sample test ep 4

review sheetep 4

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. How many moles of tungsten atoms are in 4.8 10 atoms of tungsten?
a. 8.0 10 moles c. 1.3 10 moles
b. 8.0 10 moles d. 1.3 10 moles


____ 28. How many molecules are in 2.10 mol CO ?
a. 2.53 10 molecules c. 3.49 10 molecules
b. 3.79 10 molecules d. 1.26 10 molecules


____ 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 number of moles in 432 g Ba(NO ) ?
a. 0.237 mol c. 1.65 mol
b. 0.605 mol d. 3.66 mol


____ 31. What is the volume, in liters, of 0.500 mol of C H gas at STP?
a. 0.0335 L c. 16.8 L
b. 11.2 L d. 22.4 L


____ 32. What is the density at STP of the gas sulfur hexafluoride, SF ?
a. 0.153 g/L c. 3270 g/L
b. 6.52 g/L d. 3.93 10 g/L


____ 33. What is the percent composition of chromium in BaCrO ?
a. 4.87% c. 20.5%
b. 9.47% d. 25.2%


____ 34. Which of the following compounds have the same empirical formula?
a. CO and SO c. C H and C H
b. C H and C H d. C H and C H


____ 35. What are the coefficients that will balance the skeleton equation below?
AlCl + NaOH Al(OH) NaCl
a. 1, 3, 1, 3 c. 1, 1, 1, 3
b. 3, 1, 3, 1 d. 1, 3, 3, 1


____ 36. What are the coefficients that will balance the skeleton equation below?
N + H NH
a. 1, 1, 2 c. 3, 1, 2
b. 1, 3, 3 d. 1, 3, 2


____ 37. When the equation KClO (s) KCl(s) + O (g) is balanced, the coefficient of KClO3 is ____.
a. 1 c. 3
b. 2 d. 4


____ 38. 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


____ 39. When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction?
4Fe(s) + 3O (g)  2Fe2O (s)
a. 1.2 mol c. 2.4 mol
b. 1.8 mol d. 3.2 mol


____ 40. At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water?
2H (g) + O (g)  2H O(g)
a. 1.8 L c. 2.0 L
b. 3.6 L d. 2.4 L


____ 41. The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO is formed?

a. 1.00 g c. 2.88 g
b. 2.00 g d. 32.0 g


review sheet
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: B DIF: L2 REF: p. 290, p. 291
OBJ: 10.1.2

28. ANS: D 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. 299 OBJ: 10.2.1

31. ANS: B DIF: L2 REF: p. 301 OBJ: 10.2.2

32. ANS: B DIF: L2 REF: p. 302 OBJ: 10.2.2

33. ANS: C DIF: L2 REF: p. 307 OBJ: 10.3.1

34. ANS: B DIF: L1 REF: p. 309 OBJ: 10.3.2

35. ANS: A DIF: L1 REF: p. 324, p. 325
OBJ: 11.1.3

36. ANS: D DIF: L1 REF: p. 324, p. 325
OBJ: 11.1.3

37. ANS: B DIF: L1 REF: p. 327 OBJ: 11.1.3

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

39. ANS: B DIF: L2 REF: p. 359, p. 360
OBJ: 12.2.1

40. ANS: A DIF: L1 REF: p. 363, p. 364, p. 365, p. 366
OBJ: 12.2.2

41. ANS: B DIF: L2 REF: p. 360, p. 361, p. 362
OBJ: 12.2.2