Stoichiometric Calculations – Ch9 | Test Bank – 15th Ed

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Package Title: Hein Test Bank

Course Title: Hein 15e

Chapter Number: 9

Question type: Multiple Choice

1) Based on the following chemical equation: 2 C₆H₆ + 15 O₂ 12 CO₂ + 6 H₂O, calculate the number of moles of CO₂ that will be formed when 8.90 mol of H₂O are produced?

a) 1.07 10²⁵ mol

b) 4.45 mol

c) 17.8 mol

d) 2.68 10²⁴ mol

Difficulty: easy

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

2) How many moles of hydrogen gas will be produced when 12 g of Mg will react completely with excess of an acid according to the following reaction?
2 Mg + 2 HCl 2 MgCl2 + H2

a) 1.0 mol

b) 0.50 mol

c) 1.5 mol

d) 0.25 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

3) How many moles of sulfur trioxide will be produced when the complete combustion of 100.0 g of sulfur dioxide takes place? The product of this reaction is sulfur trioxide.

a) 0.7804 mol

b) 1.561 mol

c) 0.641 mol

d) 1.281 mol

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

4) How many grams of molecular chlorine will be required to completely react with 0.0223 mol of sodium iodide according to the following reaction?
2 NaI + Cl2 2 NaCl + I2

a) 1.57 10^-4 g

b) 3.16 g

c) 0.0112 g

d) 0.791 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

5) How many grams of water will be required to completely react with 1.00 mol of CaO according to the following reaction?
CaO + H2O Ca(OH)2

a) 5.55 g

b) 0.0555 g

c) 18.0 g

d) 1.00 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

6) What mass of sodium hydroxide will neutralize completely 3.612 mol of HCl?

a) 3.612 g

b) 144.5 g

c) 11.07 g

d) 0.09030 g

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

7) If 1.5 moles of oxygen combine with aluminum to form Al₂O₃ then mass of aluminum metal used in this reaction is_______.

a) 27 g

b) 1.0 g

c) 54 g

d) 40.5 g

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

8) How many moles of benzene (C6H6) should be completely combusted in order to produce 0.4000 mol of carbon dioxide?
2C6H6 + 15O2 12CO2 + 6 H2O

a) 4.800 mol

b) 0.2000 mol

c) 2.400 mol

d) 0.06667 mol

Difficulty: easy

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

9) What mass of sodium hydroxide will completely neutralize 2.5 mol of sulfuric acid?

a) 2.50 g

b) 100. g

c) 50.0 g

d) 200. g

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

10) How many molecules of hydrogen will be required to react completely with 0.600 mol of H₂ in order to form water?

a) 0.300 molecules

b) 7.23 10²³ molecules

c) 1.81 10²³ molecules

d) 3.61 10²³ molecules

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

11) Consider the following unbalanced equation. How many molecules of hydrogen will be required to produce 1.60 mol of water?

H2 + O2 H2O

a) 4.82 10²³ molecules

b) 9.64 10²³ molecules

c) 1.93 10²⁴ molecules

d) 0.800 molecules

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

12) How many moles of iron(III) oxide are required to completely react with 1.40 1022 atoms of carbon in the following reaction?

Fe₂O₃ + 3C 2Fe + 3CO

a) 0.0232 mol

b) 0.00775 mol

c) 0.0697 mol

d) 4.67 10²¹ mol

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

13) How many grams of O2 are required to produce 1.23 1024 molecules of water?

2H₂ + O₂ 2H₂O

a) 32.7 g

b) 131 g

c) 65.4 g

d) 16.3 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

14) How many grams of sodium iodide are required to react completely with 3.01 1023 molecules of chlorine?

2 NaI + Cl₂ I₂ + 2 NaCl

a) 1.50 g

b) 37.5 g

c) 150. g

d) 74.9 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

15) What mass of sodium hydroxide will be required to neutralize completely 1.60 10²³ molecules of HCl?

a) 10.6 g

b) 16.5 g

c) 38.5 g

d) 64.0 g

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

16) What mass of sodium chloride will be required to completely react with 4.00 10²⁴ formula units of AgNO₃ and form AgCl and sodium nitrate?

a) 6.64 g

b) 0.114 g

c) 388 g

d) 8.80 g

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

17) How many grams of silver oxide are produced on complete combustion of 2.76 g of silver carbonate?

a) 2.48 g

b) 2.16 g

c) 2.32 g

d) 2.64 g

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

18) Calculate the number of moles of excess reactant that will be left-over when 50.0 g of KI react with 50.0 g of Br2:

2KI + Br₂ 2KBr + I₂

a) both reactants are consumed completely

b) 0.145 mol

c) 0.0117 mol

d) 0.162 mol

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

19) How many moles of Ba3(PO4)2 can be produced when 0.50 moles of BaCl2 is mixed with 0.20 moles of Na3PO4 according to the following reaction:

3BaCl₂ + 2Na₃PO₄ Ba₃(PO₄)₂ + 6NaCl

a) 0.70 mol

b) 0.50 mol

c) 0.30 mol

d) 0.10 mol

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

20) Calculate the number of moles of excess reactant that will be left-over when 56.0 g of CaCl2 react with 64.0 g of Na2SO4:

CaCl₂ + Na₂SO₄ CaSO₄ + 2NaCl

a) 0.0540 mol

b) 0.0798 mol

c) 0.291 mol

d) both reactants are consumed completely

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

21) Based on the following chemical equation: 2 H₂ + O₂ 2 H₂O:

Identify the limiting reactant when 32.0 g hydrogen is allowed to react with 16.0 g oxygen.

a) hydrogen

b) oxygen

c) water

d) both reactants are consumed completely

Difficulty: medium

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

22) Based on the following chemical equation: 4 HCN + 5 O₂ 2 N₂ + 4 CO₂ + 2 H₂O. Identify the limiting reactant and the mass of N₂ produced when 100. g of HCN react with 100. g of O₂.

a) the limiting reactant is HCN and 25.9 g of N₂ are produced

b) the limiting reactant is O₂ and 35.0 g of N₂ are produced

c) the limiting reactant is HCN and 51.8 g of N₂ are produced

d) both reactants are consumed completely

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

23) Calculate the number of moles of excess reactant that will be left-over when 0.350 g of HCN react with 0.0156 mol of O2:

4 HCN + 5 O₂ 2 N₂ + 4 CO₂ + 2 H₂O

a) 0.150 mol

b) 3.24 10³ mol

c) 4.50 10⁴ mol

d) 5.62 10⁴ mol

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

24) For the balanced reaction of: N₂ + 3H₂ 🡪 2NH₃. What is the mass of the excess reagent when 84.06g of N₂ and 22.18g of H₂ are combined?

a) 19.15 g

b) 16.13 g

c) 44.25 g

d) 4.03 g

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

25) For the reaction: N₂ + H₂ 🡪 NH₃. Which of the following is the limiting reactant if 78 g of N₂ and 26 g of H₂ are combined?

a) N₂

b) H₂

c) NH₃

d) None of these choices.

Difficulty: medium

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

26) How many moles of NH3 will be produced when 1.60 mol of N2 react with excess of hydrogen gas according to the following reaction?

N₂ + 3H₂ → 2NH₃

a) 0.533 mol

b) 1.60 mol

c) 3.20 mol

d) 4.80 mol

Difficulty: easy

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

27) How many moles of Al in reaction with excess of oxygen will be consumed when 0.400 mol of Al2O3 are produced in the following equation?

4Al + 3O₂ → 2Al₂O₃

a) 0.200 mol

b) 0.400 mol

c) 0.600 mol

d) 0.800 mol

Difficulty: easy

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

28) How many moles of propane (C3H8) are required to react completely with 3.00 mol of oxygen in the following equation?

C₃H₈ + 5O₂ → 3CO₂ + 9H₂O

a) 0.600 mol

b) 1.67 mol

c) 1.00 mol

d) 0.67 mol

Difficulty: easy

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

29) How many moles of C3H6 will be consumed when 4.11 mol of CO2 are produced in the following equation?

2C₃H₆ + 9O₂ → 6CO₂ + 6H₂O

a) 1.37 mol

b) 4.11 mol

c) 6.00 mol

d) 12.3 mol

Difficulty: easy

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

30) How many moles of Cl2 are consumed in reaction with excess of Al when 0.500 mol of AlCl3 are produced in the following equation?

2Al + 3Cl₂ → 2AlCl₃

a) 0.333 mol

b) 0.500 mol

c) 0.750 mol

d) 1.00 mol

Difficulty: easy

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

31) How many moles of H2O are produced when 3.01 1023 molecules of C3H6 react completely in the following equation?

2C₃H₆ + 9O₂ → 6CO₂ + 6H₂O

a) 0.167 mol

b) 1.50 mol

c) 1.51 10²³ mol

d) 2.01 10²³ mol

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

32) How many moles of C3H8 are consumed when 1.81 1023 molecules of CO2 are produced in the following equation?

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

a) 0.100 mol

b) 0.897 mol

c) 6.03 10²² mol

d) 5.43 10²³ mol

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

33) How many moles of H2O are produced when 1.60 1022 molecules of O2 react completely in the following equation?

2C₂H₂ + 5O₂ → 4CO₂ + 2H₂O

a) 0.0106 mol

b) 0.0664 mol

c) 2.41 10²³ mol

d) 1.51 10²⁴ mol

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

34) Given the balanced reaction: 4NH₃ + 5O₂ 🡪 4NO + 6H₂O; If 2.50 g of NH₃ and 2.85 g of O₂ are combined, which of the below is correct?

a) NH₃ is the limiting reactant and 4.14 g of NO are produced

b) NH₃ is the limiting reactant and 1.10 g of NO are produced

c) O₂ is the limiting reactant and 2.14 g of NO are produced

d) O₂ is the limiting reactant and 4.28 g of NO are produced

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

35) For the balanced reaction: 2NH₃ + CO₂ 🡪 CH₄N₂O + H₂O. If 136.4 g of NH₃ react with excess amount of CO₂ to produce 168.4 g of CH₄N₂O, what is the percent yield for this reaction?

a) 80.10%

b) 70.03%

c) 56.71%

d) 61.29%

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

36) How many moles of carbon dioxide are produced when 9.03 1023 molecules of oxygen react completely in the following equation?

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

a) 0.600 mol

b) 1.67 mol

c) 0.900 mol

d) 2.50 mol

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

37) How many moles of hydrogen gas are produced when 1.60 1024 molecules of HCl react with excess of Zinc in the following equation?

Zn + 2HCl → ZnCl₂ + H₂

a) 1.33 mol

b) 2.66 mol

b) 3.99 mol

d) 5.32 mol

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

38) How many molecules of NH3 are produced when 3.00 mol of H2 react completely in the following equation?

N₂ + 3H₂ → 2NH₃

a) 0.667 molecules

b) 1.50 molecules

c) 1.20 10²⁴ molecules

d) 2.71 10²⁴ molecules

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

39) How many molecules of sulfur trioxide are produced when 1.62 mol of oxygen react completely in the following equation?

S₈ + 12O₂ → 8SO₃

a) 1.08 molecules

b) 2.43 molecules

c) 6.50 10²³ molecules

d) 1.46 10²⁴ molecules

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

40) How many molecules of water are produced when 3.00 mol of copper react completely in the following equation?

Cu + 2H₂SO₄ → CuSO₄ + 2H₂O + SO₂

a) 9.03 10²³ molecules

b) 3.61 10²⁴ molecules

c) 1.20 10²⁴ molecules

d) 2.71 10²⁴ molecules

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

41) Given the reaction magnesium and iron(III) chloride forming magnesium chloride and elemental iron, which of the following is correct is 41.0 g of magnesium and 175 g of iron(III) chloride are combined?

a) Iron(III) chloride is the limiting reactant and 1.67g of magnesium are left in excess.

b) Iron(III) chloride is the limiting reactant and 14.8g of magnesium are left in excess.

c) Magnesium is the limiting reactant and 10.3g of iron(III) chloride are left in excess.

d) Magnesium is the limiting reactant and 10.3g of iron(III) chloride are left in excess.

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

42) How many atoms of carbon are needed to completely react with 2.00 mol of chlorine according to the following equation?

C + 2Cl₂ → CCl₄

a) 3.01 10²³ atoms

b) 6.02 10²³ atoms

c) 1.20 10²⁴ atoms

d) 2.41 10²⁴ atoms

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

43) How many molecules of O2 are produced when 0.500 mol of P4O10 react completely in the following equation?

P₄O₁₀ → 4P + 5O₂

a) 1.21 10²⁴ molecules

b) 1.51 10²⁴ molecules

c) 6.02 10²⁴ molecules

d) 3.01 10²⁴ molecules

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

44) How many molecules of O2 are consumed when 1.00 mol of N2O5 is produced in the following equation?

2N₂ + 5O₂ → 2N₂O₅

a) 3.01 10²⁴ molecules

b) 1.20 10²⁴ molecules

c) 2.41 10²³ molecules

d) 1.51 10²⁴ molecules

Difficulty: medium

Learning Objective 1: Solve problems where the reactants and products are both in moles.

Section Reference 1: Section 9.2

45) What mass of HCl is produced when 3.00 mol of Cl2 react completely in the following equation?

H₂ + Cl₂ → 2 HCl

a) 54.7 g

b) 72.9 g

c) 109 g

d) 219 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

46) What mass of H2O is produced when 0.400 mol of KOH react completely in the following equation?

KOH + HCl → KCl + H₂O

a) 7.21 g

b) 18.0 g

c) 45.1 g

d) 90.2 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

47) What mass of limestone (CaCO₃) on heating will produce 56.00 kg of CaO according to the following reaction?

CaCO₃→ CaO + CO₂

a) 1000. kg

b) 56.00 kg

c) 44.00 g

d) 100.0 kg

Difficulty: hard

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

48) What mass of carbon monoxide is produced when 1.50 mol of oxygen react completely in the following equation?

2C + O₂ → 2CO

a) 84.0 g

b) 42.0 g

c) 28.0 g

d) 21.0 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

49) What mass of carbon dioxide is produced when 3.00 mol of oxygen react completely in the following equation?

2CO + O₂ → 2CO₂

a) 88.0 g

b) 44.0 g

c) 29.3 g

d) 264 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

50) How many grams of hydrogen gas would be produced when 6.0 grams of magnesium reacts with excess of an acid?

Mg + 2HCl → MgCl₂ + H₂

a) 0.50 g

b) 1.0 g

c) 2.0 g

d) 4.0 g

Difficulty: easy

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

51) What mass of hydrogen is produced when 0.400 mol of water react completely in the following equation?

2Na + 2H₂O → 2NaOH + H₂

a) 0.323 g

b) 1.62 g

c) 0.404 g

d) 2.02 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

52) What mass of NH3 is produced when 1.20 mol of N2 react completely in the following equation?

N₂ + 3H₂ → 2NH₃

a) 40.8 g

b) 20.4 g

c) 13.6 g

d) 30.7 g

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

53) Given the balanced reaction: 2 Al + Fe₂O₃ 🡪 Al₂O₃ + 2 Fe. If 4.85 mol of Al react with 3.76 mol of Fe₂O₃, which of the following is correct?

a) 1.47 mol of Fe are produced and 3.76 mol of Al are present in excess.

b) 4.85 mol of Fe are produced and 1.34 mol of Fe₂O₃ are in present in excess.

c) 4.85 mol of Fe are produced and 2.43 mol of Fe₂O₃ are present in excess.

d) 2.43 mol of Fe are produced and 2.29 mol of Fe₂O₃ are present in excess.

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

54) How many moles of carbon monoxide are produced when 40.0 g of oxygen react completely in the following equation?

2 C + O₂ → 2 CO

a) 0.625 mol

b) 1.25 mol

c) 2.50 mol

d) 80.0 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

55) How many moles of oxygen are consumed when 38.0 g of aluminum oxide are produced in the following equation?

4 Al + 3 O₂ → 2 Al₂O₃

a) 0.248 mol

b) 0.559 mol

c) 1.50 mol

d) 3.00 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

56) How many moles of N2O5 are produced when 3.00 g of O2 react completely in the following equation?

2 N₂ + 5 O₂ → 2 N₂O₅

a) 0.0375 mol

b) 0.0750 mol

c) 0.234 mol

d) 0.469 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

57) How many moles of CO2 are produced when 45.0 g of C6H6 react completely in the following equation?

2 C₆H₆ + 15 O₂ → 12 CO₂ + 6 H₂O

a) 0.0960 mol

b) 0.289 mol

c) 3.46 mol

d) 10.4 mol

­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­­

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

58) How many moles of K2S are consumed when 14.0 g of KBr is formed in the following equation?

FeBr₂ + K₂S → 2 KBr + FeS

a) 0.0588 mol

b) 0.235 mol

c) 4.25 mol

d) 17.0 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

59) How many moles of CO2 are consumed when 22.0 g of NH3 react completely in the following equation?

CO₂ + 2 NH₃ → CO(NH₂)₂ + H₂O

a) 0.387 mol

b) 0.646 mol

c) 1.55 mol

d) 2.58 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

60) How many moles of Al(OH)3 are produced when 50.0 g of KOH react completely in the following equation?

AlCl₃ + 3 KOH → Al(OH)₃ + 3 KCl

a) 0.297 mol

b) 0.374 mol

c) 2.67 mol

d) 3.37 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

61) How many moles of carbon dioxide are produced when 12.0 g of oxygen react completely in the following equation?

C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O

a) 0.225 mol

b) 0.450 mol

c) 0.625 mol

d) 1.25 mol

Difficulty: medium

Learning Objective 1: Solve problems where the mass is given and the answer is to be determined in moles or the moles are given and mass is to be determined.

Section Reference 1: Section 9.3

62) What mass of oxygen is consumed when 54.0 g of water is produced in the following equation?

2 H₂ + O₂ → 2 H₂O

a) 0.167 g

b) 0.667 g

c) 1.50 g

d) 47.9 g

Difficulty: medium

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

63) What mass of CO2 is produced when 50.0 g of C2H4 reacts completely in the following equation?

C₂H₄ + 3 O₂ → 2 CO₂ + 2 H₂O

a) 12.3 g

b) 39.2 g

c) 49.4 g

d) 157 g

Difficulty: medium

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

64) What mass of CO2 will be produced when 100. g of C8H18 react completely in the following equation?

2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

a) 0.00249 g

b) 6.29 g

c) 308 g

d) 402 g

Difficulty: medium

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

65) What mass of H2O is produced when 12.0 g of HCl react completely in the following equation?

6 HCl + Fe₂O₃ → 2F eCl₃ + 3 H₂O

a) 2.97 g

b) 39.4 g

c) 27.4 g

d) 110. g

Difficulty: medium

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

66) What mass of oxygen is consumed when 100. g of nitrogen react completely in the following equation?

N₂ + O₂ → 2 NO

a) 0.112 g

b) 64.0 g

c) 100. g

d) 114 g

Difficulty: medium

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

67) When 22.0 g of NaOH and 21.0 g of H₂SO₄ are mixed and react according to the reaction:

2 NaOH + H₂SO₄ 🡪 Na₂SO₄ + 2 H₂O, which is the limiting reagent?

a) NaOH

b) H₂SO₄

c) Na₂SO₄

d) Neither reagent is limiting.

Difficulty: medium

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

68) What is the mass of the excess reactant remaining at the end of the reaction of 90.0 g of SO₂ and 100. g of O₂ to form sulfur trioxide?

a) 11.5g

b) 22.5g

c) 67.5g

d) 77.5g

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

69) Which is the limiting reactant when 12.0 mol of CH4 are reacted with 20.0 mol of O2 in the following equation?

CH₄ + 2 O₂ → CO₂ + 2 H₂O

a) CH₄

b) O₂

c) CO₂

d) H₂O

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

70) Which is the limiting reactant when 3.00 mol of calcium are reacted with 8.00 mol of water in the following equation?

Ca + 2 H₂O → Ca(OH)₂ + H₂

a) Ca

b) H₂O

c) Ca(OH)₂

d) H₂

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

71) Which is the limiting reactant when 3.00 mol of copper are reacted with 3.00 mol of silver nitrate in the following equation?

Cu + 2 AgNO₃ → Cu(NO₃)₂ + 2 Ag

a) Cu

b) AgNO₃

c) Cu(NO₃)₂

d) Ag

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

72) Which is the excess reactant when 3.00 mol of MnO2 are reacted with 10.0 mol of HCl in the following equation?

MnO₂ + 4HCl → MnCl₂ + 2H₂O + Cl₂

a) MnO₂

b) HCl

c) MnCl₂

d) H₂O

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

73) Which substance is in excess when 6.00 mol of aluminum are reacted with 12.00 mol of oxygen in the following equation?

alumium + oxygen gas 🡪 alumium oxide

a) aluminum

b) oxygen

c) aluminum oxide

Difficulty: medium

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

74) Which substance is the limiting reactant when 2.00 mol of cobalt are reacted with 1.50 mol of lead(II) chloride in the following equation?

Co + PbCl₂ → CoCl₂ + Pb

a) Co

b) PbCl₂

c) CoCl₂

d) Pb

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

75) Which substances are in excess when 3.00 mol of Pb, 1.50 mol of PbO2, and 5.00 mol of H2SO4 are reacted in the following equation?

Pb + PbO₂ + 2 H₂SO₄ → 2 PbSO₄ + 2 H₂O

a) Pb and PbO₂

b) Pb and H₂SO₄

c) PbO₂ and H₂SO₄

d) PbSO₄ and H₂O

Difficulty: medium

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

76) Which substance is in excess when 1.50 mol of aluminum bromide are reacted with 2.50 mol of barium hydroxide in the following equation?

2 AlBr₃ + 3 Ba(OH)₂ → 3 BaBr₂ + 2 Al(OH)₃

a) BaBr₂

b) Al(OH)₃

c) Ba(OH)₂

d) AlBr₃

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

77) In a reaction to produce sulfuric acid, the theoretical yield is 300. g. What is the percent yield if the actual yield is 280. g?

a) 6.67%

b) 7.14%

c) 93.3%

d) 107%

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

78) In a reaction to produce ammonia, the theoretical yield is 420. g. What is the percent yield if the actual yield is 350. g?

a) 83.3%

b) 20.0%

c) 16.7%

d) 120.%

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

79) In a reaction to produce chlorine gas, the theoretical yield is 25.6 g. What is the percent yield if the actual yield is 20.2 g?

a) 21.1%

b) 127%

c) 20.2%

d) 78.9%

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

80) In a reaction to produce iron the theoretical yield is 340 kg. What is the percent yield if the actual yield is 300. kg?

a) 13.3%

b) 88.2%

c) 11.8%

d) 113%

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

81) What is the percent yield for a reaction in which 24.6 g of a product is actually produced when the theoretical yield is 30.0 g?

a) 82.0%

b) 122%

c) 21.0%

d) 18.0%

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

82) Consider the following reaction: PCl₃ + Cl₂ 🡪 PCl₅. If the percent yield is 66.3%, what mass of PCl₅ is actually formed when 61.3 g of Cl₂ reacts with excess PCl₃?

a) 40.6 g

b) 92.5 g

c) 119. g

d) 145. g

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

83) What is the percent yield in a reaction in which 1.038 g of a product is actually produced when the theoretical yield is 1.132 g?

a) 8.304%

b) 109.1%

c) 89.16%

d) 91.70%

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

84) Calculate the percent yield for the following reaction if 233 g of NO2 reacted and 175 g of HNO3 were produced.

3 NO₂ + H₂O 2 HNO₃ + NO

a) 75.1%

b) 82.2%

c) 27.4%

d) 60.8%

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

85) Calculate the percent yield for the following reaction if 76.8 g of H2O reacted and 125 g of NO were produced.

3 NO₂ + H₂O 2 HNO₃ + NO

a) 99.0%

b) 61.4%

c) 60.0%

d) 97.7%

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

86) Calculate how much acetylene (C2H2) will be produced from 358 g of H2O and an excess of CaC2 if the percent yield for this reaction is 94.5%.

CaC₂ + 2 H₂O C₂H₂ + Ca(OH)₂

a) 338 g

b) 489 g

c) 244 g

d) 259 g

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

87) Calculate how much ethanol, C2H5OH, will be produced from the reaction of 590. g of sugar (C6H12O6) if the reaction has a 88.5% yield.

C₆H₁₂O₆ 2C₂H₅OH + 2CO₂

a) 302 g

b) 170. g

c) 267 g

d) 134 g

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Question type: True/False

88) The limiting reactant in a chemical reaction is the reactant, which is completely consumed first.

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

89) The limiting reagent limits the amount of product formed in a chemical reaction.

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

90) In all chemical reactions, the reactants are always completely consumed.

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

91) When carbon combines with oxygen gas to from carbon dioxide, the mole ratio of carbon to oxygen is 1:2.

Difficulty: medium

Learning Objective 1: Define stoichiometry and describe the strategy required to solve problems based on chemical equations

Section Reference 1: Section 9.1

92) The equation for a reaction should be balanced before doing stoichiometric calculations.

Difficulty: easy

Learning Objective 1: Define stoichiometry and describe the strategy required to solve problems based on chemical equations

Section Reference 1: Section 9.1

93) The limiting reactant in a chemical reaction limits the amount of reactant that can be consumed

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

94) In all chemical reactions the percent yield is approximately 50%.

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

95) The percent yield is the maximum amount of product that can be produced from a given amount of reactant.

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

96) A mole ratio is used to convert the given number of moles of one substance to the unknown number of moles of a second substance.

Difficulty: easy

Learning Objective 1: Define stoichiometry and describe the strategy required to solve problems based on chemical equations

Section Reference 1: Section 9.1

97) The percent yield of a reaction can be used as a measure of how efficient the chemical change is.

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

98) In every chemical reaction the number of moles of reactant must equal the number of moles of product.

Difficulty: easy

Learning Objective 1: Define stoichiometry and describe the strategy required to solve problems based on chemical equations

Section Reference 1: Section 9.1

99) A mole ratio is the ratio between the number of moles of any two species involved in the chemical reaction.

Difficulty: easy

Learning Objective 1: Define stoichiometry and describe the strategy required to solve problems based on chemical equations

Section Reference 1: Section 9.1

100) The reactant present in the fewest number of moles is always the limiting reactant.

Difficulty: easy

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Question type: Essay

101) When limestone (calcium carbonate) is reacted with hydrochloric acid the products are calcium chloride, water, and carbon dioxide.
a) Write a balanced chemical equation for this reaction.
b) What mass of calcium carbonate will be consumed when 20.0 g of hydrochloric acid react completely in this reaction?
c) What mass of carbon dioxide will be produced when 20.0 g of hydrochloric acid react completely in this reaction?

Difficulty: hard

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

Solution: a) CaCO₃ + 2 HCl → CaCl₂ + H₂O + CO₂; c) 27.5g of calcium carbonate will be consumed; c) 12.1 g of carbon dioxide will be produced

102) When limestone (calcium carbonate) is heated it decomposes to form lime (calcium oxide) and carbon dioxide.
a) Write a balanced chemical equation for this reaction.
b) What mass of lime will be produced from the complete decomposition of 100. g of limestone?
c) What mass of carbon dioxide will be produced from the complete decomposition of 100. g of limestone?

Difficulty: hard

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

Solution: a) CaCO₃ → CaO + CO₂; b) 56.0 g of lime will be produced; c) 44.0 g of carbon dioxide will be produced

103) Dinitrogen tetroxide can be decomposed to form nitrogen dioxide.
a) Write a balanced chemical equation for this reaction.
b) What is the mass, in grams, of dinitrogen tetroxide needed to produce 1.000 kg of nitrogen dioxide?

Difficulty: hard

Learning Objective 1: Solve problems where mass is given and the answer is to be determined as mass.

Section Reference 1: Section 9.4

Solution: a) N₂O₄ → 2 NO₂; b) 1000. g of dinitrogen tetroxide is needed

104) The pollutant nitrogen monoxide can be reacted with ammonia to produce nitrogen gas and water.
a) Write a balanced chemical equation for this reaction.
b) In this equation, write the mole ratio of
1) nitrogen monoxide to ammonia
2) nitrogen monoxide to nitrogen gas
3) nitrogen monoxide to water
4) ammonia to nitrogen gas
5) ammonia to water
6) nitrogen gas to water

Difficulty: easy

Learning Objective 1: Define stoichiometry and describe the strategy required to solve problems based on chemical equations

Section Reference 1: Section 9.1

Solution: a) 6 NO + 4 NH₃ → 5 N₂ + 6 H₂O; b1) 6:4 or 3:2; b2) 6:5; b3) 6:6 or 1:1; b4) 4:5; b5) 4:6 or 2:3; b6) 5:6

105) Two solutions are combined in a beaker. One solution contains 200.0 g of lead(II) nitrate and the other contains 200.0 g of sodium sulfide. A double-displacement reaction occurs. What mass of each of the following substances remain when the reaction stops?
a) lead(II) nitrate
b) sodium sulfide
c) lead(II) sulfide
d) sodium nitrate

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Solution: a) approximately 0.000 g of lead(II) nitrate remain; b) 152.9 g of sodium sulfide remain; c) 144.5 g of lead(II) sulfide form; d) 102.7 g of sodium nitrate form

106) Two solutions are combined in a beaker. One solution contains 500.0 g of potassium phosphate and the other contains 500.0 g of calcium nitrate. A double-displacement reaction occurs. What mass of each of the following substances is present when the reaction stops.
a) potassium phosphate
b) calcium nitrate
c) calcium phosphate
d) potassium nitrate

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Solution: a) 68.82 g of potassium phosphate remain; b) approximately 0.000 g of calcium nitrate remain; c) 315.0 g of calcium phosphate form; d) 616.1 g of potassium nitrate form

107) Nitrogen gas combines with hydrogen gas to produce ammonia. 40.0 g of nitrogen is reacted with 10.0 g of hydrogen. The reaction proceeds until one reactant is completely consumed.
a) Write a balanced chemical equation for this reaction.
b) What is the theoretical yield of ammonia?
c) What is the percent yield of ammonia if 45.3 g is actually produced?

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Solution: a) N₂ + 3 H₂ → 2 NH₃; b) 48.7 g is the theoretical yield of ammonia; c) 93.0% yield

108) Sulfur dioxide reacts with oxygen to produce sulfur trioxide. 150. g of sulfur dioxide is reacted with 50.0 g of oxygen. The reaction proceeds until one reactant is completely consumed.
a) Write a balanced chemical equation for this reaction.
b) What is the theoretical yield of sulfur trioxide?
c) What is the percent yield of sulfur trioxide if 180. g is actually produced?

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Solution: a) 2 SO₂ + O₂ → 2S O₃; b) 187 g is the theoretical yield of sulfur trioxide; c) 96.3% yield

109) 12.0 g of copper is converted to copper(II) oxide by heating in oxygen.
a) Write a balanced chemical equation for this reaction.
b) What mass of oxygen is required to convert the 12.0 g of copper into copper(II) oxide?
c) What mass of copper(II) oxide will be theoretically produced?
d) What is the percent yield of copper(II) oxide if 12.8 g of copper(II) oxide is actually produced?

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Solution: a) 2 Cu + O₂ → 2 CuO; b) 3.02 g of oxygen are required; c) 15.0 g is the theoretical production of copper(II) oxide; d) 85.3% yield

110) Answer the following questions based on the diagram:

a) Complete the diagram showing the products formed from this combustion reaction.

b) Write a complete and balanced chemical equation for the reaction shown and identify the limiting reactant. Explain your reasoning in 1 – 2 sentences.

c) Assuming that each unit shown represents one mole of each compound, calculate the mass of the excess reactant that will remain once the reaction is complete.

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Solution: a)

b) CH₄ + 2O₂ CO₂ + 2H₂O; In the reaction shown, 4 molecules of CH₄ are combusted. Because of the stoichiometry for this reaction, 8 out of the 9 molecules of O₂ shown will react producing 4 molecules of CO₂ and 8 molecules of water, leaving one molecule of O₂ remaining. The limiting reactant is CH₄. c) 32 g

111) Consider the single-displacement reaction in which zinc metal displaces hydrogen from hydrochloric acid.
a) Write a complete and balanced chemical equation for this reaction.
b) If 3.4 10²³ zinc atoms react with 4.5 10²³ molecules of hydrochloric acid, calculate the mass of zinc chloride produced in this reaction.
c) Calculate the number of moles of the excess reactant that remain once the reaction stops.

Difficulty: hard

Learning Objective 1: Solve problems involving limiting reactants and yield.

Section Reference 1: Section 9.5

Solution: a) Zn + 2 HCl ZnCl₂ + H₂; b) 50.9 g; c) 0.191 mol