

Ch 22 Hydrocarbon Compounds
22.1 Hydrocarbons
22.2 Unsaturated Hydrocarbons
22.3 Isomers
22.4 Hydrocarbon Rings
22.5 Hydrocarbons from the Earth’s Crust
Pages: 692-723 6 ü

Ch 23 Functional Groups
23.1 Introduction to Functional Groups
23.2 Alcohols and Ethers
23.3 Carbonyl Compounds
23.4 Polymerication Pages: 724-761 9

ü


Mr. Gary Sakuma











EXAMINATION CONTENT FOR SUMMATIVE AND FINAL TEST

Semester: 2 Academic Year: 2009

Code: SC40224 Subject: Foundation Science (Chemistry) EP-M 6/1-2

No. Prentice Hall Chemistry
Contents / Chapters
Page(s)
Periods Exams
Sum Final
Ch. 20 Oxidation-Reduction Reactions
20.1 The Meaning of Oxidation and Reduction
20.2 Oxidation Numbers
20.3 Balancing Redox Equations Pages: 630-661 12 ü

Ch 21 Electrochemistry
21.1 Electrochemical Cells
21.2 Half-Cells and Cell Potentials
21.3 Electrolytic Cells Pages: 662-691 9 ü


Ch 10 Chemical Quantities
10.1 The Mole: A Measurement of Matter
10.2 Mole-Mass and Mole-Volume Relatoinships
10.3 Percent Composition and Chemical Formulas Pages: 286-319 6 ü

Ch 11 Chemical Reactions
11.1 Describing Chemical Reactions
11.2 Types of Chemical Reactions
11.3 Reactions in Aqueous Solution Pages: 320-351 6 ü

Ch 12 Stoichemistry
12.1 The Arithmetic of Equations
12.2 Chemical Calculations
12.3 Limiting Reagent and Percent Yield Pages: 352-383 6 ü



Mr. Gary Sakuma

Make up quiz ep 4 week of November 16

1. Give me two mole factors:
4 Fe + 3 O2  2 Fe2O3
2. How many moles of Fe2O3 are produced when 10.0 moles O2 react? Show me your work


full points on this will give you a passing grade on the quiz. only a passing grade.

debate National Coach

Mr. Gary has been assigned to be part of the National Team as a coach. I try to get out, and they drag me in.

Debate resultsd

Debate

the good news: it's a great tournament

Debate Updates

Final round
ac 1--is 2 and 2, ac 2 is 3-1, ac 3 is 2-2, and ac 4 is 2-2, while ac 5 1-3... coming up...

Debate Updates

AC 1 is Vichitpol, Thanakorn, and Suthipat. AC 2 is Sappaya, Tanachai, and Teechayut. AC 3 is Jakkrapat, Sathawut, and Sirivitch.



AC 1 is 2-0 along with AC 2 and AC 3 while AC 4 and AC 5 face an uphill battle tomorrow.

reminder: I will be absent on Monday and Tuesday

Assignments pending

Video of Moles to Atoms

Make up QUIZ EP 4 Balancing Equations

page 327 #3 and 4--

DEBATE--NATIONAL HIGH SCHOOL November 7-10

the debate team will be going to the National High School Championships held at ABAC Bangna

This week in Chem Nov 2, 2009

EP 4 Moles to Grams, moles to volume Quiz Monday Nov 9
EP 5 Common Ion Effect and hw: pages 562 #17, 18 p. 564 #19, 20 page 565 #24-28 write the question. quiz on Monday Nov 9

EP 6 Intro to Electro Chemistry

3rd High School League Challenge First Speaker

3rd High School League Challenge Second Speaker

3rd High School League Challenge Third Speaker

Quizzes: Second Semester

we are planning on having many more quizzes this semester so be prepared

start reading...

ep 4 read ch 10

ep 5 read ch 18.4 and 18.5

ep 6 read ch 20.3

Bring notebooks and textbooks for first day back

just a reminder

Survey

any special topics you want to talk about or learn about within the curriculum?

Bonus Find me sample problems

Get me sample problems for your section

ep 4--hybrid orbitals, naming
ep 5 thermochemistry or le chatelier's principle
ep 6 redox reactions

Retest for EP Chemistry Final

Ep 4 write all the questions and answers in your book
page 208 # 52, 53, 61, 72, 80
page 247 # 42, 53, 59, 67, 71, 78
page 281 #42, 48, 55, 65, 66

EP 5
page 535 #38, 45, 49, 55, 58, 60, 76, 83
page 581 #43, 46, 50, 55

EP 6
page 657 # 26-36, 45, 49ab but not c, 54, 58, 59, 61

EP 6 Exam Results

EP 6/1
High score:
435/440
Woraphon Lilasathapornkit


415/440
Apinut Siripowsuwankul
Jakkrapat Tangsongjareon

Fails:
42277, 42300, 42304, 42396, 46524, 48861, 48862

EP 6/2
440/440
Natee Wongsrisujarit

435/440
Yothin Visanta

Fails:
42346, 42600,

EP 5 Fails and High Score on Exam

High scores
EP 5/1
525/540 Thanatat Pasupa

Second
515/540 Sappaya Surakitjakorn

EP 5/2
540/540 Perfect
Vasin Dumrongprechachan

Second
520/540
Thanatham Julaphatachote


Fails EP 5/1
43179, 43269, 47334, 49538, 49543,

EP 5/2
43075, 43444, 47210, 47212, 47220, 47221, 47237, 47242

High Scores for EP 4

High Score:
EP 4/1 600/625
Chanayut Montrisuksirikul
Ronapart Srisupavanich

second: 590/625
Jiramate Chanturakarnnon

third: 585/625
Yosapol Kriengyuttapoon


EP 4/2
First and HIGHEST in LEVEL 620/625
Techin Udomsinwatana

Second: 610/625

Kitipon Sae-Tang

Third: 605/625
Thanakorn Panichaporn
Most IMPROVED since Midterm

ep 4 the following id number failed the exam

43540, 48021, 50380, 50382, 50399, 50406

make up exam posting tomorrow

Posting fails Wednesday and put up Make ups

If you fail the exam, the make up will be up

San Gabriel Final Round InterVarsity 2009

Assumption Sports Day

Bonus Link Search

Find me a nice powerpoint link--downloadable of

ep 4--stoichemistry

ep 5-- rate law

ep 6--electro chemistry

Good Luck on the exams

Hope the exams went well. Make up exams will be posted next week, if you feel it's necessary you can submit it upon the return from the break. I am not able to tell you your grades until the EP office says it's okay. Have a great vacation

San Gabriel Final Round InterVarsity 2009 4th speaker

San Gabriel Final Round InterVarsity 2009

San Gabriel Final Round InterVarsity 2009

San Gabriel Final Round InterVarsity 2009

UPDATED GRADES EP 4/1 as of 9/26/2009

43513 79.5%
43566 98.0%
0.0%
43819 94.0%
43889 102.6%
0.0%
0.0%
0.0%
47995 98.0%
48000 99.3%
48005 96.0%
48011 66.9%
48021 94.0%
0.0%
0.0%
50377 96.7%
0.0%
50382 100.6%
0.0%
50399 80.8%
50406 98.0%
50483 98.0%
50449 98.6%
50541 99.3%

UPDATED GRADES EP 4/2 as of 9/26/2009

0.0%
43540 68.0%
43544 92.0%
0.0%
43616 98.8%
43661 94.0%
43697 92.0%
43732 94.0%
43817 99.5%
43822 88.0%
43856 58.5%
0.0%
47993 96.8%
47998 100.3%
47999 99.8%
48006 99.5%
0.0%
48016 78.5%
49694 0.0%
50383 85.3%
50385 99.0%
50388 94.3%
50390 81.5%

Ep 4/2 grade as of Sept 2009

0.0%
43540 60.5%
43544 54.5%
0.0%
43616 65.8%
43661 83.5%
43697 71.0%
43732 83.5%
43817 99.5%
43822 47.5%
43856 58.5%
0.0%
47993 96.8%
47998 100.3%
47999 99.8%
48006 88.3%
0.0%
48016 78.5%
49694 0.0%
50383 0.0%
50385 99.0%
50388 94.3%
50390 42.5%

ep 4/1 grades before midterm

43513 79.5%
43566 98.0%
0.0%
43819 94.0%
43889 102.6%
0.0%
0.0%
0.0%
47995 98.0%
48000 99.3%
48005 96.0%
48011 66.9%
48021 94.0%
0.0%
0.0%
50377 96.7%
0.0%
50382 100.6%
0.0%
50399 80.8%
50406 98.0%
50483 98.0%
50449 98.6%
50541 99.3%

so you want to pass the exam

go through the book, read all the pertinent sample problems, go over the problems we did in the homework. read your notes.

good luck

so you want to pass the exam

go through the book, read all the pertinent sample problems, go over the problems we did in the homework. read your notes.

good luck

Sample Exam question

Compare and contrast the following bonds--covalent--polar, nonpolar, coordinate, network, and ionic along with metallic bonds in terms of electronegativity, dissociation energy, shape, and properties.

British Parliamentary Style First Speaker

EP 5 solubility problems

There are going to be solubility problems on the exam.

Multiple Choice TIPS

When you have 4 choices;

1) Read every Choice!!
2) Eliminate wrong choices.
3) If you have to guess, break it down to the last two viable answers if possible.

IF YOU HAVE NO CLUE...guess the same letter--if you have 5 questions, and have no clue, guess the same letter for all 5 because odds are that letter is the one used at least once. If you guess 5 different letters for 5 different questions, you could miss all 5.

HINT: look at your review sheets for any letters that repeat a lot.

ep 4 I can't remember
ep 5 A was in a lot of answers
ep 6 I"m not telling

To get a GREAT grade on my EXAM

EP 4 go through and read all sample problems in the book ch 7-9

EP 5 do the same but chapter 17-18

ep 6 your chapters are ch 20 redox reactions...

good luck 14 days to go

Le Chatelier's Principle Explained again.

One of my smarter students asked me a question about Le Chatelier's principle--and if he's confused, so is everyone else.

Changes in pressure are attributable to changes in volume. The equilibrium concentrations of the products and reactants do not directly depend on the pressure subjected to the system. However, a change in pressure due to a change in volume of the system will shift the equilibrium.

Once again, let us refer to the reaction of nitrogen gas with hydrogen gas to form ammonia:

N2 + 3 H2 ⇌ 2 NH3 ΔH = −92kJ mol-1
4 volumes ⇌ 2 volumes

Note the number of moles of gas on the left hand side, and the number of moles of gas on the right hand side. When the volume of the system is changed, the partial pressures of the gases change. Because there are more moles of gas on the reactant side, this change is more significant in the denominator of the equilibrium constant expression, causing a shift in equilibrium.


Thus, an increase in pressure due to decreasing volume causes the reaction to shift to the side with the fewer moles of gas.[3] A decrease in pressure due to increasing volume causes the reaction to shift to the side with more moles of gas. There is no effect on a reaction where the number of moles of gas is the same on each side of the chemical equation.

when you increase pressure, it favors the side with more moles--because it spreads the pressure out, and thus, causes the reaction to shift to the side with fewer moles....

is that better?! AHAHAH sorry... i got the excerpt above from wikipedia

Bonus question September 17, 2009

EP 4--what is an emulsion plus describe in your own words, hybridization of ethyne and corresponding pi and sigma bonds

EP 5--what is an oxidation/reduction? plus describe in your own words, using collision theory terminology, how reactants cross the activation energy barrier to form a product discussing the activated transition complex.

EP 6--describe why an oxidizing agent is reduced while a reducing agent is oxidized and why you need one for the other?

EP 4 Must READ

know the tables on page 192 and 200--common ions and polyatomic ions

EP 5 Review

ep 5 review

Matching

Match each item with the correct statement below.
a. activated complex d. activation energy
b. reaction rate e. free energy
c. inhibitor


____ 1. the minimum energy colliding particles must have in order to react

____ 2. arrangement of atoms at the peak of an energy barrier

____ 3. the number of atoms, ions, or molecules that react in a given time to form products

____ 4. a substance that interferes with a catalyst

____ 5. energy available to do work

Match each item with the correct statement below.
a. spontaneous reaction d. reaction mechanism
b. entropy e. elementary reaction
c. chemical equilibrium


____ 6. when the forward and reverse reactions take place at the same rate

____ 7. a reaction that releases free energy

____ 8. the measure of disorder

____ 9. Reactants are converted to products in a single step.

____ 10. includes all elementary reactions of a complex reaction

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 11. Activation energy is ____.
a. the heat released in a reaction
b. an energy barrier between reactants and products
c. the energy given off when reactants collide
d. generally very high for a reaction that takes place rapidly


____ 12. Why does a higher concentration make a reaction faster?
a. There are more collisions per second only.
b. Collisions occur with greater energy only.
c. There are more collisions per second and the collisions are of greater energy.
d. There are more collisions per second or the collisions are of greater energy.


____ 13. What happens to a catalyst in a reaction?
a. It is unchanged. c. It is incorporated into the reactants.
b. It is incorporated into the products. d. It evaporates away.


____ 14. Consider the reaction N (g) 3H (g) 2NH (g). What is the effect of decreasing the volume on the contained gases?
a. The reaction shifts toward the product gas.
b. The system reacts by increasing the number of gas molecules.
c. The pressure on the gases decreases momentarily.
d. Ammonia is consumed in the reaction.


____ 15. What happens to a reaction at equilibrium when more reactant is added to the system?
a. The reaction makes more products. c. The reaction is unchanged.
b. The reaction makes more reactants. d. The answer cannot be determined.


____ 16. In an endothermic reaction at equilibrium, what is the effect of raising the temperature?
a. The reaction makes more products. c. The reaction is unchanged.
b. The reaction makes more reactants. d. The answer cannot be determined.


____ 17. What is the effect of adding more water to the following equilibrium reaction?
CO + H O H CO
a. More H CO is produced.
b. CO concentration increases.
c. The equilibrium is pushed in the direction of reactants.
d. There is no effect.


____ 18. In an equilibrium reaction with a K of 1 10 , the ____.
a. reactants are favored c. the products are favored
b. reaction is spontaneous d. reaction is exothermic


____ 19. The K of a reaction is 4 10 . At equilibrium, the ____.
a. reactants are favored
b. products are favored
c. reactants and products are present in equal amounts
d. rate of the forward reaction is much greater than the rate of the reverse reaction


____ 20. The amount of disorder in a system is measured by its ____.
a. activation energy c. equilibrium position
b. entropy d. K


____ 21. Which one of the following systems has the highest entropy?
a. 10 mL of water at 10 C
b. 10 mL of water at 50 C
c. 10 mL of water at 100 C
d. All have the same entropy because all are water.


____ 22. If a system is left to change spontaneously, in what state will it end?
a. the same state in which it began
b. the state with lowest possible energy
c. the state with the maximum disorder
d. the state with the lowest possible energy consistent with the state of maximum disorder


____ 23. The melting of ice at temperatures above 0 C ____.
a. liberates heat c. is not favorable
b. is not spontaneous d. is endothermic


____ 24. What determines whether or not a reaction is spontaneous?
a. change in molar volume and heat change
b. change in enthalpy only
c. enthalpy change and entropy change
d. change in entropy only


____ 25. Which variable is NOT required to calculate the Gibbs free-energy change for a chemical reaction?
a. change in enthalpy c. temperature in kelvins
b. temperature in C d. change in entropy


____ 26. What is the rate law for the following reaction?
A + 2B  C + D
a. rate = k[A][B] c. rate = k[A][B]
b. rate = k[A] [B] d. rate = k[A] [B]


____ 27. What is the order of the following reaction? A + 2B  C + D
a. zero c. second
b. first d. third


____ 28. If a reaction rate decreases by a factor of one-ninth when a reactant concentration is decreased by one-third, what is the order of the reaction with respect to that reactant?
a. fourth c. second
b. third d. first


____ 29. When nitrous oxide is converted to nitrogen and oxygen, what is the term used to describe the oxygen atoms formed?
a. reactants c. activated complexes
b. products d. intermediates


____ 30. For a complex reaction, the reaction progress curve ____.
a. is a flat line c. has several hills and valleys
b. has only one peak d. shows energy versus pressure


Essay

31. Explain the effects of reactant concentration and particle size on the rate of a reaction.

32. What is the effect of a catalyst on the rate of a reaction? Give an example of a catalyst.

ep 5 review
Answer Section

MATCHING

1. ANS: D DIF: L1 REF: p. 543 OBJ: 18.1.1

2. ANS: A DIF: L1 REF: p. 544 OBJ: 18.1.1

3. ANS: B DIF: L1 REF: p. 542 OBJ: 18.1.1

4. ANS: C DIF: L1 REF: p. 547 OBJ: 18.1.2

5. ANS: E DIF: L1 REF: p. 566 OBJ: 18.4.1

6. ANS: C DIF: L1 REF: p. 550 OBJ: 18.2.1

7. ANS: A DIF: L1 REF: p. 567 OBJ: 18.4.1

8. ANS: B DIF: L1 REF: p. 569 OBJ: 18.4.2

9. ANS: E DIF: L1 REF: p. 578 OBJ: 18.5.2

10. ANS: D DIF: L1 REF: p. 578 OBJ: 18.5.2

MULTIPLE CHOICE

11. ANS: B DIF: L1 REF: p. 543 OBJ: 18.1.1

12. ANS: A DIF: L1 REF: p. 545 OBJ: 18.1.2

13. ANS: A DIF: L1 REF: p. 546 OBJ: 18.1.2

14. ANS: A DIF: L2 REF: p. 554 OBJ: 18.2.2

15. ANS: A DIF: L2 REF: p. 552, p. 553
OBJ: 18.2.2

16. ANS: A DIF: L2 REF: p. 554 OBJ: 18.2.2

17. ANS: A DIF: L2 REF: p. 552, p. 553
OBJ: 18.2.2

18. ANS: C DIF: L1 REF: p. 556 OBJ: 18.2.3

19. ANS: A DIF: L1 REF: p. 556 OBJ: 18.2.3

EP 5 Review questions and answers

ep 5 review 2

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.

____ 1. What happens to the energy produced by burning gasoline in a car engine?
a. The energy is lost as heat in the exhaust.
b. The energy is transformed into work to move the car.
c. The energy heats the parts of the engine.
d. all of the above


____ 2. How does a calorie compare to a joule?
a. A calorie is smaller than a joule. c. A calorie is equal to a joule.
b. A calorie is larger than a joule. d. The relationship cannot be determined.


____ 3. Which of the following is NOT a form of energy?
a. light c. heat
b. pressure d. electricity


____ 4. If heat is released by a chemical system, an equal amount of heat will be ____.
a. absorbed by the surroundings c. released by the surroundings
b. absorbed by the universe d. released by the universe


____ 5. In an exothermic reaction, the energy stored in the chemical bonds of the reactants is ____.
a. equal to the energy stored in the bonds of the products
b. greater than the energy stored in the bonds of the products
c. less than the energy stored in the bonds of the products
d. less than the heat released


____ 6. A process that absorbs heat is a(n) ____.
a. endothermic process c. exothermic process
b. polythermic process d. ectothermic process


____ 7. The quantity of heat required to change the temperature of 1 g of a substance by 1 C is defined as ____.
a. a joule c. a calorie
b. specific heat d. density


____ 8. How many joules are in 148 calories? (1 cal = 4.18 J)
a. 6.61 J c. 148 J
b. 35.4 J d. 619 J


____ 9. What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample by 15 C?
a. 0.033 c. 0.99
b. 0.33 d. 1.33


____ 10. The heat capacity of an object depends in part on its ____.
a. mass c. shape
b. enthalpy d. potential energy


____ 11. When 45 g of an alloy, at 25 C, are dropped into 100.0 g of water, the alloy absorbs 956 J of heat. If the final temperature of the alloy is 37 C, what is its specific heat?
a. 0.423 c. 9.88
b. 1.77 d. 48.8


____ 12. How can you describe the specific heat of olive oil if it takes approximately 420 J of heat to raise the temperature of 7 g of olive oil by 30 C?
a. greater than the specific heat of water c. equal to the specific heat of water
b. less than the specific heat of water d. Not enough information is given.


____ 13. In an equilibrium reaction with a K of 1 10 , the ____.
a. reactants are favored c. the products are favored
b. reaction is spontaneous d. reaction is exothermic


Short Answer

14. What is the equilibrium constant for the following reaction?
3A + 2B 2C

15. Calculate the value of K for the following reaction at equilibrium.
2NClO(g) 2NO(g) + Cl (g)
An analysis of the equilibrium mixture in a 1-L flask gives the following results: NClO, 1.6 mol; NO, 6.4 mol; Cl , 0.49 mol

Essay

16. Explain the effects of reactant concentration and particle size on the rate of a reaction.

17. What is the effect of a catalyst on the rate of a reaction? Give an example of a catalyst.

ep 5 review 2
Answer Section

MULTIPLE CHOICE

1. ANS: D DIF: L1 REF: p. 505 OBJ: 17.1.1

2. ANS: B DIF: L1 REF: p. 506 OBJ: 17.1.1

3. ANS: B DIF: L1 REF: p. 505 OBJ: 17.1.1

4. ANS: A DIF: L1 REF: p. 506 OBJ: 17.1.1

5. ANS: B DIF: L2 REF: p. 506 OBJ: 17.1.1

6. ANS: A DIF: L1 REF: p. 506 OBJ: 17.1.2

7. ANS: B DIF: L1 REF: p. 507 OBJ: 17.1.2

8. ANS: D DIF: L1 REF: p. 507 OBJ: 17.1.3

9. ANS: B DIF: L1 REF: p. 509, p. 510
OBJ: 17.1.3

10. ANS: A DIF: L1 REF: p. 508 OBJ: 17.1.3

11. ANS: B DIF: L2 REF: p. 509 OBJ: 17.1.3

12. ANS: B DIF: L2 REF: p. 509, p. 510
OBJ: 17.1.3

13. ANS: C DIF: L1 REF: p. 556 OBJ: 18.2.3

SHORT ANSWER

14. ANS:
Keq =

DIF: L2 REF: p. 556 OBJ: 18.2.3

15. ANS:
K =
= 7.8

DIF: L3 REF: p. 556, p. 557 OBJ: 18.2.3

ESSAY

16. ANS:
A high concentration of reactants increases the reaction rate. This is because more molecules are present to collide each second. A small particle size increases the rate of a reaction. Because there is more surface area for a given mass of particles, more collisions are possible per second.

DIF: L3 REF: p. 545, p. 546 OBJ: 18.1.2

17. ANS:
A catalyst increases the rate of a reaction. A catalyst permits the formation of a less energetic activated complex. Platinum is a catalyst for certain reactions of gases.

DIF: L3 REF: p. 546, p. 547 OBJ: 18.1.2

EP 6 Sample Problem Solution

C +H2SO4--> CO2 +SO2 + H2O


C=0
H=+1 so +2 O4=-8, so S is +6
C=+4 because O2=-4
S=+4 because O2=-4
H2=+2 O=-2

C goes from C=0-->+4 loses electrons Oxidized LEO/reducing agent
S goes from S=+6-->+4 gains electrons reduced GER/oxidizing agent

Sample EP 6 problem explained

Sb+HNO3-->Sb2O5+NO +H2O


sb=0
H=+1, N=+5, 0=(-2) 3


sb2O5=sb=+5, O=(-2)5
N=+2 O=-2

H=+1, O=-2

Sb 0--> +5 loss of electron oxidation, reducing agent
N=+5-->+2 gain electrons reduction, oxidizing agent

EP Sample problems answers

KMnO4 +HCl-->MnCl2+Cl2+H2O+KCl

km is +8 because oxygen is -2 time 4 because there are four of them, so O is -8
H is +1=as rule, so cl=-1 as charge.

Mn becomes +2 because Cl=-1 times two.
Cl2 is 0 because it's a diatomic element by itself
H=+1 while o=-2
K =+1 while Cl=-1


did that help

EP 6 Sample Problems

KMnO4 +HCl-->MnCl2+Cl2+H2O+KCl
Sb+HNO3-->Sb2O5+NO +H2O
C +H2SO4--> CO2 +SO2 + H2O



put the numbers in, I cant make the numbers subscripts on the html.

EP 5 Solubility/Equilbrium Problems from PPT

question 1.
Circle the letters of the terms that complete the sentence correctly. Stresses
that upset the equilibrium of a chemical system include changes in all except b .
a. concentration

c. pressure
d. temperature

question 2

When you add a product to a reversible chemical reaction, the reaction is always pushed in the direction of Reactants
When you remove a product, the reaction is pulled in the direction of products

question 3
What are the exponents in the equilibrium-constant expression?
A. Number of Moles

question 4
At a certain temperature, the equilibrium constant for this reaction is 11.1. Suppose that pure BrCl is placed in a 1-L container and allowed to come to equilibrium. Analysis then shows that the reaction mixture contains 4.00 moles of Cl2. How many moles of Br2 and BrCl are also present in the equilibrium mixture?
2BrCl(g) → Br2(g) + Cl2(g)

Exam Topics by Page Numbers

EP 4 pages 186-268 chapters 7, 8, and 9

EP 5 pages 504-560 ch 17 and 18

EP 6 pages 630-655 ch 20

Exam topics

Format for Exam--approximate 20 multiple choice and 20 problems.

EP 4 Ch 7-9
Naming covalents and ionic compounds
Bonding--covalents, ionic, metallics, and molecular (network solids).
Electron dot structures--polyatomic ions, ionics, and covalents
Hybrid orbitals--VSEPR
ion charge

EP 5 Ch 17-18
Thermochemistry--calorimetry, heat of fusion, heat of vaporization, and change of state
Equilibrium
equilibrium constants
solubility constants

EP 6 ch 20 Reduction/oxidation/
Assigning oxidation numbers
Polyatomic ions oxidation numbers
Balancing reactions

San Gabriel Pix

An awesome tournament!

Assignments for August 31 Week

EP 4 page 236 # 23-28 define vocab on page 237
EP 5 P. 555 #6, p. 559 #11-13, 15
EP 6 worksheet on redox

Debate Results

Congratulations to EP 6/1 Thananan and Sathawut for placing 4th while EP 4/2 Jiramate and EP 6/2 Vichitpol won the Public Speaking Contest

Public Speaking Contest on Monday at ABAC

There will be a Public Speaking contest on Monday at ABAC

THB: PSP's should be legal in Schools the Government Reply speech

the government reply speech

THB: PSP's should be legal in Schools the Opposition Reply

Opp Reply Speech

Chem Bonus: Come to the San Gabriel Debate tournament at Abac HUAMAK

Saturday or Sunday we'll be there competing so come and support them

EP 4 Make up Quiz

In ch 7 do page 207 # 30-40 in your notebook and write the question

Assignments for August 17

EP 4 p. 193 #1-11

EP 5 page 547 1-5, define collision theory and inhibitor

EP 6 page 641 #9, 10 page 643 #11-16

Notebook checks at the end of the week

Reading Assignments for Week August 17, 2009

EP 4 Finish Reading Chapter 7--Ionic Bonding
EP 5 Read Ch 17 Thermochemistry and define any unknown words
EP 6 Read Ch 20 Oxidation and Reduction. Review the rules as we'll be covering that in lecture this week.

Make up exams due MONDAY August 17 4 p.m.

no pressure. but if it's late...well, you get to do a new one.

Short WEEK--retest due May 17

be sure you enjoy yourselves and turn in any late assignments.

Short WEEK--retest due May 17

be sure you enjoy yourselves and turn in any late assignments.

EP 6/2 Midterm Graes

42211 93.4% A+
42220 87.7% A+
42346 52.8% D-
42357 60.4% C-
42416 36.8% F
42502 68.9% C+
42534 70.8% B-
42589 76.4% B
42600 50.0% D-
42625 0.0% F
42722 43.4% F
42738 68.9% C+
42763 76.4% B
42867 80.2% A-
45823 37.7% F
45832 62.3% C-
46526 30.2% F
46547 51.9% D-
46554 67.9% C+
46573 99.1% A+
46634 79.2% B+
48371 34.9% F

EP 5/2 Grades from Midterm

43024 0.0% F
43075 74.2% C
43485 0.0% F
43444 40.4% F
45146 0.0% F
45170 60.7% D-
46583 0.0% F
47206 56.2% F
47210 80.9% B-
47212 46.1% F
47213 0.0% F
47220 55.1% F
47221 60.7% D-
47222 0.0% F
47237 16.9% F
47242 30.3% F
47255 67.4% D+
47256 100.0% A+
47257 0.0% F
47260 0.0% F
47342 85.4% B
43406 0.0% F

EP 4/2 Grades on Midterm

0.0% F
43540 87.5% B+
43544 80.7% B-
0.0% F
43616 93.2% A
43661 94.3% A
43697 90.9% A-
43732 56.8% F
43817 81.8% B-
43822 85.2% B
43856 77.3% C+
0.0% F
47993 86.4% B
47998 97.7% A+
47999 96.6% A
48006 65.9% D
0.0% F
48016 65.9% D
49694 0.0% F
50383 60.2% D-
50385 90.9% A-
50388 77.3% C+
50390 94.3% A

EP 5/1 Grades from Midterm and first Quiz

42969 80.0% A-
43092 75.3% B
43097 77.4% B+
43151 0.0% F
43179 15.1% F
43183 58.1% D+
43269 38.7% F
43397 97.8% A+
0.0% F
47236 69.9% C+
47334 44.6% F
49536 81.7% A-
49536 56.8% D
49542 44.1% F
49542 20.4% F
49549 76.3% B
49550 61.3% C-
49556 86.4% A
49556 0.0% F
49558 50.0% D-
49723 72.0% B-

EP 4/1 Grades

43513 89.2% A+
43566 85.6% A
24.8% F
43819 89.2% A+
43889 98.2% A+
28.1% F
16.9% F
23.6% F
47995 66.1% C
48000 98.5% A+
48005 92.8% A+
48011 73.5% B
48021 61.2% C-
23.8% F
28.3% F
50377 87.7% A+
14.8% F
50382 43.4% F
26.3% F
50399 65.6% C
50406 71.5% B-
50483 77.9% B+
50499 75.5% B
50541 92.3% A+

High Scores for Chemistry Midterm

EP 4/1 Ronapat 430/440 Yosapol Kriengyuttapoom 415/440
EP 4/2 Techin Udomsinwatana 430/440 Warit Jamkachornkiat 425/440

EP 5/1 Sappaya Surakitjakorn 430/445 Thanadej Throngkitpaisan 380/445
EP 5/2 Vasin Dumrongprechachan 445/445 Thanatham Julaphatachote 380/445

EP 6/1 Jakkrapat Tangsongjareon 470/530 Sirivitch Pornpojratanakul 423/530
EP 6/2 Natee Wongsrisujarit 525/530 Yothin Visanta 495/530

Good job to all of the high scores as we made an conscious effort to make the exam much harder than normal as we strive to become better Chemists.

Bonus coming soon

Debate Events for AUGUST

There will be two training sessions for National High School. The first will be August 15 at ABAC Huamak, and the second is August 30th ABAC Huamak. We will be going to both of these events.

The San Gabriel Tournament will be held on August 29th at ABAC Huamak. This tournament is only for newbie debaters.

August 7th is the Chula IV British Parliamentary style debate tournament.

August 28th will be our own 4th High School Debate League tournament held here at AC Bangrak.

If you are interested in going to any of these events, please send me a message or see me.

Assignments for August 2 Week

EP 4: Read Ch 7.3 and 7.4 Naming Ionic Compounds
powerpoint: Naming
EP 5: Read Ch 17.3, and 17.4 Reaction Rates
powerpoint: Reaction Rates
EP 6: Reach Ch 19.4 Titrations and Neutralizing Reactions between Acids/Bases
powerpoint: Titrations and neutralizations reactions
problem sets: TBA
Lab this week depending on availability.

Bonus: Do the Make-up Exam

If you are doing the Make up exam for your level for a bonus, print it out, and staple it in your notebook. write your answers in your notebook.

If you get 80% correct, you will raise your grade approximately 10%. 70%, 6%; 60% 4%; 50% 3%; and less than that...

EP 6 Make up Exam--you must write answers in your notebook

Match each item with the correct statement below.
a. substitution reaction J hydrogenation reaction
b. addition reaction k. dehydrogenation reaction
c. hydration reaction l. asymmetric carbon
d. substituent m. trans configuration
e. structural isomers n. cis configuration
f. geometric isomers o. lignite
g. stereoisomers p. bituminous coal
h. aromatic compound q aliphatic hydrocarbon
i anthracite coal


____ 1. a reaction in which an atom or group of atoms replaces another atom or group of atoms

____ 2. a reaction in which a substance is added at the double or triple bond of an alkene or alkyne

____ 3. a reaction involving the addition of hydrogen to a carbon—carbon double bond to produce an alkane

____ 4. a reaction involving the addition of water to an alkene

____ 5. a reaction involving the loss of hydrogen
____ 6. atom or group of atoms that can take the place of a hydrogen in a parent hydrocarbon molecule

____ 7. compounds that have the same molecular formula, but the atoms are joined in a different order

____ 8. arrangement in which substituted groups are on the same side of a double bond

____ 9. molecules in which atoms are joined in the same order but differ in the arrangements of their atoms in space

____ 10. arrangement in which substituted groups are on opposite sides of a double bond

____ 11. compounds that differ in the orientation of groups around a double bond

____ 12. carbon atom to which four different atoms or groups are attached
__ 13. any straight-chain or branched-chain alkane, alkene, or alkyne

____ 14. any hydrocarbon compound in which a ring has bonding similar to benzene

____ 15. hard coal, having a carbon content of over 80%

____ 16. brown coal, having a carbon content of approximately 50%

____ 17. soft coal, having a carbon content of 70–80%

Multiple Choice ( 5 points each, 25 points total)
Identify the letter of the choice that best completes the statement or answers the question.

____ 18. Aldehydes have the general structure ____________.
a.
c.

b.
d.



____ 19. A ketone has the general structure ____________.
a.
ROR c.

b.
d.





____ 20. Which carbon skeleton contains a carboxyl group?
a.
CCCO c.

b.

d.



____ 21. Which of the following carbon skeletons represents a carboxylic acid?
a.
CCCCCO c.

b.

d.



____ 22. Which carbon skeleton represents an ester?
a.
CCCCCOCC c.

b.
d.



Short Answer ( 20 points each, 80 points total)

23. Write an equation using structural formulas for the reaction of benzene and chlorine.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

24. Write complete, balanced equations for the reaction of 2-pentene and water. Use structural formulas.
____________________________________________________________________________________________________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________





25. What is the expected product when the following compound is oxidized?
CH CH CH CH OH
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

26. Complete the condensation polymerization reaction between two amino acids to form a peptide bond:

______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

Problem ( 20 points each 340 points total)

27.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

28.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

29. Write an equation for the synthesis of
a. 2-chlorobutane from 1-butene and hydrogen chloride
b. bromobenzene from benzene and bromine
______________________________________________________________________________________


______________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


30.
______________________________________________________________________________________


______________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


31.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

32.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

33. Write the structural formula for each of the following compounds.
a. 3-ethyl-2,3-dimethylpentane
b. 3,4-diethylhexane
c. 2,3,4,5-tetramethylnonane
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


34.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

35.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

36.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

37.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

38. Match the description with the appropriate description.


39. Identify the hydrogen ion donor(s) and hydrogen ion acceptor(s) for ionization
of H2SO4 in water. Label the conjugate acidbase pairs.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

40. Classify the following acids as monoprotic, diprotic, or triprotic.
a. HCOOH b. HBr c. H2SO3 d. H3ClO4
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

41. Rank 1M of these compounds in order of increasing hydrogen ion
concentration: weak acid, strong acid, strong base, weak base.
______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

42. Write the expression for the acid dissociation constant of the strong acid
hydrofluoric acid, HF. ______________________________________________________________________________________


________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


43. Describe a polymerization condensation reaction. Give an example.
______________________________________________________________________________________

EP 5 Make up Exam--Write answers in your notebook

you must write the vocab out.

Match each item with the correct statement below.
a. Boyle's law i. Graham's law
b. Charles's law f. Gay-Lussac's law
c. Dalton's law g. ideal gas law

d. effusion h. diffusion
e. compressibility i. partial pressure

f. Henry's law j. supersaturated solution
g. immiscible k concentration
h. saturated solution

____ 1. For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.

____ 2. The volume of a fixed mass of gas is directly proportional to its Kelvin temperature, if the pressure is kept constant.

____ 3. The pressure of a gas is directly proportional to its Kelvin temperature if the volume is kept constant.

____ 4. P  V = n  R  T

____ 5. At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.

____ 6. The rate at which a gas will effuse is inversely proportional to the square root of the gas’s molar mass.

____ 7. a measure of how much the volume of matter decreases under pressure

____ 8. the pressure exerted by a gas in a mixture

____ 9. the escape of gas through a small hole in a container

____ 10. tendency of molecules to move to regions of lower concentration


____ 11. describes liquids that are insoluble in one another

____ 12. solution containing maximum amount of solute

____ 13. solution containing more solute than can theoretically dissolve at a given temperature

____ 14. At a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.

____ 15. measure of the amount of solute dissolved in a specified quantity of solvent

Multiple Choice ( 5 points each, 35 points total)
Identify the letter of the choice that best completes the statement or answers the question.

____ 16. To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.
a. 0.37 atm c. 1.37 atm
b. 0.7 atm d. 2.7 atm


____ 17. What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?
a. 81M c. 12M
b. 0.081M d. 4.0M


____ 18. What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)
a. 1.5M c. 2.1M
b. 2.2M d. 0.0022M


____ 19. The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____.
a. 372 mL c. 248 mL
b. 40.0 mL d. 580 mL


____ 20. What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute = 24 g)
a. 0.67m c. 1.67m
b. 4m d. 0.17m


____ 21. The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is ____. (K = 1.86 C/m; molar mass of water = 18 g)
a. 1.66 C c. 3.33 C
b. –1.66 C d. –3.33 C


____ 22. What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (K = 0.512 C/m; molar mass of water = 18 g)
a. 97 C c. 101.4 C
b. 99.7 C d. 103 C


Short Answer (10 points each, 40 points total)

23. The gaseous product of a reaction is collected in a 25.0-L container at 27 C. The pressure in the container is 300.0 kPa and the gas has a mass of 96.0 g. How many moles of the gas are in the container?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
24. What is the pressure exerted by 32 g of O in a 22.0-L container at 30.0 C?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
25. A mixture of gases at a total pressure of 95 kPa contains N , CO , and O . The partial pressure of the CO is 24 kPa and the partial pressure of the N is 48 kPa. What is the partial pressure of the O ?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
26. Use Graham’s law to calculate how much faster fluorine gas, F , will effuse than chlorine gas, Cl , will. The molar mass of F = 38.0; the molar mass of Cl = 70.9.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
Problem (15 pts each, 235 points total)

27. Use kinetic theory to explain why on a cold autumn morning a camper’s air
mattress may appear to be somewhat flatter than when it was blown up the
afternoon before. Assume no leaks.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
28. A sample of O2 with an initial temperature of 50.0C and a volume of 105 L
is cooled to 25C. The new pressure is 105.4 kPa and the new volume is
55.0 L. What was the initial pressure of the sample?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
29. Is it possible for a balloon with an initial pressure of 200.0 kPa to naturally
expand to four times its initial volume when the temperature remains
constant and atmospheric pressure is 101.3 kPa?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
30. A 35.0-L tank contains 7.00 mol of compressed air. If the pressure inside the
tank is 500.0 kPa, what is the temperature of the compressed gas?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
31. What is the volume occupied by 0.355 mole of nitrogen gas at STP?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
32. A gaseous mixture consisting of nitrogen, argon, and oxygen is in a 3.5-L vessel
at 25C. Determine the number of moles of oxygen if the total pressure is 98.5
kPa and the partial pressures of nitrogen and argon are 22.0 kPa and 50.0 kPa,
respectively.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
33. Compare the effusion rates of O2 (molar mass, 32.0 g/mol) and N2 (molar mass,
28.0 g/mol).
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
34. The volume of a gas at 155.0 kPa changes from 22.0 L to 10.0 L. What is the
new pressure if the temperature remains constant
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
35. 1. In your own words, explain hydrogen bonds.
a. Draw a diagram of the hydrogen bonding between three water molecules.
b. Explain why the density of ice at 0°C is less than the density of liquid water at 0°C.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
36. Which of the following compounds are soluble in water? Which are insoluble?
a. CaCl2
b. N2
c. HBr
d. NH2C2H3O2
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

37. 1. Distinguish colloids and suspensions from solutions by discussing their
properties. Classify each of the following mixtures as a colloid, suspension, or solution.
a. fog
b. milk
c. sodium chloride dissolved in water
d. cornstarch in water
e. potting soil shaken with water
f. soap suds
g. a mixture of sucrose and water
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
38. The solubility of CO2 in water at 1.22 atm is 0.54 g/L. What is the solubility of
carbon dioxide at 1.86 atm? Assume that temperature is constant.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
39. Calculate the molarity of each of the following solutions.
a. 0.40 mol of NaCl dissolved in 1.6 L of solution
b. 20.2 g of potassium nitrate, KNO3, in enough water to make 250.0 mL of
solution
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
40. Calculate the number of grams of solute needed to prepare each of the
following solutions.
a. 2500.0 mL of a 3.0M solution of potassium hydroxide, KOH
b. 2.0 liters of 2.0M nitric acid, HNO3, solution
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
41. What is the concentration in percent by volume, %(v/v), of the following
solutions?
a. 60.0 mL of methanol in a total volume of 500.0 mL
b. 25.0 mL of rubbing alcohol (C3H7OH) diluted to a volume of 200.0 mL
with water
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
42. What is the boiling point of a solution that contains 2 mol of magnesium
chloride in 100.0 g of water?
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
43. Calculate the mole fraction of solute in each of the following solutions.
a. 3.0 moles of lithium bromide, LiBr, dissolved in 6.0 moles of water
b. 125.0 g of potassium nitrate, KNO3, dissolved in 800.0 g of water
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

Essay (20 pts each, 60 pts total)

44. What are some of the differences between a real gas and an ideal gas? ________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

45. Explain on a particle basis how the addition of a solute affects the boiling point, the freezing point, and the vapor pressure of the solvent. ________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________


46. Compare and contrast molarity and molality.
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________