Question 1

Determine the mass of precipitate (in grams)  that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO3) 2 solution. 2KI(aq)  + Pb(NO3) 2(aq)  → PbI2(s)  + 2KNO3(aq)

Accepted Answer

A)  5.19 g
B)  2.59 g
C)  12.0 g
D)  3.48 g
E)  9.55 gF) D) and E)
G) B) and E)

Question 2

What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.)  (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  24.6 g
B)  70.8 g
C)  272 g
D)  408 g
E)  612 gF) C) and D)
G) A) and B)

Question 3

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

Accepted Answer

A)  28.1 g
B)  14.04 g
C)  4.96 g
D)  7.02 g
E)  400.0 gF) C) and E)
G) A) and D)

Question 4

If 31.3 g of manganese(II)  chloride, 48.3 g of chlorine gas, and 25.7 g of water react to produce manganese(IV)  oxide and hydrochloric acid, what is the limiting reactant and what mass of hydrochloric acid is produced?

Accepted Answer

A)  manganese(II)  chloride is the limiting reactant and 9.07 g of hydrochloric acid is produced
B)  chlorine is the limiting reactant and 99.3 g of hydrochloric acid is produced
C)  chlorine is the limiting reactant and 24.8 g of hydrochloric acid is produced
D)  manganese(II)  chloride is the limiting reactant and 36.3 g of hydrochloric acid is produced
E)  water is the limiting reactant and 52.0 g of hydrochloric acid is producedF) B) and C)
G) C) and D)

Question 5

What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al2O3 + 3C → 2Al + 3CO

Accepted Answer

A)  15.9 g
B)  31.8 g
C)  44.9 g
D)  63.6 g
E)  67.4 gF) None of the above
G) B) and C)

Question 6

What mass of ammonia is formed when 5.36 g of nitrogen gas reacts with excess hydrogen gas?

Accepted Answer

A)  3.26 g
B)  0.629 g
C)  13.04 g
D)  17.63 g
E)  6.52 gF) A) and B)
G) A) and E)

Question 7

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

Accepted Answer

A)  90.g
B)  36 g
C)  42 g
D)  45 g
E)  108 gF) B) and E)
G) A) and B)

Question 8

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced?

Accepted Answer

A)  Calcium is the limiting reactant and 47.2 g of calcium oxide are produced
B)  Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced
C)  Oxygen is the limiting reactant and 48.7 g of calcium oxide are produced
D)  Calcium is the limiting reactant and 23.6 g of calcium oxide are producedE) A) and D)
F) A) and C)

Question 9

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S8? 8Fe(s)  + S8(s)  → 8FeS(s)

Accepted Answer

A)  186 g
B)  142 g
C)  119 g
D)  14.8 g
E)  0.169 gF) A) and E)
G) C) and D)

Question 10

How much heat is released if 7.15 g CaO(s)  is added to 152 g of H2O(l) ? CaO(s)  + H2O(l)  → Ca(OH) 2(s)  heat of reaction = −64.8 kJ/mol

Accepted Answer

A)  7.68 kJ
B)  8.26 kJ
C)  508 kJ
D)  547 kJ
E)  555 kJF) A) and D)
G) C) and E)

Question 11

What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO2 + O2 → 2SO3

Accepted Answer

A)  10.0 g
B)  12.5 g
C)  22.5 g
D)  55.0 g
E)  77.5 gF) C) and D)
G) A) and B)

Question 12

One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na3(CO3) (HCO3) ·2H2O. 2Na3(CO3) (HCO3) ·2H2O(s)  → 3Na2CO3(s)  + CO2(g)  + 5H2O(g) 
When 1.00 metric ton (1.00 × 103 kg)  of trona is decomposed, 0.650 metric ton of Na2CO3 is recovered.What is the percent yield of this reaction?

Accepted Answer

A)  92.4%
B)  72.1%
C)  65.0%
D)  48.1%
E)  35.0%F) C) and D)
G) A) and C)

Question 13

What volume of 0.233 M H2SO4 is needed to react exactly with 15.0 grams of aluminum? 2Al(s)  + 3H2SO4(aq)  → Al2(SO4) 3(aq)  + 3H2(g)

Accepted Answer

A)  2.39 L
B)  0.556 L
C)  0.864 L
D)  4.22 L
E)  3.58 LF) A) and C)
G) C) and D)

Question 14

Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides)  and dichlorine oxide (used as a bleach for wood, pulp and textiles) .SO2(g)  + 2Cl2(g)  → SOCl2(g)  + Cl2O(g)  If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed?

Accepted Answer

A)  0.800 mol
B)  0.400 mol
C)  0.200 mol
D)  0.100 mol
E)  0.0500 molF) A) and B)
G) A) and E)

Question 15

Magnesium (used in the manufacture of light alloys)  reacts with iron(III)  chloride to form magnesium chloride and iron.A mixture of 41.0 g of magnesium and 175.0 g of iron(III)  chloride is allowed to react.Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.

Accepted Answer

A)  Limiting reactant is Mg; 7.4 g of FeCl3 remain.
B)  Limiting reactant is Mg; 46.5 g of FeCl3 remain.
C)  Limiting reactant is FeCl3; 1.7 g of Mg remain.
D)  Limiting reactant is FeCl3; 37.8 g of Mg remain.
E)  Limiting reactant is Mg; 134.0 g of FeCl3 remain.F) A) and D)
G) C) and D)

Question 16

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Accepted Answer

A)  Chlorine is the limiting reactant; 1.14 g of potassium remain.
B)  Potassium is the limiting reactant; 2.00 g of chlorine remain.
C)  Potassium is the limiting reactant; 2.47 g of chlorine remain.
D)  Chlorine is the limiting reactant; 3.07 g of potassium remain.
E)  Potassium is the limiting reactant; 4.50 g of chlorine remain.F) B) and D)
G) A) and C)

Question 17

What volume of 0.307 M K2SO4 solution is required to react exactly with 85.0 mL of 0.100 M AgNO3? K2SO4(aq)  + 2AgNO3(aq)  → 2KNO3(aq)  + Ag2SO4(s)

Accepted Answer

A)  52.2 mL
B)  26.1 mL
C)  55.4 mL
D)  27.7 mL
E)  13.8 mLF) B) and D)
G) A) and E)

Question 18

What mass of nitrogen gas is required to react completely with 2.79 g of hydrogen gas to produce ammonia?

Accepted Answer

A)  25.8 g
B)  12.9 g
C)  78.2 g
D)  38.7 g
E)  77.4 gF) C) and D)
G) A) and E)

Question 19

What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V2O5 with 4.0 moles of calcium based on the following chemical equation? V2O5(s)  + 5Ca(l)  → 2V(l)  + 5CaO(s)

Accepted Answer

A)  1.0 mol
B)  1.6 mol
C)  2.0 mol
D)  0.80 mol
E)  3.2 molF) A) and D)
G) C) and D)

Question 20

How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen gas?

Accepted Answer

A)  8.62 g
B)  34.5 g
C)  4.31 g
D)  40.1 g
E)  17.2 gF) B) and C)
G) A) and E)

Exam 11: Using Balanced Chemical Equations

What volume of 0.233 M H₂SO₄ is needed to react exactly with 15.0 grams of aluminum? 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄) ₃(aq) + 3H₂(g)

Correct Answer
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What volume of 0.307 M K₂SO₄ solution is required to react exactly with 85.0 mL of 0.100 M AgNO₃? K₂SO₄(aq) + 2AgNO₃(aq) → 2KNO₃(aq) + Ag₂SO₄(s)

Correct Answer
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How much heat is released if 7.15 g CaO(s) is added to 152 g of H₂O(l) ? CaO(s) + H₂O(l) → Ca(OH) ₂(s) heat of reaction = −64.8 kJ/mol

Correct Answer
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What mass of nitrogen gas is required to react completely with 2.79 g of hydrogen gas to produce ammonia?

Correct Answer
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Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO₃) ₂ solution. 2KI(aq) + Pb(NO₃) ₂(aq) → PbI₂(s) + 2KNO₃(aq)

Correct Answer
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What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s) + S₈(s) → 8FeS(s)

Correct Answer
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Correct Answer
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Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Correct Answer
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What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al₂O₃ + 3C → 2Al + 3CO

Correct Answer
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What mass of ammonia is formed when 5.36 g of nitrogen gas reacts with excess hydrogen gas?

Correct Answer
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What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

Correct Answer
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If 31.3 g of manganese(II) chloride, 48.3 g of chlorine gas, and 25.7 g of water react to produce manganese(IV) oxide and hydrochloric acid, what is the limiting reactant and what mass of hydrochloric acid is produced?

Correct Answer
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What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

Correct Answer
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If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced?

Correct Answer
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What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V₂O₅ with 4.0 moles of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) → 2V(l) + 5CaO(s)

Correct Answer
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Correct Answer
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How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen gas?

Correct Answer
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How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

Correct Answer
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Correct Answer
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What mass of excess reactant remains at the end of the reaction if 90.0 g of SO₂ are mixed with 100.0 g of O₂? 2SO₂ + O₂ → 2SO₃

Correct Answer
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Exam 11: Using Balanced Chemical Equations

What volume of 0.233 M H2SO4 is needed to react exactly with 15.0 grams of aluminum? 2Al(s) + 3H2SO4(aq) → Al2(SO4) 3(aq) + 3H2(g)

Correct AnswerverifiedShow Answer

What volume of 0.307 M K2SO4 solution is required to react exactly with 85.0 mL of 0.100 M AgNO3? K2SO4(aq) + 2AgNO3(aq) → 2KNO3(aq) + Ag2SO4(s)

Correct AnswerverifiedShow Answer

How much heat is released if 7.15 g CaO(s) is added to 152 g of H2O(l) ? CaO(s) + H2O(l) → Ca(OH) 2(s) heat of reaction = −64.8 kJ/mol

Correct AnswerverifiedShow Answer

What mass of nitrogen gas is required to react completely with 2.79 g of hydrogen gas to produce ammonia?

Correct AnswerverifiedShow Answer

Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO3) 2 solution. 2KI(aq) + Pb(NO3) 2(aq) → PbI2(s) + 2KNO3(aq)

Correct AnswerverifiedShow Answer

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S8? 8Fe(s) + S8(s) → 8FeS(s)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Correct AnswerverifiedShow Answer

What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al2O3 + 3C → 2Al + 3CO

Correct AnswerverifiedShow Answer

What mass of ammonia is formed when 5.36 g of nitrogen gas reacts with excess hydrogen gas?

Correct AnswerverifiedShow Answer

What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

If 31.3 g of manganese(II) chloride, 48.3 g of chlorine gas, and 25.7 g of water react to produce manganese(IV) oxide and hydrochloric acid, what is the limiting reactant and what mass of hydrochloric acid is produced?

Correct AnswerverifiedShow Answer

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

Correct AnswerverifiedShow Answer

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced?

Correct AnswerverifiedShow Answer

What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V2O5 with 4.0 moles of calcium based on the following chemical equation? V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)

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Correct AnswerverifiedShow Answer

How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen gas?

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How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

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Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp and textiles) .SO2(g) + 2Cl2(g) → SOCl2(g) + Cl2O(g) If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed?

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What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO2 + O2 → 2SO3

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What volume of 0.233 M H₂SO₄ is needed to react exactly with 15.0 grams of aluminum? 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄) ₃(aq) + 3H₂(g)

Correct Answer
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What volume of 0.307 M K₂SO₄ solution is required to react exactly with 85.0 mL of 0.100 M AgNO₃? K₂SO₄(aq) + 2AgNO₃(aq) → 2KNO₃(aq) + Ag₂SO₄(s)

Correct Answer
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How much heat is released if 7.15 g CaO(s) is added to 152 g of H₂O(l) ? CaO(s) + H₂O(l) → Ca(OH) ₂(s) heat of reaction = −64.8 kJ/mol

Correct Answer
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Correct Answer
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Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO₃) ₂ solution. 2KI(aq) + Pb(NO₃) ₂(aq) → PbI₂(s) + 2KNO₃(aq)

Correct Answer
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What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s) + S₈(s) → 8FeS(s)

Correct Answer
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Correct Answer
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Correct Answer
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What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al₂O₃ + 3C → 2Al + 3CO

Correct Answer
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Correct Answer
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What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V₂O₅ with 4.0 moles of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) → 2V(l) + 5CaO(s)

Correct Answer
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Correct Answer
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Correct Answer
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How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

Correct Answer
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Correct Answer
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What mass of excess reactant remains at the end of the reaction if 90.0 g of SO₂ are mixed with 100.0 g of O₂? 2SO₂ + O₂ → 2SO₃

Correct Answer
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