When the following equation is balanced, the coefficients are ________.

C8H18 + O2 → CO2 + H2O

A) 2, 3, 4, 4

B) 1, 4, 8, 9

C) 2, 12, 8, 9

D) 4, 4,
32, 36

E) 2, 25, 16, 18

E

Of the reactions below, which one is not a combination
reaction?

A) C + O2 → CO2

B) 2Mg + O2 → 2MgO

C) 2N2 +
3H2 → 2NH3

D) CaO + H2O → Ca(OH)2

E) 2CH4 + 4O2 → 2CO2 + 4H2O

E

When a hydrocarbon burns in air, what component of air
reacts?

A) oxygen

B) nitrogen

C) carbon dioxide

D)
water

E) argon

A

When a hydrocarbon burns in air, a component produced is
________.

A) oxygen

B) nitrogen

C) carbon

D)
water

E) argon

D

Of the reactions below, which one is a decomposition
reaction?

A) NH4Cl → NH3 + HCl

B) 2Mg + O2 → 2MgO

C)
2N2 + 3H2 → 2NH3

D) 2CH4 + 4O2 → 2CO2 + 4H2O

E) Cd(NO3)2 +
Na2S → CdS + 2NaNO3

A

Which one of the following substances is the product of this combination reaction?

Al (s) + I2(s) → ________

A) AlI2

B) AlI

C) AlI3

D) Al2I3

E) Al3I2

C

Which one of the following is not true concerning automotive air
bags?

A) They are inflated as a result of a decomposition
reaction.

B) They are loaded with sodium azide initially.

C)
The gas used for inflating them is oxygen.

D) The two products of
the decomposition reaction are sodium and nitrogen.

E) A gas is
produced when the air bag activates.

C

The reaction used to inflate automobile airbags ________.

A)
produces sodium gas

B) is a combustion reaction

C) is a
combination reaction

D) violates the law of conservation of
mass

E) is a decomposition reaction

E

Which of the following are combination reactions?

1) CH4 (g) +
O2 (g) → CO2 (g) + H2O (l)

2) CaO (s) + CO2 (g) → CaCO3
(s)

3) Mg (s) + O2(g) → MgO (s)

4) PbCO3 (s) → PbO (s) +
CO2 (g)

A) 1, 2, and 3

B) 2 and 3

C) 1, 2, 3, and
4

D) 4 only

E) 2, 3, and 4

B

Which of the following are combustion reactions?

1) CH4 (g) +
O2 (g) → CO2 (g) + H2O (l)

2) CaO (s) + CO2 (g) → CaCO3
(s)

3) PbCO3 (s) → PbO (s) + CO2 (g)

4) CH3OH (l) + O2 (g) →
CO2 (g) + H2O (l)

A) 1 and 4

B) 1, 2, 3, and 4

C) 1, 3,
and 4

D) 2, 3, and 4

E) 3 and 4

A

Which of the following are decomposition reactions?

1) CH4 (g)
+ O2 (g) → CO2 (g) + H2O (l)

2) CaO (s) + CO2 (g) → CaCO3
(s)

3) Mg (s) + O2(g) → MgO (s)

4) PbCO3 (s) → PbO (s) +
CO2 (g)

A) 1, 2, and 3

B) 4 only

C) 1, 2, 3, and
4

D) 2 and 3

E) 2, 3, and 4

B

The formula of nitrobenzene is C6H5NO2. The molecular weight of this
compound is ________ amu.

A) 107.11

B) 43.03

C)
109.10

D) 123.11

E) 3.06

D

The formula weight of potassium dichromate (K2Cr2O7) is ________
amu.

A) 107.09

B) 255.08

C) 242.18

D)
294.18

E) 333.08

D

The formula weight of silver chromate (Ag2CrO4) is ________
amu.

A) 159.87

B) 223.87

C) 331.73

D)
339.86

E) 175.87

C

The formula weight of ammonium sulfate ((NH4)2SO4), rounded to the
nearest integer, is ________ amu.

A) 100

B) 118

C)
116

D) 132

E) 264

D

The molecular weight of the acetic acid (CH3CO2H), rounded to the
nearest integer, is ________ amu.

A) 60

B) 48

C)
44

D) 32

A

The formula weight of a substance is ________.

A) identical to
the molar mass

B) the same as the percent by mass weight

C)
determined by combustion analysis

D) the sum of the atomic
weights of each atom in its chemical formula

E) the weight of a
sample of the substance

D

The formula weight of calcium nitrate (Ca(NO3)2), rounded to one
decimal place, is ________ amu.

A) 102.1

B) 164.0

C)
204.2

D) 150.1

E) 116.1

B

What is the formula weight of magnesium fluoride (MgF2)?

A)
86.6

B) 43.3

C) 62.3

D) 67.6

E) 92.9

C

What is the formula weight of lead iodide (PbI2)?

A)
334.1

B) 168.7

C) 295.6

D) 461.0

E) 668.2

D

The mass % of C in methane (CH4) is ________.

A) 25.13

B)
133.6

C) 74.87

D) 92.26

E) 7.743

C

The mass % of H in methane (CH4) is ________.

A) 25.13

B)
4.032

C) 74.87

D) 92.26

E) 7.743

A

The mass % of F in the binary compound KrF2 is ________.

A)
18.48

B) 45.38

C) 68.80

D) 81.52

E) 31.20

E

Calculate the percentage by mass of nitrogen in PtCl2(NH3)2.

A)
4.67

B) 9.34

C) 9.90

D) 4.95

E) 12.67

B

Calculate the percentage by mass of lead in Pb(NO3)2.

A)
38.6

B) 44.5

C) 62.6

D) 65.3

E) 71.2

C

Calculate the percentage by mass of carbon in CO2.

A)
27.29

B) 75.10

C) 73.05

D) 72.71

E) 37.53

A

Calculate the percentage by mass of oxygen in Pb(NO3)2.

A)
9.7

B) 14.5

C) 19.3

D) 29.0

E) 33.4

D

Calculate the percentage by mass of ammonia in cisplatin,
PtCl2(NH3)2.

A) 5.68

B) 11.35

C) 4.67

D)
12.53

E) 18.09

B

Calculate the percentage by mass of hydrogen in PtCl2(NH3)2.

A)
1.558

B) 1.008

C) 0.672

D) 0.034

E) 2.016

E

Which of the following contains the largest number of atoms in
mole?

A) S8

B) C4H10

C) Al2(SO4)3

D)
Na3PO4

E) Cl2

C

One mole of ________ contains the smallest number of atoms.

A)
S8

B) C10H8

C) Al2(SO4)3

D) Na3PO4

E) NaCl

E

One million argon atoms is ________ mol (rounded to two significant
figures) of argon atoms.

A) 3.0

B) 1.7 × 10^{-18}

C) 6.0 × 10^{23}

D) 1.0 × 10^{-6}

E) 1.0 × 10^{+6}

B

How many molecules of CH4 are in 48.2 g of this compound?

A)
5.00 × 10^{-24}

B) 2.00 × 10^{23}

C)
4.64 × 10^{26}

D) 1.81 × 10^{24}

E) 4.00

D

A 30.5 gram sample of glucose (C6H12O6) contains ________ mol of
glucose.

A) 0.424

B) 0.169

C) 5.90

D) 2.36

E) 0.136

B

A sample of CH2F2 with a mass of 19 g contains ________ atoms of
F.

A) 2.2 × 10^{23}

B) 38

C) 3.3 ×
10^{24}

D) 4.4 × 10^{23}

E) 9.5

D

A sample of CH4O with a mass of 32.0 g contains ________ molecules of
CH4O.

A) 5.32 × 10^{-23}

B) 1.00

C) 1.88 ×
10^{22}

D) 6.02 × 10^{23}

E) 32.0

D

How many atoms of nitrogen are in 10 g of NH4NO3?

A) 3.5

B)
1.5 × 10^{23}

C) 3.0 × 10^{23}

D)
1.8

E) 2

B

Gaseous neon has a density of 0.900 g/L at standard conditions. How
many neon atoms are in 1.00 L of neon gas at standard
conditions?

A) 5.42 × 10^{23}

B) 1.35 ×
10^{25}

C) 7.41 × 10^{-26}

D) 2.69 ×
10^{22}

E) 6.02 × 10^{23}

D

How many oxygen atoms are contained in 2.74 g of Al2(SO4)3?

A)
12

B) 6.02 × 10^{23}

C) 7.22 × 10^{24}

D) 5.79 × 10^{22}

E) 8.01 × 10^{-3}

D

What is the total number of atoms in 0.139 mol of
Fe(OH_{2})_{6} ^{3+}?

A) 19.0

B)
1.59 × 10^{24}

C) 8.37 × 102^{2}

D)
2.64

E) 1.84 × 10^{24}

B

How many sulfur dioxide molecules are there in 1.80 mol of sulfur
dioxide?

A) 1.08 × 10^{23}

B) 6.02 ×
10^{24}

C) 1.80 × 10^{24}

D) 1.08 ×
10^{24}

E) 6.02 × 10^{23}

D

How many sulfur dioxide molecules are there in 0.180 mol of sulfur
dioxide?

A) 1.80 × 10^{23}

B) 6.02 ×
10^{24}

C) 6.02 × 10^{23}

D) 1.08 ×
10^{24}

E) 1.08 × 10^{23}

E

How many carbon atoms are there in 52.06 g of carbon dioxide?

A)
5.206 × 10^{24}

B) 3.134 × 10^{25}

C)
7.122 × 10^{23}

D) 8.648 × 10^{-23}

E)
1.424 × 10^{24}

C

How many oxygen atoms are there in 52.06 g of carbon dioxide?

A)
1.424 × 10^{24}

B) 6.022 × 10^{23}

C)
7.122 × 10^{23}

D) 5.088 × 10^{23}

E)
1.018 × 10^{24}

A

How many moles of sodium carbonate contain 1.773 × 10^{17}
carbon atoms?

A) 5.890 × 10^{-7}

B) 2.945 ×
10^{-7}

C) 1.473 × 10^{-7}

D) 8.836 ×
10-^{7}

E) 9.817 × 10^{-8}

B

How many grams of sodium carbonate contain 1.773 × 10^{17}
carbon atoms?

A) 3.121 × 10^{-5}

B) 1.011 ×
10^{-5}

C) 1.517 × 10^{-5}

D) 9.100 ×
10^{-5}

E) 6.066 × 10^{-5}

A

The compound responsible for the characteristic smell of garlic is
allicin, C6H10OS2. What is the mass (g) of 1.00 mol of
allicin?

A) 34

B) 162

C) 86

D) 61

E) 19

B

The molecular formula of aspartame, the generic name of NutraSweet®,
is C14H18N2O5. What is the mass (g) of 1.00 mol of aspartame?

A)
24

B) 156

C) 294

D) 43

E) 39

C

There are ________ oxygen atoms in 30 molecules of
C20H42S3O2.

A) 6.0 × 10^{23}

B) 1.8 ×
10^{25}

C) 3.6 × 10^{25}

D) 1.2 ×
10^{24}

E) 60

E

A nitrogen oxide is 63.65% by mass nitrogen. The molecular formula
could be ________.

A) NO

B) NO2

C) N2O

D)
N2O4

E) either NO2 or N2O4

C

A sulfur oxide is 50.0% by mass sulfur. This molecular formula could
be ________.

A) SO

B) SO2

C) S2O

D) S2O4

E)
either SO2 or S2O4

E

Which hydrocarbon pair below has identical mass percentage of
C?

A) C3H4 and C3H6

B) C2H4 and C3H4

C) C2H4 and
C4H2

D) C2H4 and C3H6

E) none of the above

D

Propane (C3H8) reacts with oxygen in the air to produce carbon
dioxide and water. In a particular experiment, 38.0 grams of carbon
dioxide are produced from the reaction of 22.05 grams of propane with
excess oxygen. What is the % yield in this reaction?

A)
38.0

B) 57.6

C) 66.0

D) 86.4

E) 94.5

B

When the following equation is balanced, the coefficients are ________.

NH3 (g) + O2 (g) → NO2 (g) + H2O (g)

A) 1, 1, 1, 1

B) 4, 7, 4, 6

C) 2, 3, 2, 3

D) 1, 3,
1, 2

E) 4, 3, 4, 3

Answer: B

B

When the following equation is balanced, the coefficients are ________.

Al(NO3)3 + Na2S → Al2S3 + NaNO3

A) 2, 3, 1, 6

B) 2, 1, 3, 2

C) 1, 1, 1, 1

D) 4, 6,
3, 2

E) 2, 3, 2, 3

A

When the following equation is balanced, the coefficient of H2 is ________.

K (s) + H2O (l) → KOH (aq) + H2 (g)

A) 1

B) 2

C) 3

D) 4

E) 5

A

When the following equation is balanced, the coefficient of Al is ________.

Al (s) + H2O (l) → Al(OH (s) + H2 (g)

A) 1

B) 2

C) 3

D) 5

E) 4

B

When the following equation is balanced, the coefficient of H2O is ________.

Ca (s) + H2O (l) → Ca(OH)2 (aq) + H2 (g)

A) 1

B) 2

C) 3

D) 5

E) 4

B

When the following equation is balanced, the coefficient of Al2O3 is ________.

Al2O3 (s) + C (s) + Cl2 (g) → AlCl3 (s) + CO (g)

A) 1

B) 2

C) 3

D) 4

E) 5

A

When the following equation is balanced, the coefficient of H2S is ________.

FeCl3 (aq) + H2S (g) → Fe2S3 (s) + HCl (aq)

A) 1

B) 2

C) 3

D) 5

E) 4

C

When the following equation is balanced, the coefficient of HCl is ________.

CaCO3 (s) + HCl (aq) → CaCl2 (aq) + CO2 (g) + H2O (l)

A) 1

B) 2

C) 3

D) 4

E) 0

B

When the following equation is balanced, the coefficient of HNO3 is ________.

HNO3 (aq) + CaCO3 (s) → Ca(NO3)2 (aq) + CO2 (g) + H2O (l)

A) 1

B) 2

C) 3

D) 5

E) 4

B

When the following equation is balanced, the coefficient of H3PO4 is ________.

H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l)

A) 1

B) 2

C) 3

D) 4

E) 0

A

When the following equation is balanced, the coefficient of C3H8O3 is ________.

C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)

A) 1

B) 2

C) 3

D) 7

E) 5

B

When the following equation is balanced, the coefficient of O2 is ________.

C2H4O (g) + O2 (g) → CO2 (g) + H2O (g)

A) 2

B) 3

C) 4

D) 5

E) 1

D

Balance the following reaction and determine the coefficient of H2O.

CO (g) + H2 (g) → H2O (g) + CH4 (g)

A) 1

B) 2

C) 3

D) 4

E) 0

A

When the following equation is balanced, the coefficient of H2SO4 is ________.

H2SO4 (aq) + NaOH (aq) → Na2SO4 (aq) + H2O (l)

A) 1

B) 2

C) 3

D) 4

E) 0.5

A

When the following equation is balanced, the coefficient of water is ________.

K (s) + H2O (l) → KOH (aq) + H2 (g)

A) 1

B) 2

C) 3

D) 4

E) 5

B

Balance the following reaction and determine the coefficient of potassium hydroxide.

K (s) + H2O (l) → KOH (aq) + H2 (g)

A) 1

B) 2

C) 3

D) 4

E) 5

B

When the following equation is balanced, the coefficient of oxygen is ________.

PbS (s) + O2 (g) → PbO (s) + SO2 (g)

A) 1

B) 3

C) 2

D) 4

E) 5

B

When the following equation is balanced, the coefficient of sulfur dioxide is ________.

PbS (s) + O2 (g) → PbO (s) + SO2 (g)

A) 5

B) 1

C) 3

D) 2

E) 4

D

When the following equation is balanced, the coefficient of dinitrogen pentoxide is ________.

N2O5 (g) + H2O (l) → HNO3 (aq)

A) 1

B) 2

C) 3

D) 4

E) 5

A

When the following equation is balanced, the coefficient of water is ________.

N2O5 (g) + H2O (l) → HNO3 (aq)

A) 5

B) 2

C) 3

D) 4

E) 1

E

Balance the following reaction and determine the coefficient of nitric acid.

N2O5 (g) + H2O (l) → HNO3 (aq)

A) 5

B) 2

C) 3

D) 4

E) 1

B

Write the balanced equation for the reaction that occurs when
methanol, CH3OH (l), is burned in air. What is the coefficient of
methanol in the balanced equation?

A) 1

B) 2

C)
3

D) 4

E) 3/2

B

Write the balanced equation for the reaction that occurs when butane
undergoes combustion. What is the coefficient of oxygen in the
balanced equation?

A) 10

B) 8

C) 13

D) 4

E) 13/2

C

What is the coefficient of O2 when the following equation is completed and balanced?

C4H8O2 + O2 → ________

A) 2

B) 3

C) 5

D) 6

E) 1

C

Predict the product in the combination reaction below.

Al (s) + N2 (g) → ________

A) AlN

B) Al3N

C) AlN2

D) Al3N2

E) AlN3

A

The balanced equation for the decomposition of sodium azide is
________.

A) 2NaN3 (s) → 2Na (s) + 3N2 (g)

B) 2NaN3 (s) →
Na2 (s) + 3N2 (g)

C) NaN3 (s) → Na (s) + N2 (g)

D) NaN3 (s)
→ Na (s) + N2 (g) + N (g)

E) 2NaN3 (s) → 2Na (s) + 2N2 (g)

A

There are ________ mol of carbon atoms in 4 mol of C4H8O2.

A)
4

B) 8

C) 16

D) 20

E) 32

C

There are ________ sulfur atoms in 25 molecules of C4H4S2.

A)
1.5 × 10^{25}

B) 4.8 × 10^{25}

C) 3.0 ×
10^{25}

D) 50

E) 6.02 × 10^{23}

D

There are ________ hydrogen atoms in 25 molecules of C4H4S2.

A)
25

B) 3.8 × 10^{24}

C) 6.0 × 10^{25}

D) 100

E) 1.5 × 10^{25}

D

A sample of C3H8O that contains 200 molecules contains ________
carbon atoms.

A) 600

B) 200

C) 3.61 × 10^{26}

D) 1.20 × 10^{26}

E) 4.01 × 10^{25}

A

How many moles of carbon monoxide are there in 36.55 g of carbon
monoxide?

A) 1.023

B) 1.305

C) 0.8307

D)
0.7761

E) 1023

B

How many moles of carbon dioxide are there in 52.06 g of carbon
dioxide?

A) 0.8452

B) 1.183

C) 6.022 × 10^{23}

D) 8.648 × 10^{23}

E) 3.134 × 10^{25}

B

There are ________ molecules of methane in 0.123 mol of methane
(CH4).

A) 5

B) 2.46 × 10^{-2}

C) 2.04 ×
10^{-25}

D) 7.40 × 10^{22}

E) 0.615

D

What is the empirical formula of a compound that contains 27.0% S,
13.4% O, and 59.6% Cl by mass?

A) SOCl

B) SOCl2

C)
S2OCl

D) SO2Cl

E) ClSO4

B

What is the empirical formula of a compound that contains 29% Na, 41%
S, and 30% O by mass?

A) Na2S2O3

B) NaSO2

C)
NaSO

D) NaSO3

E) Na2S2O6

A

What is the empirical formula of a compound that contains 49.4% K,
20.3% S, and 30.3% O by mass?

A) KSO2

B) KSO3

C)
K2SO4

D) K2SO3

E) KSO4

D

A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The
molecular weight of the compound is 60.05 amu. The molecular formula
of this compound is ________.

A) C2H4O2

B) CH2O

C)
C2H3O4

D) C2H2O4

E) CHO2

A

A compound that is composed of carbon, hydrogen, and oxygen contains
70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the
compound is 136 amu. What is the molecular formula?

A)
C8H8O2

B) C8H4O

C) C4H4O

D) C9H12O

E) C5H6O2

A

A compound that is composed of only carbon and hydrogen contains
85.7% C and 14.3% H by mass. What is the empirical formula of the
compound?

A) CH2

B) C2H4

C) CH4

D) C4H8

E) C86H14

A

A compound that is composed of only carbon and hydrogen contains
80.0% C and 20.0% H by mass. What is the empirical formula of the
compound?

A) C20H60

B) C7H20

C) CH3

D)
C2H6

E) CH4

C

A compound contains 38.7% K, 13.9% N, and 47.4% O by mass. What is
the empirical formula of the compound?

A) KNO3

B)
K2N2O3

C) KNO2

D) K2NO3

E) K4NO5

A

A 1.038 g sample of unknown containing C, H, and O yielded 2.48 g of
CO2 and 0.510 g of H2O during combustion analysis. Determine the
empirical formula of the compound.

A) C3H3O

B) C6H6O

C)
CH3O

D) C6H6O2

E) C2H6O2

A

Combustion of a 1.031-g sample of a compound containing only carbon,
hydrogen, and oxygen produced of CO2 and of H2O. What is the empirical
formula of the compound?

A) C3H8O

B) C3H5O

C)
C12H16O5

D) C3H9O3

E) C3H6O3

A

Combustion of a 0.9827-g sample of a compound containing only carbon,
hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of H2O. What
is the empirical formula of the compound?

A) C2H5O

B)
C5H7O3

C) C4H11O2

D) C4H10O

E) C2H5O2

C

The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O:

4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g)

The combustion of 43.9 g of ammonia produces ________ g of
NO2.

A) 2.58

B) 178

C) 119

D) 0.954

E) 43.9

C

The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)

When 2.5 mol of O2 are consumed in their reaction, ________ mol of
CO2 are produced.

A) 1.5

B) 3.0

C) 4.2

D)
7.5

E) 2.5

A

Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2):

CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g)

Production of 13 g of C2H2 requires consumption of ________ g of
H2O.

A) 4.5

B) 9.0

C) 18

D) 4.8 × 10^{2}

E) 4.8 × 10^{-2}

C

Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2) as shown in the unbalanced reaction below:

CaC2 (s) + H2O (g) → Ca(OH)2 (s) + C2H2 (g)

How many grams of H2O are required to completely react with 82.4 g
of CaC2.

A) 1.29

B) 11.6

C) 46.3

D) 23.2

E) 18.0

C

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia. Write the reaction and determine the mass of H2 (g) required to completely react with 25.8 g of N2.

A) 5.57

B) 1.86

C) 77.4

D) 2.78

E) 0.928

A

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:

N2 (g) + 3H2 (g) → 2NH3 (g)

Determine the mass of N2 (g) required to completely react with 18.5
g of H2.

A) 0.51

B) 771

C) 257

D) 85.7

E) 6.17

D

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:

PbCO3 (s) → PbO (s) + CO2 (g)

How many grams of lead (II) oxide will be produced by the
decomposition of 2.50 g of lead (II) carbonate?

A) 0.41

B)
2.50

C) 0.00936

D) 2.09

E) 2.61

D

The combustion of propane (C3H8) produces CO2 and H2O:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)

The reaction of 2.5 mol of O2 with 4.6 mol of C3H8 will produce
________ mol of H2O.

A) 4.0

B) 1.25

C) 2.5

D)
2.0

E) 18.4

D

GeF3H is formed from GeH4 and GeF4 in the combination reaction:

GeH4 + 3GeF4 → 4GeF3H

If the reaction yield is 89.1%, how many moles of GeH4 are needed
to produce 3.50 mol of GeF3H?

A) 15.7

B) 3.93

C)
0.982

D) 0.875

E) 2.95

C

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:

N2 (g) + 3H2 (g) → 2NH3 (g)

If the reaction yield is 81.4 %, how many moles of N2 are needed to
produce 8.50 mol of NH3?

A) 20.9

B) 10.4

C)
5.22

D) 6.92

E) 15.7

C

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:

PbCO3 (s) → PbO (s) + CO2 (g)

If the reaction yield is 92.4%, how many grams of lead (II) oxide
will be produced by the decomposition of 1.30 g of lead (II)
carbonate?

A) 1.00

B) 1.18

C) 1.20

D) 1.09

E) 1.41

A

The combustion of ammonia in the presence of oxygen yields NO2 and H2O:

4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g)

The combustion of 43.9 g of ammonia with 258 g of oxygen produces
________ g of NO2.

A) 212

B) 178

C) 119

D)
0.954

E) 43.9

C

What mass in grams of hydrogen is produced by the reaction of 31.3 g of magnesium with 2.12 g of water?

Mg (s) + 2H2O (l) → Mg(OH)2 (s) + H2 (g)

A) 0.119

B) 0.237

C) 0.474

D) 0.0593

E) 2.71

A

If the reaction yield is 88.2%, what mass in grams of hydrogen is produced by the reaction of 7.73 g of magnesium with 1.31 g of water?

Mg (s) + 2H2O (l) → Mg(OH)2 (s) + H2 (g)

A) 0.0646

B) 0.0323

C) 0.0733

D) 0.147

E) 0.641

A

Silver nitrate and aluminum chloride react with each other by exchanging anions:

3AgNO3 (aq) + AlCl3 (aq) → Al(NO3)3 (aq) + 3AgCl (s)

What mass in grams of AgCl is produced when 4.22 g of AgNO3 react
with 7.73 g of AlCl3?

A) 2.76

B) 28.5

C) 24.9

D)
3.56

E) 11.9

D

How many moles of magnesium oxide are produced by the reaction of 1.82 g of magnesium nitride with of water?

Mg3N2 + 3H2O → 2NH3 + 3MgO

A) 0.0180

B) 0.0541

C) 0.00601

D) 0.984

E) 3.00

B

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of
water:

Mg3N2 + 3H2O → 2NH3 + 3MgO

The yield of MgO is 3.60 g. What is the percent yield in the
reaction?

A) 94.5

B) 78.7

C) 46.6

D) 49.4

E) 20.8

B

Pentacarbonyliron (Fe(CO)5) reacts with phosphorous trifluoride (PF3) and hydrogen, releasing carbon monoxide:

Fe(CO)5 + PF3 + H2 → Fe(CO)2(PF3)2(H)2 + CO (not balanced)

The reaction of 9.0 mol of Fe(CO)5, 11.0 mol of PF3 and 3.0 mol of
H2 will release ________ mol of CO.

A) 9

B) 3

C)
27

D) 16.5

E) 23

A

What is the maximum mass in grams of NH3 that can be produced by the reaction of of N2 with of H2 via the equation below?

N2 (g) + H2 (g) → NH3 (g) (not balanced)

A) 2.0

B) 1.2

C) 0.61

D) 17

E) 4.0

B

What is the maximum number of moles of SO3 that can be produced by the reaction of 2.0 mol of S with 3.0 mol of O2?

A) 2/3

B) 1.0

C) 5.0

D) 3.0

E) 2.0

E

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide:

4Al (s) + 3O2 (g) → 2Al2O3 (s)

The maximum amount of Al2O3 that can be produced from 5.0 g of Al
and 5.0 g of O2 is ________ g.

A) 19

B) 4.7

C)
9.4

D) 11

E) 2.5

C

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride:

S (s) + 3F2(g) → SF6 (g)

The maximum amount of SF6 that can be produced from the reaction of
32.1 g of sulfur with 114G of fluorine is ________ g.

A)
584

B) 438

C) 146

D) 48.7

E) 219

C

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide:

4Al (s) + 3O2 (g) → 2Al2O3 (s)

In a particular experiment, the reaction of 2.5 g of Al with 2.5 g
of O2 produced 3.5 g of Al2O3. The % yield of the reaction is
________.

A) 74

B) 37

C) 47

D) 66

E) 29

A

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant:

2S (s) + 3O2 (g) → 2SO3 (g)

In a particular experiment, the reaction of 1.0 g S with 1.0 g O2
produced 0.80 g of SO3. The % yield in this experiment is ________.

A) 32

B) 80

C) 21

D) 64

E) 47

E

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride:

S (s) + 3F2 (g) → SF6 (g)

In a particular experiment, the percent yield is 83.1%. This means
that in this experiment, a 4.50 g sample of fluorine yields ________ g
of SF6 .

A) 9.58

B) 3.74

C) 4.79

D) 43.1

E) 14.4

C

When the following equation is balanced, the coefficients are ________.

C8H18+ O2 → CO2 + H2O

A) 4, 50, 16, 18

B) 1, 5, 2, 2

C) 2, 2, 7, 1

D) 1,
13, 8, 9

E) 2, 25, 16, 18

E

The formula weight of PbCO3 is ________ amu.

A) 279.2

B)
112.0

C) 118.0

D) 267.2

E) 235.2

D

The formula weight of Zn(ClO4)2 is ________ amu.

A)
164.7

B) 327.9

C) 228.6

D) 264.3

E) 116.7

D

The formula weight of LiClO4 is ________ amu.

A) 212.3

B)
101.0

C) 52.0

D) 106.3

E) 58.3

D

The molecular weight of 2-propanol ( C3H7OH ), known as rubbing
alcohol, is ________ amu (rounded to one decimal place).

A)
59.1

B) 29.0

C) 60.1

D) 12.0

E) 34.0

C

The molecular weight of ethanol (C2H5OH), rounded to one decimal
place, is ________ amu.

A) 45.1

B) 34.1

C) 29.1

D)
46.1

E) 29.0

D

The molecular weight of maltose ( C12H22O11 ), rounded to one decimal
place, is ________ amu.

A) 507.2

B) 182.0

C)
45.0

D) 342.3

E) 29.0

D

What is the mass percent of C in carbonic acid (H*2*CO3).

19.36

What is the mass % of carbon in dimethylsulfoxide (C2H6SO) rounded to
three significant figures?

A) 15.4

B) 19.7

C)
30.7

D) 7.74

E) 20.5

C

What is the mass % of oxygen in methanol?

A) 16.0

B)
12.0

C) 50.0

D) 4.00

E) 32.0

C

What is the mass % of aluminum in aluminum sulfate (Al2(SO4)3)
rounded to three significant figures?

A) 7.90

B)
35.7

C) 15.8

D) 19.4

E) 342.2

C

What is the mass % of oxygen in lead (II) nitrate (Pb(NO3)2) rounded
to three significant figures?

A) 4.83

B) 19.3

C)
29.0

D) 14.5

E) 0.331

C

There are ________ mol of carbon atoms in 5 mol of dimethylsulfoxide
(C2H6SO).

A) 2

B) 5

C) 10

D) 12

E) 50

C

1 mole of which of the following will contain the largest number of
atoms?

A) sodium

B) magnesium

C) mercury

D)
neon

E) 1 mole of any element will contain the same number of atoms.

E

1 mole of which of the following will have the largest mass?

A)
rubidium

B) magnesium

C) gold

D) neon

E) 1 mole of
any element will contain the same mass.

C

How many grams of hydrogen are in 46 g of CH4O?

A) 5.8

B)
1.5

C) 2.8

D) 0.36

E) 180

A

There are ________ atoms of oxygen in 300 molecules of
CH3CO2H.

A) 300

B) 600

C) 150

D) 3.6 ×
10^{26}

E) 1.0 × 10^{-22}

B

How many grams of oxygen are in 56 g of C2H2O2?

A) 11

B)
58

C) 15

D) 31

E) 33

D

How many atoms of carbon are in 23.1 g of glucose (C6H12O6)?

A)
7.72 × 10^{22}

B) 4.63 × 10^{23}

C) 1.29 ×
10^{22}

D) 6.00

E) 138.6

B

A 1.36-g sample of magnesium nitrate, Mg(NO3)2, contains ________ mol
of this compound.

A) 109

B) 2.02

C) 0.0157

D)
0.0182

E) 0.00917

E

A 22.5-g sample of ammonium carbonate contains ________ mol of
ammonium ions.

A) 0.467

B) 0.288

C) 0.234

D)
2.14

E) 3.47

A

What is the mass in grams of 9.76 × 10^{12} atoms of
naturally occurring potassium?

A) 2.41 × 10^{12}

B)
2.50 × 10^{11}

C) 6.34 × 10^{-10}

D) 1.62
× 10^{-11}

E) 3.82 × 101^{4}

C

What is the mass in grams of 2.00 × 10^{5} atoms of naturally
occurring neon?

A) 6.08 × 10^{19}

B) 2.43 × 10^{30}

C) 6.70 × 10^{-18}

D) 1.65 × 10^{-20}

E) 3.32 × 10^{-24}

C

How many moles of pyridine (C5H5N) are contained in 4.14 g of
pyridine?

A) 0.0523

B) 327

C) 6.88 × 10^{-24}

D) 2.49 ×10^{24}

E) 79.1

A

How many moles of lithium phosphate (Li3PO4) are contained in 66.6 g
of lithium phosphate?

A) 0.575

B) 7710

C) 1.11 ×
10^{-22}

D) 4.01 × 10^{25}

E) 116

A

How many grams of calcium cyanide (Ca(CN)2) are contained in 0.69 mol
of calcium cyanide?

A) 64

B) 0.0075

C) 1.2 × 10^{-24}

D) 4.2 × 10^{23}

E) 92

A

How many grams of phenol (C6H5OH) are contained in 5.50 mol of
phenol?

A) 518

B) 0.0584

C) 9.14 × 10^{-24}

D) 3.31 × 10^{24}

E) 94.1

A

What is the empirical formula of a compound that is 66.6% C, 11.2% H,
and 22.2% O by mass?

A) C4HO

B) C6HO2

C)
C8H16O2

D) C6H11O

E) C4H8O

E

A certain alcohol contains only three elements, carbon, hydrogen, and oxygen. Combustion of a 60.00 gram sample of the alcohol produced 114.6 grams of CO2 and 70.44 grams of H2O. What is the empirical formula of the alcohol?

C2H6O

Lithium and nitrogen react to produce lithium nitride:

6Li (s) + N2 (g) → 2Li3N (s)

How many moles of N2 are needed to react with 0.550 mol of
lithium?

A) 3.30

B) 0.550

C) 0.183

D) 1.65

E) 0.0917

E

The combustion of propane (C3H8) produces CO2 and H2O:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)

The reaction of 2.5 mol of O2 will produce ________ mol of
H2O.

A) 4.0

B) 3.0

C) 2.5

D) 2.0

E) 1.0

D

Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:

3 Mg + N2 → Mg3N2

In a particular experiment, a 8.33-g sample of reacts completely.
The mass of Mg consumed is ________ g.

A) 7.23

B)
21.7

C) 28.9

D) 0.92

E) 13.9

B

The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O:

4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g)

The combustion of 14.4 g of ammonia consumes ________ g of
oxygen.

A) 13.5

B) 28.8

C) 54.1

D) 47.3

E) 94.6

D

Lithium and nitrogen react to produce lithium nitride:

6Li (s) + N2 (g) → 2Li3N (s)

How many moles of lithium nitride are produced when 0.330 mol of
lithium react in this fashion?

A) 0.110

B) 0.660

C)
0.0550

D) 0.990

E) 0.165

A

Lithium and nitrogen react in a combination reaction to produce lithium nitride:

6Li (s) + N2 (g) → 2Li3N (s)

How many moles of lithium are needed to produce 0.45 mol of Li3N
when the reaction is carried out in the presence of excess
nitrogen?

A) 0.23

B) 1.4

C) 0.15

D) 0.30

E) 2.7

B

Automotive air bags inflate when sodium azide decomposes explosively
to its constituent elements:

2NaN3 (s) → 2Na (s) + 3N2 (g)

How many moles of N2 are produced by the decomposition of 1.75 mol
of sodium azide?

A) 1.17

B) 5.25

C) 2.63

D)
0.583

E) 0.875

C

Automotive air bags inflate when sodium azide decomposes explosively
to its constituent elements:

2NaN3 (s) → 2Na (s) + 3N2 (g)

How many grams of sodium azide are required to produce 28.0 g of
nitrogen?

A) 1.50

B) 0.666

C) 65.0

D) 43.3

E) 97.5

D

Magnesium burns in air with a dazzling brilliance to produce
magnesium oxide:

2Mg (s) + O2(g) → 2MgO (s)

How many moles of O2 are consumed when 3.55 mol of magnesium
burns?

A) 0.146

B) 0.563

C) 3.55

D) 7.10

E) 1.78

E

Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2):

CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g)

Production of 6.5 g of C2H2 requires consumption of ________ g of
H2O.

A) 2.3

B) 4.5

C) 9.0

D) 480

E) 0.048

C

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:

PbCO3 (s) → PbO (s) + CO2 (g)

________ grams of lead (II) oxide will be produced by the
decomposition of 8.75 g of lead (II) carbonate?

A) 10.5

B)
2.50

C) 0.033

D) 7.31

E) 8.75

D

Lithium and nitrogen react in a combination reaction to produce lithium nitride:

6Li (s) + N2 (g) → 2Li3N (s)

In a particular experiment, 2.50-g samples of each reagent are
reacted. The theoretical yield of lithium nitride is ________
g.

A) 2.51

B) 2.09

C) 12.5

D) 4.18

E) 6.2

D

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:

2Mg (s) + O2 (g) → 2MgO (s)

When 5.50 g of magnesium burns, the theoretical yield of magnesium
oxide is ________ g.

A) 5.50

B) 9.12

C) 0.226

D)
4.56

E) 18.2

B

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:

CaO (s) + H2O (l) → Ca(OH)2 (s)

A 3.50 g sample of CaO is reacted with 3.38 g of H2O. How many grams
of water remain after completion of reaction?

A) 0.00

B)
0.00694

C) 2.25

D) 1.04

E) 0.125

C

If 588 grams of FeS2 is allowed to react with 352 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced?

FeS2 + O2 → Fe2O3 + SO2

320

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:

CaO (s) + H2O (l) → Ca(OH)2 (s)

In a particular experiment, a 2.00-g sample of CaO is reacted with
excess water and 2.14 g of Ca(OH)2 is recovered. What is the percent
yield in this experiment?

A) 107

B) 1.07

C)
2.88

D) 81.1

E) 93.3

D

Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of 6.0 grams of O2 with 7.0 grams of S. What is the % yield of SO3 in this experiment?

S (s) + O2 (g) → SO3 (g) (not balanced)

A) 45

B) 53

C) 22.5

D) 79

E) 35

D

Complete and balance the following reaction, given that elemental sodium reacts with elemental oxygen to form Na2O (s).

K (s) + S (s) → ________

K2S (s)

A compound was found to contain 90.6% lead (Pb) and 9.4% oxygen. The empirical formula for this compound is ________.

Pb3O4

The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)

How many grams of CO2 is produced when 12.5 g of C3H8 burns in open air?

37.4

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia. A 18.2 g sample of hydrogen requires ________ g of N2 for a complete reaction.

84.3

Water can be formed from the stoichiometric reaction of hydrogen with oxygen. How many grams of H2O is generated when 45.3 g of O2 reacts with excess hydrogen?

51.0

The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide and sulfur dioxide. The combustion of 10 mol of CS2 in the presence of excess oxygen yields ________ mol of SO2.

20

The mass of a single atom of an element (in amu) is numerically equal to the mass in grams of that element.

false

The empirical weight is always a whole-number multiple of the molecular formula weight.

false

A great deal of oxygen is produced during combustion.

false

The quantity of product that is calculated to form when all of the limiting reagent reacts is called the percent yield.

false