Download CHAPTER 10-11 PRACTICE FOR TEST Answer Section

CHAPTER 10-11 PRACTICE FOR TEST
Matching
Match each itme with the correct statement below.
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
c. chemical equation
b. reactant
d. balanced equation
____ 10. an equation in which each side has the same number of atoms of each element.
____ 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
Match each item with the correct statement below.
a. double-replacement reaction
c. combustion reaction
b. single-replacement reaction
d. decomposition reaction
____ 14. a reaction in which a single compound is broken down into simpler substances
____ 15. a reaction in which oxygen reacts with another substance, often producing heat or light
____ 16. a reaction in which the atoms of one element replace the atoms of a second element in a compound
____ 17. a reaction in which two compounds are broken down into ions in solution then each of the cations rebond to
the opposite anions to form new compounds
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 18. Which of the following elements exists as a diatomic molecule?
a. neon
c. nitrogen
b. lithium
d. sulfur
____ 19. How many atoms are in 0.075 mol of titanium?
a. 1.2 10-25
c. 6.4
b. 2.2 10
d. 4.5
____ 20. How many molecules are in 2.10 mol CO ?
a. 2.53 10 molecules
b. 3.79 10 molecules
c. 3.49
d. 1.26
10
10
10
10
molecules
molecules
____ 21. Which of the following is NOT a true about atomic mass?
a. The atomic mass is 12 g for magnesium.
b. The atomic mass is the mass of one mole of atoms.
c. The atomic mass is found by checking the periodic table.
d. The atomic mass is the number of grams of an element that is numerically equal to the
mass in amu.
____ 22. The mass of a mole of NaCl is the ____.
a. molar mass
b. atomic mass
c. molecular mass
d. gram atomic mass
____ 23. What is the molar mass of (NH ) CO ?
a. 144 g
b. 138 g
c. 96 g
d. 78 g
____ 24. What is the mass in grams of 5.90 mol C H ?
a. 0.0512 g
c. 389 g
b. 19.4 g
d. 673 g
____ 25. 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
____ 26. The molar volume of a gas at STP occupies ____.
a. 22.4 L
c. 1 kilopascal
b. 0 C
d. 12 grams
____ 27. Which combination of temperature and pressure correctly describes standard temperature and pressure, STP?
a. 0 C and 101 kPa
c. 0 C and 22.4 kPa
b. 1 C and 0 kPa
d. 100 C and 100 kPa
____ 28. The molar mass of a substance can be calculated from its density alone, if that substance is a(n) ____.
a. element
c. liquid
b. gas at STP
d. solid
____ 29. 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
____ 30. If the density of an unknown gas Z is 4.50 g/L at STP, what is the molar mass of gas Z?
a. 0.201 g/mol
c. 26.9 g/mol
b. 5.00 g/mol
d. 101 g/mol
____ 31. If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the percent
composition of Hg in the compound?
a. 28.5%
c. 71.5%
b. 39.9%
d. 60.1%
____ 32. Which of the following compounds has the lowest percent gold content by weight?
a. AuOH
c. AuCl
b. Au(OH)
d. AuI
____ 33. The lowest whole-number ratio of the elements in a compound is called the ____.
a. empirical formula
c. binary formula
b. molecular formula
d. representative formula
____ 34. What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?
a. SO
c. SO
b. SO
d. S O
____ 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. Chemical equations ____.
a. describe chemical reactions
b. show how to write chemical formulas
c. give directions for naming chemical compounds
d. describe only biological changes
____ 38. In the chemical equation H O (aq)  H O(l) O (g), the
a. catalyst
c. product
b. solid
d. reactant
is a ____.
____ 39. If you rewrite the following word equation as a balanced chemical equation, what will the coefficient and
symbol for fluorine be?
nitrogen trifluoride
a. 6F
b. F
nitrogen
fluorine
c. 6F
d. 3F
____ 40. Chemical equations must be balanced to satisfy ____.
a. the law of definite proportions
c. the law of conservation of mass
b. the law of multiple proportions
d. Avogadro’s principle
____ 41. When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed.
The balanced equation for this reaction is ____.
a. KH BaCl
KCl BaH
c. 2KOH BaCl
2KCl Ba(OH)
b. KOH BaCl
KCl BaOH
d. KOH BaCl
KCl
BaOH
____ 42. In a combustion reaction, one of the reactants is ____.
a. hydrogen
c. oxygen
b. nitrogen
d. a metal
____ 43. What are the correct formulas and coefficients for the products of the following double-replacement reaction?
RbOH H PO

a. Rb(PO )
c. Rb PO
H O
3H O
b. RbPO
d. H Rb PO OH
2H O
____ 44. A double-replacement reaction takes place when aqueous Na CO reacts with aqueous Sn(NO ) . You
would expect one of the products of this reaction to be ____.
a. NaNO
c. Sn(CO )
b. NaSn
d. CNO
____ 45. What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide?
a. Br
c. Br NaI
NaI
NaBr
I
NaBrI
b. Br
d. Br NaI
2NaI
2NaBr I
NaBr I
Short Answer
46. What is the percent by mass of hydrogen in aspirin, C H O ?
47. Calculate the molecular formulas of the compounds having the following empirical formulas and molar
masses: C H , 58 g/mol; CH, 78 g/mol.
48. Balance the following equation.
Au O
Au O
49. Balance the following equation.
Na PO
ZnSO
Na SO
Zn (PO )
50. Write a balanced net ionic equation for the following reaction.
H PO (aq) Ca(OH) (aq)
Ca (PO ) (aq) H O(l)
Essay
51. Predict the precipitate that forms when aqueous solutions of silver nitrate and potassium chloride react to
form products in a double-replacement reaction. Include a discussion of how to determine the products and
which of them is the solid precipitate. Be sure to include the whole balanced equation with your
discussion.
CHAPTER 10-11 PRACTICE FOR TEST
Answer Section
MATCHING
1. ANS: C
PTS: 1
DIF: L1
REF: p. 294
OBJ: 10.1.3 Distiguish between the atomic mass of an element and its molar mass.
STA: Ch.1.a
2. ANS: B
PTS: 1
DIF: L1
REF: p. 294 | p. 295
OBJ: 10.1.3 Distiguish between the atomic mass of an element and its molar mass. | 10.1.4 Describe how
the mass of a mole of a compound is calculated.
STA: Ch.3.d
3. ANS: A
PTS: 1
DIF: L1
REF: p. 300
OBJ: 10.2.2 Identify the volume of a quantity of gas at STP. STA: Ch.4
4. ANS: C
PTS: 1
DIF: L1
REF: p. 290
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: Ch.3.b
5. ANS: A
PTS: 1
DIF: L1
REF: p. 290
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: Ch.3.b
6. ANS: B
PTS: 1
DIF: L1
REF: p. 290
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance, and
moles to mass.
STA: Ch.3.b | Ch.3.c
7. ANS: E
PTS: 1
DIF: L1
REF: p. 300
OBJ: 10.2.2 Identify the volume of a quantity of gas at STP. STA: Ch.4.d
8. ANS: D
PTS: 1
DIF: L1
REF: p. 305
OBJ: 10.3.1 Describe how to calculate the percent by mass of an element in a compound.
STA: Ch.5
9. ANS: F
PTS: 1
DIF: L1
REF: p. 309
OBJ: 10.3.2 Interpret an empirical formula.
STA: Ch.3
10. ANS:
OBJ:
11. ANS:
OBJ:
12. ANS:
OBJ:
13. ANS:
OBJ:
STA:
D
11.1.2
A
11.1.2
B
11.1.2
C
11.1.3
Ch.3.a
PTS: 1
DIF: L1
REF: p. 323
Describe how to write a skeleton equation
STA: Ch.3.a
PTS: 1
DIF: L1
REF: p. 323
Describe how to write a skeleton equation
STA: Ch.3.e
PTS: 1
DIF: L1
REF: p. 323
Describe how to write a skeleton equation
STA: Ch.3.e
PTS: 1
DIF: L1
REF: p. 323
Describe the steps for writing a balanced chemical equation.
14. ANS:
OBJ:
15. ANS:
OBJ:
16. ANS:
OBJ:
17. ANS:
D
PTS: 1
DIF: L1
11.2.1 Describe the five general types of reactions.
C
PTS: 1
DIF: L1
11.2.1 Describe the five general types of reactions.
B
PTS: 1
DIF: L1
11.2.1 Describe the five general types of reactions.
A
PTS: 1
DIF: L1
REF: p. 332
REF: p. 336 | p. 337
STA: Ch.3.g | Ch.7.b
REF: p. 333
REF: p. 333
OBJ: 11.2.2 Predict the products of the five general types of reactions.
MULTIPLE CHOICE
18. ANS: C
PTS: 1
DIF: L1
REF: p. 290
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: Ch.1
19. ANS: D
PTS: 1
DIF: L2
REF: p. 291 | p. 292
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: Ch.3.d
20. ANS: D
PTS: 1
DIF: L2
REF: p. 291 | p. 292
OBJ: 10.1.2 Relate Avogadro’s number to a mole of a substance.
STA: Ch.3.d
21. ANS: A
PTS: 1
DIF: L2
REF: p. 294
OBJ: 10.1.3 Distiguish between the atomic mass of an element and its molar mass.
STA: Ch.3
22. ANS: A
PTS: 1
DIF: L1
REF: p. 295
OBJ: 10.1.4 Describe how the mass of a mole of a compound is calculated.
STA: Ch.3
23. ANS: C
PTS: 1
DIF: L2
REF: p. 295 | p. 296
OBJ: 10.1.4 Describe how the mass of a mole of a compound is calculated.
STA: Ch.3
24. ANS: D
PTS: 1
DIF: L2
REF: p. 297 | p. 298
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance, and
moles to mass.
STA: Ch.3
25. ANS: C
PTS: 1
DIF: L2
REF: p. 299
OBJ: 10.2.1 Describe how to convert the mass of a substance to the number of moles of a substance, and
moles to mass.
STA: Ch.3
26. ANS: A
PTS: 1
DIF: L1
REF: p. 300
OBJ: 10.2.2 Identify the volume of a quantity of gas at STP. STA: Ch.4.c
27. ANS: A
PTS: 1
DIF: L1
REF: p. 300
OBJ: 10.2.2 Identify the volume of a quantity of gas at STP. STA: Ch.4.d
28. ANS: B
PTS: 1
DIF: L1
REF: p. 302
OBJ: 10.2.2 Identify the volume of a quantity of gas at STP. STA: Ch.4.d
29. ANS: B
PTS: 1
DIF: L2
REF: p. 301
OBJ: 10.2.2 Identify the volume of a quantity of gas at STP. STA: Ch.4.h
30. ANS: D
PTS: 1
DIF: L2
REF: p. 302
OBJ: 10.2.2 Identify the volume of a quantity of gas at STP. STA: Ch.4.h
31. ANS: C
PTS: 1
DIF: L2
REF: p. 305 | p. 306
OBJ: 10.3.1 Describe how to calculate the percent by mass of an element in a compound.
STA: Ch.3
32. ANS: D
PTS: 1
DIF: L3
REF: p. 307
OBJ: 10.3.1 Describe how to calculate the percent by mass of an element in a compound.
STA: Ch.3
33. ANS: A
PTS: 1
DIF: L1
REF: p. 309
OBJ: 10.3.2 Interpret an empirical formula.
STA: Ch.3
34. ANS: C
PTS: 1
DIF: L2
REF: p. 310
OBJ: 10.3.2 Interpret an empirical formula.
STA: Ch.3
35. ANS: D
PTS: 1
DIF: L3
REF: p. 310
OBJ:
36. ANS:
OBJ:
STA:
37. ANS:
OBJ:
38. ANS:
OBJ:
39. ANS:
OBJ:
STA:
40. ANS:
OBJ:
41. ANS:
OBJ:
STA:
42. ANS:
OBJ:
43. ANS:
OBJ:
44. ANS:
OBJ:
45. ANS:
OBJ:
STA:
10.3.2 Interpret an empirical formula.
STA: Ch.3
D
PTS: 1
DIF: L1
REF: p. 311
10.3.3 Distinguish between empirical and molecular formulas.
Ch.3
A
PTS: 1
DIF: L1
REF: p. 323
11.1.2 Describe how to write a skeleton equation
STA: Ch.3.a
C
PTS: 1
DIF: L1
REF: p. 323
11.1.2 Describe how to write a skeleton equation
STA: Ch.3.a
D
PTS: 1
DIF: L1
REF: p. 324 | p. 325
11.1.3 Describe the steps for writing a balanced chemical equation.
Ch.3.a | Ch.3.e
C
PTS: 1
DIF: L1
REF: p. 325
11.1.3 Describe the steps for writing a balanced chemical equation.
C
PTS: 1
DIF: L2
REF: p. 327
11.1.3 Describe the steps for writing a balanced chemical equation.
Ch.3.a | Ch.3.e
C
PTS: 1
DIF: L1
REF: p. 336
11.2.1 Describe the five general types of reactions.
STA: Ch.3.g
C
PTS: 1
DIF: L2
REF: p. 334 | p. 335
11.2.1 Describe the five general types of reactions.
STA: Ch.3.a | Ch.3.e
A
PTS: 1
DIF: L2
REF: p. 334 | p. 335
11.2.1 Describe the five general types of reactions.
STA: Ch.3.a | Ch.3.e
B
PTS: 1
DIF: L2
REF: p. 333 | p. 334
11.2.2 Predict the products of the five general types of reactions.
Ch.3.a | Ch.3.e
SHORT ANSWER
46. ANS:
8.00 g H /180 g C H O
100% = 4.44% H
PTS: 1
DIF: L3
REF: p. 307
OBJ: 10.3.1 Describe how to calculate the percent by mass of an element in a compound.
STA: Ch.3
47. ANS:
58 g/mol/29 g/efm = 2 efm/mol; C H
78 g/mol/13 g/efm = 6 efm/mol; C H
PTS: 1
DIF: L3
REF: p. 312
OBJ: 10.3.3 Distinguish between empirical and molecular formulas.
STA: Ch.3
48. ANS:
2Au O
4Au 3O
PTS: 1
DIF: L3
REF: p. 327
OBJ: 11.1.3 Describe the steps for writing a balanced chemical equation.
STA: Ch.3.e
49. ANS:
2Na PO
3ZnSO
3Na SO
Zn (PO )
PTS: 1
DIF: L3
REF: p. 327
OBJ: 11.1.3 Describe the steps for writing a balanced chemical equation.
STA: Ch.3.e
50. ANS:
H (aq) OH (aq)
H O(l)
PTS: 1
DIF: L3
REF: p. 342 | p. 343
OBJ: 11.3.1 Describe the information found in a net ionic equation.
STA: Ch.3.a | Ch.3.e
ESSAY
51. ANS:
Because the reaction is a double-replacement type, cations are exchanged among compounds during the
reaction. The first step is to write the equation in skeleton form:
AgNO + KCl
AgCl + KNO
Inspection of this equation shows that the insoluble precipitate silver chloride forms in an aqueous solution of
potassium nitrate. The relative amounts of elements are the same on either side of the equation, so the
complete equation is:
AgNO (aq) + KCl(aq)
AgCl(s) + KNO (aq) (balanced)
PTS: 1
DIF: L3
REF: p. 334 | p. 335
OBJ: 11.3.2 Predict the formation of a precipitate in a double-replacement reaction.
STA: Ch.3.a | Ch.3.e