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