Chemistry Chapter 9 The theoretical mass of sulfur dioxide produced

74) The maximum number of moles of carbon dioxide that can be produced from four moles of

C3H8O is ________.

2 C3H8O + 9 O2 → 6 CO2 + 8 H2O

A) 4

B) 6

C) 8

D) 12

75) Which reactant is present in excess if 10.0 g of CaO react with 3.0 mol of H2O?

CaO + H2O → Ca(OH)2

A) Ca(OH)2

B) CaO

C) H2O

D) None of the above, the amounts exactly balance.

76) Which of the following abides by the principle of mass conservation according to the

balanced reaction?

4 K + O2 → 2 K2O

A) 39.0g K + 16.0g O2 → 94.0g K2O

B) 156.0 g K + 24.0g O2 → 188.0g K2O

C) 156.0g K + 32.0g O2 → 188.0g K2O

D) 78.0g K + 32.0g O2 → 110.0g K2O

77) The theoretical number of carbon dioxide moles produced from 3 moles of C2H6O is

________.

C2H6O + O2 → CO2 + H2O

A) 3

B) 4

C) 6

D) 9

78) The theoretical number of carbon dioxide moles produced from 6 moles of NaHCO3 is

________.’

NaHCO3 → Na2CO3 + CO2 + H2O

A) 1

B) 3

C) 6

D) 12

79) The theoretical number of moles of water produced from 8 moles of NaHCO3 is ________.

NaHCO3 → Na2CO3 + CO2 + H2O

A) 2

B) 4

C) 8

D) 16

80) What is the theoretical mass of carbon dioxide produced from 4.0 moles of NaHCO3?

NaHCO3 → Na2CO3 + CO2 + H2O

A) 1.0 g

B) 22 g

C) 44 g

D) 88 g

81) What is the theoretical mass of water produced from 10 moles of NaHCO3?

NaHCO3 → Na2CO3 + CO2 + H2O

A) 180 g

B) 90 g

C) 45 g

D) 18 g

82) Determine the percent yield of an experiment in which 1.00 mole of NaHCO3 was consumed

and 22.0 g of carbon dioxide was isolated.

NaHCO3 → Na2CO3 + CO2 + H2O

A) 100.%

B) 50.0%

C) 37.5%

D) 25%

83) The theoretical number of moles of water produced from 2 moles of C2H6O is ________.

C2H6O + O2 → CO2 + H2O

A) 2

B) 3

C) 6

D) 9

84) What is the theoretical mass of carbon dioxide produced from one mole of C2H6O?

C2H6O + O2 → CO2 + H2O

A) 6 g

B) 44 g

C) 88 g

D) 176 g

85) Determine the percent yield of an experiment in which 1 mole of C2H6O was consumed and

22 g of carbon dioxide was isolated.

C2H6O + O2 → CO2 + H2O

A) 100%

B) 50%

C) 37.5%

D) 25%

86) The theoretical number of moles of carbon dioxide produced from 3.0 moles of C6H14 is

________.

C6H14 + O2 → CO2 + H2O

A) 3.0

B) 6.0

C) 9.0

D) 18

87) The theoretical number of water moles produced from two moles of C6H14 is ________.

C6H14 + O2 → CO2 + H2O

A) 1

B) 6

C) 7

D) 14

88) What is the theoretical mass of carbon dioxide produced from one mole of C6H14?

C6H14 + O2 → CO2 + H2O

A) 6 g

B) 44 g

C) 132 g

D) 264 g

89) The % yield of an experiment in which 1.0 mole of C6H14 was used and 22 g of carbon

dioxide was isolated is ________.

C6H14 + O2 → CO2 + H2O

A) 100%

B) 50%

C) 17.5%

D) 8.3%

90) The theoretical number of moles of sodium produced from 4 moles of NaN3 is ________.

NaN3 → Na + N2

A) 1

B) 2

C) 4

D) 8

91) The theoretical number of moles of nitrogen produced from 6 moles of NaN3 is ________.

NaN3 → Na + N2

A) 2

B) 6

C) 9

D) 18

92) The theoretical mass of sodium produced from 2.0 moles of NaN3 is ________.

NaN3 → Na + N2

A) 11.5 g

B) 23 g

C) 34.5 g

D) 46 g

93) The percent yield of an experiment in which 2.0 moles of NaN3 was used and 21 g of

nitrogen was isolated is ________.

NaN3 → Na + N2

A) 100%

B) 50%

C) 37.5%

D) 25%

94) The minimum number of moles of oxygen needed to completely consume 4 moles of

C3H8O is ________.

2 C3H8O + 9 O2 → 6 CO2 + 8 H2O

A) 4

B) 9

C) 13.5

D) 18

95) The theoretical yield of water produced from of 2.0 moles of C3H8O is ________ g.

2 C3H8O + 9 O2 → 6 CO2 + 8 H2O

A) 8

B) 18

C) 36

D) 144

96) If 36 g of water are produced from two moles of C3H8O, the percent yield of the reaction is

________.

2 C3H8O + 9 O2 → 6 CO2 + 8 H2O

A) 100%

B) 50%

C) 25%

D) 10%

97) The theoretical number of moles of copper that will react with 4 moles of sulfuric acid is

________.

H2SO4 + Cu → SO2 + H2O + CuSO4

A) 2

B) 4

C) 6

D) 8

98) The theoretical number of moles of sulfur dioxide produced from 4 moles of sulfuric acid is

________.

H2SO4 + Cu → SO2 + H2O + CuSO4

A) 2

B) 4

C) 6

D) 8

99) The theoretical number of moles of water produced from 4 moles of sulfuric acid is

________.

H2SO4 + Cu → SO2 + H2O + CuSO4

A) 2

B) 4

C) 6

D) 8

100) The theoretical mass of sulfur dioxide produced from 2.0 moles of sulfuric acid is

________.

H2SO4 + Cu → SO2 + H2O + CuSO4

A) 8.0 g

B) 16.0 g

C) 32.0 g

D) 64.1 g

101) The percent yield of an experiment in which 2.0 moles of copper was used and 18 g of

water was isolated is ________.

H2SO4 + Cu → SO2 + H2O + CuSO4

A) 100%

B) 50%

C) 37.5%

D) 25%

102) How many grams of oxygen will react with 20 g of ammonia?

NH3 + O2 → NO + H2O

A) 71 g

B) 94 g

C) 24 g

D) 47 g

103) How many grams of NO will form when 40 g of oxygen are used?

NH3 + O2 → NO + H2O

A) 30 g

B) 15 g

C) 45 g

D) 60 g

104) How many grams of ammonia are consumed if 45.0 g of NO are formed in a 100% yield?

NH3 + O2 → NO + H2O

A) 6.51 g

B) 13.0 g

C) 26.0 g

D) 39.0 g

105) What is the percent yield if 52 g of ammonia produce 45 g of NO?

NH3 + O2 → NO + H2O

A) 100%

B) 49%

C) 25%

D) 18%

106) What is the mass of NO expected if 104 g of ammonia are consumed in a 100% yield?

NH3 + O2 → NO + H2O

A) 45.7 g

B) 91.5 g

C) 183 g

D) 366 g

107) 14 g of nitrogen will react with ________ g of oxygen.

N2 + 2 O2 → 2 NO2

A) 8

B) 16

C) 32

D) 64

108) 14 g of nitrogen will yield ________ g of nitrogen dioxide.

N2 + 2 O2 → 2 NO2

A) 23

B) 46

C) 92

D) 194

109) 64 g of oxygen will yield ________ g of nitrogen dioxide.

N2 + 2 O2 → 2 NO2

A) 23

B) 46

C) 92

D) 184

110) The maximum amount of IF7 that can be obtained from 25.0 g is fluorine is ________.

I2 + F2 → IF7

A) 63 g

B) 48.9 g

C) 24.5 g

D) 12.3 g

111) How many moles of aluminum chloride can be obtained from 4.5 moles of aluminum and

excess chlorine?

Al + Cl2 → AlCl3

A) 1.5

B) 3.0

C) 4.5

D) 6.0

112) Which reactant is the limiting reagent if 6 mol of H2 and 4 mol of O2 are used?

2H2 + O2 → 2H2O

A) O2

B) H2

C) neither H2 nor O2

D) both H2 and O2

113) Which reagent will be used up first if 78.1 g of O2 is reacted with 62.4 g of C4H10?

2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

A) C4H10, butane

B) oxygen

C) water

D) carbon dioxide

114) How many grams of CO2 can be made from reacting 78.1 g of O2 and 62.4 g of C4H10?

2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

A) 66.1 g CO2

B) 141 g CO2

C) 189 g CO2

D) 378 g CO2

E) 430 g CO2

115) The reaction was performed in the lab and 50.1 g of CO2 was collected from the reaction of

78.1 g of O2 with 62.4 g of C4H10. The percent yield of this reaction is ________.

2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

A) 11.7 %

B) 13.3 %

C) 26.5 %

D) 35.7 %

E) 75.8 %

116) The reaction was performed in the lab and 50.1 g of CO2 was collected from the reaction of

78.1 g of O2 with 62.4 g of C4H10. How many grams of the excess reactant are left over.

2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

A) 15.7 g

B) 21.8 g

C) 28.0 g

D) 40.6 g

E) 45.8 g

117) Which statement is true about the empirical formula?

A) The empirical formula is always different than the molecular formula.

B) The empirical formula is always the same as the molecular formula.

C) The empirical formula may be different than the molecular formula.

D) The empirical formula cannot be determined solely by the % composition.

118) Which statement is true about the molecular formula?

A) The molecular formula is always different than the empirical formula.

B) The molecular formula is always the same as the empirical formula.

C) The empirical formula may be different than the molecular formula.

D) The empirical formula can be determined solely by the % composition.

119) Which statement is true when comparing acetic acid C2H4O2 and formaldehyde CH2O?

A) Their empirical formulas are identical.

B) Their molecular formulas are identical.

C) Their molecular formulas are different.

D) both A and C

120) If the empirical formula of a compound is CH2O and the molecular weight is 180, the

molecular formula is ________.

A) CH2O

B) C2H4O2

C) C3H6O3

D) C6H12O6

121) Which of the following has its empirical formula different than its molecular formula?

A) CH2S

B) C2H7N3

C) C3H6N3

D) C5H7O3

122) Which of the following pairs does not share the same empirical formula?

A) CH2O and C3H6O3

B) C6H6 and C2H2

C) C2H6O and CH3O

D) C3H4Br2 and C9H12O6

123) Which of the following does not share the same empirical formula as the other three?

A) CH2O

B) C6H12O6

C) C8H16O8

D) C12H22O11

124) What is the empirical formula of C8H6O3?

A) CHO

B) C4H3O

C) C4H3O2

D) C8H6O3

125) A certain compound has the following composition: C= 40.0% and H= 6.7%. The empirical

formula is ________.

A) CH

B) CH2O

C) C6H6O

D) CHO

126) An independent experiment showed that the molecular weight of isopropyl alcohol is

approximately 62. The molecular formula therefore is ________.

A) C2H6O2

B) C3H8O2

C) C3H8O

D) C3H10O2

127) 5.82 g isopropyl alcohol yield 7.001 g of water and 12.6 g of carbon dioxide upon

combustion. The empirical formula is ________.

A) CH2O

B) C3H8O

C) C2H6O

D) C3H9O

128) Combustion of 6.51 mg of a compound produces 20.46 mg of carbon dioxide and 8.36 mg

of water. The empirical formula is ________.

A) CH2O

B) C2H3

C) C2H3O

D) CH2

129) Combustion of 5.00 mg of a compound produces 15.2 mg of carbon dioxide and 7.80 mg of

water. The empirical formula is ________.

A) CH2

B) C2H5

C) C3H7

D) C4H10

130) Combustion of 5.00 mg of a compound produces 9.60 mg of carbon dioxide and 5.90 mg of

water. The empirical formula is ________.

A) CH2O

B) C2H5

C) C2H6O

D) C4H10O

131) What is the molecular formula of a compound that weighs 46 g/mol and analyzes to 52.2%

C, 34.8% O, and 13% H?

A) C3H2O2

B) C2H6O

C) CH3O

D) C2H5O2

132) A compound is found to be 43.7% phosphorus and 56.3% oxygen. Given the molecular

mass as 285 ± 10, calculate the empirical and molecular formulas.

A) PO2; P4O8

B) P2O5; P4O10

C) P2O3; P6O9

D) P4O10; P4O10

133) A sample is composed of 2.78 g of iron and 1.19 g of oxygen. The empirical formula is

________.

A) FeO2

B) Fe2O5

C) Fe2O3

D) FeO

134) Which compound has the percent composition of 15.8% Al, 28.1% S and 56.1% O?

A) Al2(SO4)3

B) Al2(SO3)3

C) Al2S3

D) Al2(S2O3)3

135) A chromium-silicon compound contains 73.52% chromium. The empirical formula is

________.

A) CrSi

B) CrSi2

C) Cr2Si

D) Cr3Si2

136) An iron oxide is 72.4% in iron. Its empirical formula is ________.

A) FeO

B) Fe2O

C) Fe2O3

D) Fe3O4

137) An iron oxide is 77.7% in iron. Its empirical formula is ________.

A) FeO

B) Fe2O

C) Fe2O3

D) Fe3O4