Question 1

The first step in the Ostwald process for producing nitric acid is as follows: 4NH3(g)  + 5O2(g)  → 4NO(g)  + 6H2O(g) . If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction?

Accepted Answer

A)  29.0%
B)  32.9%
C)  49.5%
D)  61.8%
E)  77.3%F) A) and B)
G) D) and E)

Question 2

What volume of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 in excess HCl(aq) ? MnO2(s)  + 4HCl(aq)  → MnCl2(aq)  + 2H2O(l)  + Cl2(g)  (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  5.36 × 10−3 L
B)  0.138 L
C)  0.282 L
D)  3.09 L
E)  3.55 LF) A) and B)
G) A) and E)

Question 3

What volume of CO2 gas at 645 torr and 800.K could be produced by the decomposition of 45.0 g of CaCO3? CaCO3(s)  → CaO(s)  + CO2(g)  (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  0.449 L
B)  22.4 L
C)  25.0 L
D)  34.8 L
E)  45.7 mLF) A) and C)
G) C) and D)

Question 4

What mass of precipitate forms when 25.0 mL of 0.147 M NiCl2 solution reacts with excess sodium phosphate according to the given balanced chemical equation. 3NiCl2(aq)  + 2Na3PO4(aq)  → Ni3(PO4) 2(s)  + 6NaCl(aq)

Accepted Answer

A)  0.149 g
B)  0.448 g
C)  1.35 g
D)  0.368 g
E)  0.234 gF) None of the above
G) A) and D)

Question 5

Aluminum reacts with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis) . Al(s)  + Br2(l)  → Al2Br6(s)  [unbalanced]
How many moles of Al are needed to form 2.43 mol of Al2Br6?

Accepted Answer

A)  7.29 mol
B)  4.86 mol
C)  2.43 mol
D)  1.62 mol
E)  1.22 molF) A) and B)
G) A) and C)

Question 6

What mass of Cr can be produced by the reaction of 44.1 g of Cr2O3 with 35.0 g of Al according to the following chemical equation? 2Al + Cr2O3 → Al2O3 + 2Cr

Accepted Answer

A)  15.1 g
B)  30.2 g
C)  67.4 g
D)  99.9g
E)  104 gF) None of the above
G) B) and E)

Question 7

Zinc dissolves in hydrochloric acid to yield hydrogen gas as follows: Zn(s)  + 2HCl(aq)  → ZnCl2(aq)  + H2(g)  What mass of hydrogen gas is produced when a 7.35-g sample of zinc dissolves in 500.mL of 1.200 M HCl?

Accepted Answer

A)  0.605 g
B)  0.113 g
C)  0.302 g
D)  0.453 g
E)  0.227 gF) A) and C)
G) None of the above

Question 8

Lead(II)  sulfide was once used in glazing earthenware.It will also react with hydrogen peroxide to form lead(II)  sulfate and water.How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II)  sulfide?

Accepted Answer

A)  151 g
B)  123 g
C)  50.3 g
D)  37.7 g
E)  9.41 gF) C) and D)
G) C) and E)

Question 9

Phosphine, an extremely poisonous and highly reactive gas, reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH3(g)  + O2(g)  → P4O10(s)  + H2O(g)  [unbalanced]
Calculate the mass of P4O10(s)  formed when 225 g of PH3 reacts with excess oxygen.

Accepted Answer

A)  1880 g
B)  940.g
C)  900.g
D)  470.g
E)  56.3 gF) A) and E)
G) None of the above

Question 10

What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides)  is required to form 485 g of sulfur tetrafluoride? 3SCl2(l)  + 4NaF(s)  → SF4(g)  + S2Cl2(l)  + 4NaCl(s)

Accepted Answer

A)  1.94 kg
B)  1.51 kg
C)  754 g
D)  205 g
E)  51.3 gF) A) and B)
G) A) and C)

Question 11

Calculate the volume of H2(g)  at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with 50.0 g Zn(s)  to give hydrogen gas and aqueous zinc chloride. (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  0.56 L
B)  1.12 L
C)  2.23 L
D)  4.47 L
E)  3.54 LF) B) and E)
G) A) and D)

Question 12

Magnesium metal (0.100 mol)  and hydrochloric acid (0.500 mol HCl)  are combined and react to completion.What volume of hydrogen gas, measured at STP, is produced? Mg(s)  + 2HCl(aq)  → MgCl2(aq)  + H2(g)  (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  2.24 L of H2
B)  4.48 L of H2
C)  5.60 L of H2
D)  11.2 L of H2
E)  22.4 L of H2F) A) and B)
G) A) and C)

Question 13

Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows: 4NH3 + 5O2 → 4NO + 6H2O What is the maximum amount of water that may be produced if 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react?

Accepted Answer

A)  1.56mol
B)  1.88 mol
C)  3.52 mol
D)  3.91 mol
E)  2.35 molF) B) and E)
G) All of the above

Question 14

How much heat is evolved if 0.600 kg of SO2 is burned in excess oxygen? 2SO2(g)  + O2(g)  → 2SO3(g)  heat of reaction = −198 kJ/mol

Accepted Answer

A)  5.46 × 10−2 kJ
B)  927 kJ
C)  1.85 × 103 kJ
D)  59,400 kJ
E)  3.71 × 103 kJF) D) and E)
G) C) and D)

Question 15

What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?

Accepted Answer

A)  12.8 g
B)  25.6 g
C)  6.39 g
D)  0.399 g
E)  51.1 gF) A) and B)
G) C) and E)

Question 16

How many grams of lead(II)  chloride is produced if 13.87 g lead(II)  nitrate combines with excess hydrochloric acid to produce lead(II)  chloride and nitric acid?

Accepted Answer

A)  5.82 g
B)  14.33 g
C)  0.086 g
D)  11.64 g
E)  16.52 gF) B) and D)
G) B) and C)

Question 17

The combustion of pentane produces heat according to the following thermochemical equation.C5H 12(l)  + 8O2(g)  → 5CO2(g)  + 6H2O(l)  heat of reaction = −3510 kJ/mol How many grams of CO2 is produced per 2.50 × 103 kJ of heat released?

Accepted Answer

A)  6.27 g
B)  31.3 g
C)  61.8 g
D)  157 g
E)  220 gF) None of the above
G) All of the above

Question 18

If 119.3 g of PCl5 are formed from the reaction of 61.3 g Cl2 with excess PCl3, what is the percent yield? PCl3(g)  + Cl2(g)  → PCl5(g)

Accepted Answer

A)  94.6%
B)  66.3%
C)  57.3%
D)  51.3%
E)  48.6%F) B) and D)
G) A) and D)

Question 19

Given the following reaction, how much AgCl (in g)  can be formed from 25.0 mL of 0.115 M AgNO3 and 45.0 mL of 0.0533 M MgCl2? 2AgNO3(aq)  + MgCl2(aq)  → 2AgCl(s)  + Mg(NO3) 2(aq)

Accepted Answer

A)  0.344 g
B)  0.688 g
C)  1.10 g
D)  0.412 g
E)  0.276 gF) A) and B)
G) C) and E)

Question 20

How much heat is released if 35.0 g of ethanol (C2H5OH)  burns in excess oxygen? C2H5OH(l)  + 3O2(g)  → 2CO2(g)  + 3H2O(l)  heat of reaction = −1367 kJ/mol

Accepted Answer

A)  1797 kJ
B)  1367 kJ
C)  9.61 × 10−4 kJ
D)  4.78 × 104 kJ
E)  1040 kJF) A) and B)
G) A) and C)

Exam 11: Using Balanced Chemical Equations

What volume of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 in excess HCl(aq) ? MnO2(s) + 4HCl(aq) → MnCl2(aq) + 2H2O(l) + Cl2(g) (R = 0.08206 L • atm/K • mol)

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What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?

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Zinc dissolves in hydrochloric acid to yield hydrogen gas as follows: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) What mass of hydrogen gas is produced when a 7.35-g sample of zinc dissolves in 500.mL of 1.200 M HCl?

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Aluminum reacts with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis) . Al(s) + Br2(l) → Al2Br6(s) [unbalanced] How many moles of Al are needed to form 2.43 mol of Al2Br6?

Correct AnswerverifiedShow Answer

How much heat is released if 35.0 g of ethanol (C2H5OH) burns in excess oxygen? C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) heat of reaction = −1367 kJ/mol

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What mass of precipitate forms when 25.0 mL of 0.147 M NiCl2 solution reacts with excess sodium phosphate according to the given balanced chemical equation. 3NiCl2(aq) + 2Na3PO4(aq) → Ni3(PO4) 2(s) + 6NaCl(aq)

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Magnesium metal (0.100 mol) and hydrochloric acid (0.500 mol HCl) are combined and react to completion.What volume of hydrogen gas, measured at STP, is produced? Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g of sulfur tetrafluoride? 3SCl2(l) + 4NaF(s) → SF4(g) + S2Cl2(l) + 4NaCl(s)

Correct AnswerverifiedShow Answer

The combustion of pentane produces heat according to the following thermochemical equation.C5H 12(l) + 8O2(g) → 5CO2(g) + 6H2O(l) heat of reaction = −3510 kJ/mol How many grams of CO2 is produced per 2.50 × 103 kJ of heat released?

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Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows: 4NH3 + 5O2 → 4NO + 6H2O What is the maximum amount of water that may be produced if 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react?

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How many grams of lead(II) chloride is produced if 13.87 g lead(II) nitrate combines with excess hydrochloric acid to produce lead(II) chloride and nitric acid?

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Phosphine, an extremely poisonous and highly reactive gas, reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced] Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.

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Given the following reaction, how much AgCl (in g) can be formed from 25.0 mL of 0.115 M AgNO3 and 45.0 mL of 0.0533 M MgCl2? 2AgNO3(aq) + MgCl2(aq) → 2AgCl(s) + Mg(NO3) 2(aq)

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What mass of Cr can be produced by the reaction of 44.1 g of Cr2O3 with 35.0 g of Al according to the following chemical equation? 2Al + Cr2O3 → Al2O3 + 2Cr

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If 119.3 g of PCl5 are formed from the reaction of 61.3 g Cl2 with excess PCl3, what is the percent yield? PCl3(g) + Cl2(g) → PCl5(g)

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The first step in the Ostwald process for producing nitric acid is as follows: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) . If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction?

Correct AnswerverifiedShow Answer

What volume of CO2 gas at 645 torr and 800.K could be produced by the decomposition of 45.0 g of CaCO3? CaCO3(s) → CaO(s) + CO2(g) (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Calculate the volume of H2(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with 50.0 g Zn(s) to give hydrogen gas and aqueous zinc chloride. (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Lead(II) sulfide was once used in glazing earthenware.It will also react with hydrogen peroxide to form lead(II) sulfate and water.How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?

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How much heat is evolved if 0.600 kg of SO2 is burned in excess oxygen? 2SO2(g) + O2(g) → 2SO3(g) heat of reaction = −198 kJ/mol

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What volume of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO₂ in excess HCl(aq) ? MnO₂(s) + 4HCl(aq) → MnCl₂(aq) + 2H₂O(l) + Cl₂(g) (R = 0.08206 L • atm/K • mol)

Correct Answer
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Correct Answer
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Zinc dissolves in hydrochloric acid to yield hydrogen gas as follows: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) What mass of hydrogen gas is produced when a 7.35-g sample of zinc dissolves in 500.mL of 1.200 M HCl?

Correct Answer
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Aluminum reacts with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis) . Al(s) + Br₂(l) → Al₂Br₆(s) [unbalanced] How many moles of Al are needed to form 2.43 mol of Al₂Br₆?

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How much heat is released if 35.0 g of ethanol (C₂H₅OH) burns in excess oxygen? C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) heat of reaction = −1367 kJ/mol

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What mass of precipitate forms when 25.0 mL of 0.147 M NiCl₂ solution reacts with excess sodium phosphate according to the given balanced chemical equation. 3NiCl₂(aq) + 2Na₃PO₄(aq) → Ni₃(PO₄) ₂(s) + 6NaCl(aq)

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Magnesium metal (0.100 mol) and hydrochloric acid (0.500 mol HCl) are combined and react to completion.What volume of hydrogen gas, measured at STP, is produced? Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) (R = 0.08206 L • atm/K • mol)

Correct Answer
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What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g of sulfur tetrafluoride? 3SCl₂(l) + 4NaF(s) → SF₄(g) + S₂Cl₂(l) + 4NaCl(s)

Correct Answer
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The combustion of pentane produces heat according to the following thermochemical equation.C₅H ₁₂(l) + 8O₂(g) → 5CO₂(g) + 6H₂O(l) heat of reaction = −3510 kJ/mol How many grams of CO₂ is produced per 2.50 × 10³ kJ of heat released?

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Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows: 4NH₃ + 5O₂ → 4NO + 6H₂O What is the maximum amount of water that may be produced if 40.0 g NH₃ and 50.0 g O₂ are mixed and allowed to react?

Correct Answer
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Correct Answer
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Phosphine, an extremely poisonous and highly reactive gas, reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH₃(g) + O₂(g) → P₄O₁₀(s) + H₂O(g) [unbalanced] Calculate the mass of P₄O₁₀(s) formed when 225 g of PH₃ reacts with excess oxygen.

Correct Answer
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Given the following reaction, how much AgCl (in g) can be formed from 25.0 mL of 0.115 M AgNO₃ and 45.0 mL of 0.0533 M MgCl₂? 2AgNO₃(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO₃) ₂(aq)

Correct Answer
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What mass of Cr can be produced by the reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al according to the following chemical equation? 2Al + Cr₂O₃ → Al₂O₃ + 2Cr

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If 119.3 g of PCl₅ are formed from the reaction of 61.3 g Cl₂ with excess PCl₃, what is the percent yield? PCl₃(g) + Cl₂(g) → PCl₅(g)

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The first step in the Ostwald process for producing nitric acid is as follows: 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g) . If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction?

Correct Answer
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What volume of CO₂ gas at 645 torr and 800.K could be produced by the decomposition of 45.0 g of CaCO₃? CaCO₃(s) → CaO(s) + CO₂(g) (R = 0.08206 L • atm/K • mol)

Correct Answer
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Calculate the volume of H₂(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with 50.0 g Zn(s) to give hydrogen gas and aqueous zinc chloride. (R = 0.08206 L • atm/K • mol)

Correct Answer
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Correct Answer
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How much heat is evolved if 0.600 kg of SO₂ is burned in excess oxygen? 2SO₂(g) + O₂(g) → 2SO₃(g) heat of reaction = −198 kJ/mol

Correct Answer
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