Question 1

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) C) and D)
G) B) and E)

Question 2

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) A) and C)
G) B) and E)

Question 3

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) A) and B)
G) C) and D)

Question 4

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) B) and C)
G) B) and E)

Question 5

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) B) and C)
G) A) and E)

Question 6

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) All of the above
G) A) and B)

Question 7

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 C)
G) A) and B)

Question 8

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) None of the above

Question 9

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 C)
G) All of the above

Question 10

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) C) and D)
G) A) and D)

Question 11

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) B) and E)
G) All of the above

Question 12

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) None of the above
G) A) and D)

Question 13

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) A) and D)
G) A) and C)

Question 14

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) B) and C)
G) A) and C)

Question 15

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) B) and E)
G) A) and E)

Question 16

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) A) and B)
G) All of the above

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) All of the above
G) B) and E)

Question 18

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) B) and C)
G) A) and E)

Question 19

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 D)

Question 20

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) All of the above
G) B) and C)

Exam 11: Using Balanced Chemical Equations

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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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 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)

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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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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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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?

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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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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)

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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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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)

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

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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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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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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 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)

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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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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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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 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)

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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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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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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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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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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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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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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)

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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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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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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?

Correct Answer
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Correct Answer
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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?

Correct Answer
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Correct Answer
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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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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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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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