Deck 4: Chemical Quantities and Aqueous Reactions

Question 1

According to the following reaction,what amount of Al₂S₃ remains when 20.00 g of Al₂S₃ and 2.00 g of H₂O are reacted? A few of the molar masses are as follows: Al₂S₃ = 150.17 g/mol,H₂O = 18.02 g/mol. Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

A) 28.33 g
B) 14.00 g
C) 8.33 g
D) 19.78 g
E) 17.22 g

Answer 1

17.22 g

Question 2

Two samples of potassium iodide are decomposed into their constituent elements.The first sample produced 13.0 g of potassium and 42.3 g of iodine.If the second sample produced 24.4 kg of potassium,how many kg of iodine were produced?

A) 13.3 kg
B) 22.5 kg
C) 79.4 kg
D) 44.4 kg
E) 92.4 kg

Answer 2

79.4 kg

Question 3

Determine the molarity of a solution formed by dissolving 4.00 moles of KBr in enough water to yield 3.00 L of solution.

A) 1.33 M
B) 2.00 M
C) 0.750 M
D) 3.00 M
E) 12.00 M

Answer 3

1.33 M

Question 4

Determine the molarity of a solution formed by dissolving 468 mg of MgI₂ in enough water to yield 50.0 mL of solution.

A) 0.0297 M
B) 0.0337 M
C) 0.0936 M
D) 0.0107 M
E) 0.0651 M

Question 5

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

A) 1.50 M
B) 1.18 M
C) 0.130 M
D) 0.768 M
E) 2.30 M

Question 6

Determine the theoretical yield of HCl if 60.0 g of BCl₃ and 37.5 g of H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is BCl₃ = 117.16 g/mol. BCl₃(g)+ 3 H₂O(l)→ H₃BO₃(s)+ 3 HCl(g)

A) 75.9 g HCl
B) 132 g HCl
C) 187 g HCl
D) 56.0 g HCl
E) 25.3 g HCl

Question 7

How many moles of nitrogen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol. 4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

A) 0.290 mol N₂
B) 0.580 mol N₂
C) 18.5 mol N₂
D) 0.724 mol N₂
E) 1.73 mol N₂

Question 8

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃).If it is the only product,what mass of PCl₃ is formed?

A) 30.15 g
B) 54.93 g
C) 140.01 g
D) 79.71 g
E) 91.86 g

Question 9

Determine the limiting reactant (LR)and the mass (in g)of nitrogen that can be formed from 50.0 g N₂O₄ and 45.0 g N₂H₄.Some possibly useful molar masses are as follows: N₂O₄ = 92.02 g/mol,N₂H₄ = 32.05 g/mol. N₂O₄(l)+ 2 N₂H₄(l)→ 3 N₂(g)+ 4 H₂O(g)

A) LR = N₂H₄, 59.0 g N₂ formed
B) LR = N₂O₄, 105 g N₂ formed
C) LR = N₂O₄, 45.7 g N₂ formed
D) LR = N₂H₄, 13.3 g N₂ formed
E) No LR, 45.0 g N₂ formed

Question 10

How many grams of Li₃N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6 Li(s)+ N₂(g)→ 2 Li₃N(s)

A) 18.3 g Li₃N
B) 20.3 g Li₃N
C) 58.3 g Li₃N
D) 61.0 g Li₃N
E) 15.1 g Li₃N

Question 11

According to the following reaction,how many grams of sulfur are formed when 37.4 g of water are formed? 2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2 H₂O(l)

A) 99.8 g S
B) 66.6 g S
C) 56.1 g S
D) 44.4 g S
E) 14.0 g S

Question 12

Determine the molarity of a solution formed by dissolving 3.00 moles of NaCl in enough water to yield 4.00 L of solution.

A) 1.33 M
B) 2.00 M
C) 0.750 M
D) 3.00 M
E) 12.00 M

Question 13

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol. 4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

A) 0.290 mol O₂
B) 0.580 mol O₂
C) 18.5 mol O₂
D) 0.724 mol O₂
E) 1.73 mol O₂

Question 14

How many molecules of H₂S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO₂. 2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2 H₂O(l)

A) 1.48 × 10²⁴ molecules H₂S
B) 9.89 × 10²³ molecules H₂S
C) 5.06 × 10²⁵ molecules H₂S
D) 3.17 × 10²⁵ molecules H₂S
E) 2.44 × 10²³ molecules H₂S

Question 15

A 14.01 g sample of N₂ reacts with 3.02 g of H₂ to form ammonia (NH₃).If ammonia is the only product,what mass of ammonia is formed?

A) 17.01 g
B) 1.10 g
C) 14.01 g
D) 3.02 g
E) 23.07 g

Question 16

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe₂O₃ react with excess Al according to the following reaction. Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)

A) 61.03%
B) 28.65%
C) 57.30%
D) 20.02%
E) 81.93%

Question 17

Consider the following balanced reaction.How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present.The molar masses are as follows: H₂O = 18.02 g/mol,HNO₃ = 63.02 g/mol. 3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A) 38.0 g H₂O
B) 21.7 g H₂O
C) 43.4 g H₂O
D) 10.9 g H₂O
E) 26.5 g H₂O

Question 18

Define a greenhouse gas.

A) Greenhouse gases prevent visible light from passing through and warming the Earth's surface, and prevent heat energy from radiating back out into space.
B) Greenhouse gases allow visible light to pass through and warm the Earth's surface, and also allow heat energy to radiate back out into space.
C) Greenhouse gases allow visible light to pass through and cool the Earth's surface, and prevent heat energy from radiating back out into space.
D) Greenhouse gases allow visible light to pass through and warm the Earth's surface, and prevent heat energy from radiating back out into space.
E) Greenhouse gases prevent visible light from passing through and cooling the Earth's surface, and prevent heat energy from radiating back out into space.

Question 19

Consider the following balanced reaction.What mass (in g)of CO₂ can be formed from 288 mg of O₂? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

A) 0.396 g CO₂
B) 0.209 g CO₂
C) 0.792 g CO₂
D) 0.126 g CO₂
E) 0.198 g CO₂

Question 20

Two samples of calcium fluoride are decomposed into their constituent elements.The first sample produced 0.154 g of calcium and 0.146 g of fluorine.If the second sample produced 294 mg of fluorine,how many g of calcium were formed?

A) 0.280 g
B) 3.09 × 10² g
C) 3.13 g
D) 0.309 g
E) 2.80 × 10² g

Question 21

Give the spectator ions for the reaction that occurs when aqueous solutions of H₂SO₄ and KOH are mixed.

A) H⁺ and OH^-
B) K⁺ and SO₄^2-
C) H⁺ and SO₄^2-
D) OH^- and K⁺
E) No spectator ions are present.

Question 22

Identify the spectator ions for the reaction that occurs when aqueous solutions of lithium sulfide and copper(II)nitrate are mixed.

A) Cu²⁺ and NO₃^-
B) Li⁺ and Cu²⁺
C) Li⁺ and NO₃^-
D) S^2- and Cu²⁺
E) No spectator ions are present.

Question 23

Determine the number of grams H₂ formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 10²³ atoms of Fe according to the following reaction. 2 HCl(aq)+ Fe(s)→ H₂(g)+ FeCl₂(aq)

A) 0.374 g
B) 1.33 g
C) 1.14 g
D) 0.187 g
E) 1.51 g

Question 24

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of K₂S and Fe(NO₃)₂ are mixed.

A) K⁺(aq) + NO₃^-(aq) → KNO₃(s)
B) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) → FeS(s) + 2 K⁺(aq) + 2 NO₃^-(aq)
C) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) → Fe²⁺(aq) + S^2-(aq) + 2 KNO₃(s)
D) Fe²⁺(aq) + S^2-(aq) → FeS(s)
E) No reaction occurs.

Question 25

Identify ammonia.

A) strong electrolyte, strong base
B) strong electrolyte, weak base
C) weak electrolyte, strong base
D) weak electrolyte, weak base
E) nonelectrolyte

Question 26

How many molecules of sucrose (C₁₂H₂₂O₁₁,molar mass = 342.30 g/mol)are contained in 14.3 mL of 0.140 M sucrose solution?

A) 8.29 × 10²² molecules C₁₂H₂₂O₁₁
B) 1.21 × 10²¹ molecules C₁₂H₂₂O₁₁
C) 6.15 × 10²² molecules C₁₂H₂₂O₁₁
D) 1.63 × 10²³ molecules C₁₂H₂₂O₁₁
E) 5.90 × 10²⁴ molecules C₁₂H₂₂O₁₁

Question 27

According to the following reaction,what mass of PbCl₂ can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO₃)₂. 2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

A) 7.19 g
B) 3.59 g
C) 1.80 g
D) 5.94 g
E) 1.30 g

Question 28

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of H₂SO₄ and KOH are mixed.

A) H⁺(aq) + OH^-(aq) → H₂O(l)
B) 2 K⁺(aq) + SO₄^2-(aq) → K₂SO₄(s)
C) H⁺(aq) + OH^-(aq) + 2 K⁺(aq) + SO₄^2-(aq) → H₂O(l) + 2 K⁺(aq) + SO₄^2-(aq)
D) H⁺(aq) + OH^-(aq) + 2 K⁺(aq) + SO₄^2-(aq) → H⁺(aq) + OH^-(aq) + K₂SO₄(s)
E) No reaction occurs.

Question 29

Give the spectator ions for the reaction that occurs when aqueous solutions of K₂S and Fe(NO₃)₂ are mixed.

A) K⁺ and NO₃^-
B) Fe²⁺ and K⁺
C) S^2- and NO₃^-
D) Fe²⁺ and S^2-
E) No spectator ions are present.

Question 30

According to the following reaction,what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO₃)₂ solution? 2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

A) 97.4 mL
B) 116 mL
C) 43.0 mL
D) 86.1 mL
E) 58.1 mL

Question 31

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of K₂S and Fe(NO₃)₂ are mixed.

A) K⁺(aq) + NO₃^-(aq) → KNO₃(s)
B) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) → FeS(s) + 2 K⁺(aq) + 2 NO₃^-(aq)
C) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) → Fe²⁺(aq) + S^2-(aq) + 2 KNO₃(s)
D) Fe²⁺(aq) + S^2-(aq) → FeS(s)
E) No reaction occurs.

Question 32

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

A) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂O(l) + CO₂(g) + 2 Na⁺(aq) + 2 Cl^-(aq)
B) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂CO₃(s) + 2 NaCl(s)
C) 2 H⁺(aq) + CO₃^2-(aq) → H₂O(l) + CO₂(g)
D) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂CO₃(s) + 2 Na⁺(aq) + 2 Cl^-(aq)
E) No reaction occurs.

Question 33

What mass (in g)of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC₂H₃O₂ solution with 55.0 mL of 0.109 M MgCl₂ solution? 2 AgC₂H₃O₂(aq)+ MgCl₂(aq)→ 2 AgCl(s)+ Mg(C₂H₃O₂)₂(aq)

A) 0.838 g
B) 1.72 g
C) 0.859 g
D) 2.56 g
E) 1.70 g

Question 34

What volume of 0.305 M AgNO₃ is required to react exactly with 155.0 mL of 0.274 M Na₂SO₄ solution? Hint: You will want to write a balanced reaction.

A) 581 mL
B) 173 mL
C) 345 mL
D) 139 mL
E) 278 mL

Question 35

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of lithium sulfide and copper(II)nitrate are mixed.

A) Li⁺(aq) + NO₃^-(aq) → LiNO₃(s)
B) S^2-(aq) + Cu²⁺(aq) → CuS(s)
C) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → Cu²⁺(aq) + S^2-(aq) + 2 LiNO₃(s)
D) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → CuS(s) + 2 Li⁺(aq) + 2 NO₃^-(aq)
E) No reaction occurs.

Question 36

Choose the statement below that is TRUE.

A) A weak acid solution consists of mostly nonionized acid molecules.
B) The term "strong electrolyte" means that the substance is extremely reactive.
C) A strong acid solution consists of only partially ionized acid molecules.
D) The term "weak electrolyte" means that the substance is inert.
E) A molecular compound that does not ionize in solution is considered a strong electrolyte.

Question 37

According to the following reaction,how many moles of Fe(OH)₂ can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl₂. FeCl₂(aq)+ 2 LiOH(aq)→ Fe(OH)₂(s)+ 2 LiCl(aq)

A) 3.97 × 10^-2 moles
B) 2.52 × 10^-2 moles
C) 1.99 × 10^-2 moles
D) 5.03 × 10^-2 moles
E) 6.49 × 10^-2 moles

Question 38

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of Al(C₂H₃O₂)₃ and LiNO₃ are mixed.

A) Al³⁺(aq) + 3 NO₃^-(aq) → Al(NO₃)₃(s)
B) Li⁺(aq) + C₂H₃O₂^-(aq) → LiC₂H₃O₂(s)
C) Al³⁺(aq) + 3 NO₃^-(aq) + Li⁺(aq) + C₂H₃O₂^-(aq) → Al(NO₃)₃(aq) + LiC₂H₃O₂(s)
D) 3 Li⁺(aq) + (C₂H₃O₂)₃^3-(aq) → Li₃(C₂H₃O₂)₃(s)
E) No reaction occurs.

Question 39

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of lithium sulfide and copper(II)nitrate are mixed.

A) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → Cu²⁺(aq) + S^2-(aq) + 2 Li⁺(aq) + 2 NO₃^-(aq)
B) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → CuS(s) + 2 LiNO₃(s)
C) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → Cu²⁺(aq) + S^2-(aq) + 2 LiNO₃(s)
D) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → CuS(s) + 2 Li⁺(aq) + 2 NO₃^-(aq)
E) No reaction occurs.

Question 40

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of H₂SO₄ and KOH are mixed.

A) H⁺(aq) + OH^-(aq) → H₂O(l)
B) 2 K⁺(aq) + SO₄^2-(aq) → K₂SO₄(s)
C) H⁺(aq) + OH^-(aq) + 2 K⁺(aq) + SO₄^2-(aq) → H₂O(l) + 2 K⁺(aq) + SO₄^2-(aq)
D) H⁺(aq) + OH^-(aq) + 2 K⁺(aq) + SO₄^2-(aq) → H⁺(aq) + OH^-(aq) + K₂SO₄(s)
E) No reaction occurs.

Question 41

Give the spectator ions for the reaction that occurs when aqueous solutions of MgSO₃ and HI are mixed.

A) H⁺ and SO₃^2-
B) Mg²⁺ and I^-
C) H⁺ and I^-
D) SO₃^2- and Mg²⁺
E) No spectator ions are present.

Question 42

Determine the oxidation state of P in PO₃^3-.

A) +3
B) +6
C) +2
D) 0
E) -3

Question 43

Choose the reaction that represents the combustion of C₆H₁₂O₂.

A) C₆H₁₂O₂(l) + 8 O₂(g) → 6 CO₂(g) + 6 H₂O(g)
B) Mg(s) + C₆H₁₂O₂(l) → MgC₆H₁₂O₂(aq)
C) 6 C(s) + 6 H₂(g) + O₂(g) → C₆H₁₂O₂(l)
D) C₆H₁₂O₂(l) → 6 C(s) + 6 H₂(g) + O₂(g)
E) None of the above represents the combustion of C₆H₁₂O₂.

Question 44

Identify the combustion reaction.

A) 2 C₃H₇OH(l) + 9 O₂(g) → 6 CO₂(g) + 8 H₂O(g)
B) 2 H₂(g) + O₂(g) → 2 H₂O(g)
C) C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O
D) C(s) + O₂(g) → CO₂(g)
E) All of the reactions are examples of combustion reactions.

Question 45

Identify the oxidizing agent. 2 Al³⁺(aq)+ 2 Fe(s)→ 2 Al(s)+ 3 Fe²⁺(aq)

A) Al³⁺
B) Fe
C) Al
D) Fe²⁺
E) This is not an oxidation-reduction reaction.

Question 46

What element is undergoing oxidation (if any)in the following reaction? CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(g)

A) O
B) H
C) C
D) both C and H
E) None of the elements is undergoing oxidation.

Question 47

Determine the oxidizing agent in the following reaction. Ni(s)+ 2 AgClO₄(aq)→ Ni(ClO₄)₂(aq)+ 2 Ag(s)

A) Ag
B) Ni
C) Cl
D) O
E) This is not an oxidation-reduction reaction.

Question 48

Define an Arrhenius base.

A) an electron pair donor
B) an electron pair receiver
C) produces H⁺ ions in aqueous solution
D) accepts H⁺ ions
E) produces OH^- ions in aqueous solution

Question 49

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of MgSO₃ and HI are mixed.

A) 2 H⁺(aq) + SO₃^2-(aq) → H₂O(l) + SO₂(g)
B) Mg²⁺(aq) + 2 I^-(aq) → MgI₂(s)
C) 2 H⁺(aq) + SO₃^2-(aq) + Mg²⁺(aq) + 2 I^-(aq) → H₂SO₃(s) + MgI₂(aq)
D) 2 H⁺(aq) + SO₃^2-(aq) + Mg²⁺(aq) + 2 I^-(aq) → H₂O(l) + SO₂(g) + Mg²⁺(aq) + 2 I^-(aq)
E) No reaction occurs.

Question 50

Define an Arrhenius acid.

A) an electron pair donor
B) an electron pair receiver
C) produces H⁺ ions in aqueous solution
D) accepts H⁺ ions
E) produces OH^- ions in aqueous solution

Question 51

Identify the reducing agent. 2 Al³⁺(aq)+ 2 Fe(s)→ 2 Al(s)+ 3 Fe²⁺(aq)

A) Al³⁺
B) Fe
C) Al
D) Fe²⁺
E) This is not an oxidation-reduction reaction.

Question 52

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 M KOH solution.What is the concentration of the H₃PO₄ solution (in M)?

A) 1.03 M
B) 0.343 M
C) 0.114 M
D) 0.138 M
E) 0.0461 M

Question 53

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s)

A) Zn
B) N
C) O
D) Ag
E) This is not an oxidation-reduction reaction.

Question 54

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of 0.12 M LiOH solution.What is the concentration of the H₂SO₄ solution (in M)?

A) 0.20 M
B) 0.40 M
C) 0.10 M
D) 0.36 M
E) 0.25 M

Question 55

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

A) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂O(l) + CO₂(g) + 2 Na⁺(aq) + 2 Cl^-(aq)
B) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂CO₃(s) + 2 NaCl(s)
C) 2 H⁺(aq) + CO₃^2-(aq) → H₂O(l) + CO₂(g)
D) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂CO₃(s) + 2 Na⁺(aq) + 2 Cl^-(aq)
E) No reaction occurs.

Question 56

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of MgSO₃ and HI are mixed.

A) 2 H⁺(aq) + SO₃^2-(aq) → H₂O(l) + SO₂(g)
B) Mg²⁺(aq) + 2 I^-(aq) → MgI₂(s)
C) 2 H⁺(aq) + SO₃^2-(aq) + Mg²⁺(aq) + 2 I^-(aq) → H₂SO₃(s) + MgI₂(aq)
D) 2 H⁺(aq) + SO₃^2-(aq) + Mg²⁺(aq) + 2 I^-(aq) → H₂O(l) + SO₂(g) + Mg²⁺(aq) + 2 I^-(aq)
E) No reaction occurs.

Question 57

Identify the species reduced. 2 Al³⁺(aq)+ 2 Fe(s)→ 2 Al(s)+ 3 Fe²⁺(aq)

A) Al³⁺
B) Fe
C) Al
D) Fe²⁺
E) This is not an oxidation-reduction reaction.

Question 58

What element is undergoing reduction (if any)in the following reaction? Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s)

A) Zn
B) N
C) O
D) Ag
E) This is not an oxidation-reduction reaction.

Question 59

Give the spectator ions for the reaction that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

A) H⁺ and CO₃^2-
B) Na⁺ and CO₃^2-
C) H⁺ and Cl^-
D) Na⁺ and Cl^-
E) No spectator ions are present.

Question 60

Determine the reducing agent in the following reaction. 2 Li(s)+ Fe(C₂H₃O₂)₂(aq)→ 2 LiC₂H₃O₂(aq)+ Fe(s)

A) O
B) H
C) C
D) Fe
E) Li

Question 61

Lithium and nitrogen react to produce lithium nitride: 6 Li(s)+ (g)→ 2 Li₃N(s)
How many moles of are needed to react with 0.550 mol of lithium?

A) 3.30
B) 0.550
C) 0.183
D) 1.65
E) 0.0917

Question 62

How many grams of water react to form 6.21 moles of Ca(OH)₂? CaO(s)+ H₂O(l)→ Ca(OH)₂(s)

A) 6.21 g of H₂O
B) 24.8 g of H₂O
C) 49.7 g of H₂O
D) 112 g of H₂O
E) 99.4 g of H₂O

Question 63

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2 NaN₃(s)→ 2 Na(s)+ 3 N₂(g)
How many moles of N₂ are produced by the decomposition of 1.75 mol of sodium azide?

A) 1.17
B) 5.25
C) 2.63
D) 0.583
E) 0.875

Question 64

How many molecules of HCl are formed when 70.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3 H₂O → ICl + HIO₃ + 5 HCl

A) 3.90 × 10²⁴ molecules HCl
B) 2.34 × 10²⁴ molecules HCl
C) 7.02 × 10²⁴ molecules HCl
D) 4.68 × 10²⁴ molecules HCl
E) 3.90 × 10²⁵ molecules HCl

Question 65

According to the following balanced reaction,how many moles of Ca(OH)₂ will be formed from 3.22 moles of H₂O? CaO(s)+ H₂O(l)→ Ca(OH)₂(s)

A) 3.22 moles of Ca(OH)₂
B) 6.44 moles of Ca(OH)₂
C) 12.9 moles of Ca(OH)₂
D) 1.61 moles of Ca(OH)₂
E) 0.53 moles of Ca(OH)₂

Question 66

How many grams of calcium chloride are needed to produce 5.00 g of potassium chloride? CaCl₂(aq)+ K₂CO₃(aq)→ 2 KCl(aq)+ CaCO₃(aq)

A) 0.269 g
B) 3.72 g
C) 7.44 g
D) 14.9 g

Question 67

Balance the chemical equation given below,and determine the number of moles of iodine that react with 40.0 g of aluminum. _____ Al(s)+ _____ I₂(s)→ _____ Al₂I₆(s)

A) 0.988 mol
B) 2.22 mol
C) 2.97 mol
D) 4.45 mol

Question 68

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+ O₂(g)→ 2 MgO(s)
How many moles of O₂ are consumed when 2.10 mol of magnesium burns?

A) 0.0864
B) 0.952
C) 2.10
D) 4.20
E) 1.05

Question 69

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2 NaN₃(s)→ 2 Na(s)+ 3 N₂(g)
How many grams of sodium azide are required to produce 25.0 g of nitrogen?

A) 1.34
B) 0.595
C) 58.0
D) 38.7
E) 87.0

Question 70

Identify the species oxidized. 2 Al³⁺(aq)+ 2 Fe(s)→ 2 Al(s)+ 3 Fe²⁺(aq)

A) Al³⁺
B) Fe
C) Al
D) Fe²⁺
E) This is not an oxidation-reduction reaction.

Question 71

Lithium and nitrogen react to produce lithium nitride: 6 Li(s)+ (g)→ 2 Li₃N(s)
How many moles of lithium nitride are produced when 0.750 mol of lithium react in this fashion?

A) 0.250
B) 1.50
C) 0.125
D) 2.25
E) 0.375

Question 72

According to the following balanced reaction,how many moles of HNO₃ are formed from 2.50 moles of NO₂ if there is plenty of water present? 3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A) 7.50 moles NO
B) 3.75 moles NO
C) 2.50 moles NO
D) 1.67 moles NO
E) 0.834 moles NO

Question 73

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6 Li(s)+ (g)→ 2 Li₃N(s)
How many moles of lithium are needed to produce 0.31 mol of N when the reaction is carried out in the presence of excess nitrogen?

A) 0.16
B) 0.93
C) 0.10
D) 0.21
E) 1.9

Question 74

How many moles of CuO can be produced from 0.450 mol of Cu₂O in the following reaction? 2 Cu₂O(s)+ O₂(g)→ 4 CuO(s)

A) 0.225 mol
B) 0.450 mol
C) 0.900 mol
D) 1.80 mol
E) 63.2 mol

Question 75

According to the following balanced reaction,how many moles of NO are formed from 12.66 moles of NO₂ if there is plenty of water present? 3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A) 37.98 moles NO
B) 18.99 moles NO
C) 12.66 moles NO
D) 8.44 moles NO
E) 4.22 moles NO

Question 76

Carbonic acid can form water and carbon dioxide upon heating.How much carbon dioxide is formed from 1.55 g of carbonic acid? H₂CO₃ → H₂O + CO₂

A) 1.10 g
B) 2.18 g
C) 1.55 g
D) 0.450 g
E) 5.33 g

Question 77

Global warming is thought to be caused by the increase of one particular gas.Name the gas.

A) hydrogen
B) chlorine
C) carbon dioxide
D) nitrogen
E) helium

Question 78

According to the following balanced reaction,how many moles of CaO are required to exactly react with 3.22 moles of H₂O? CaO(s)+ H₂O(l)→ Ca(OH)₂(s)

A) 3.22 moles of CaO
B) 6.44 moles of CaO
C) 12.9 moles of CaO
D) 1.61 moles of CaO
E) 0.70 moles of CaO

Question 79

Consider the following reaction.How many moles of oxygen are required to produce 4.00 moles of water? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

A) 2.67 moles O₂
B) 6.00 moles O₂
C) 4.00 moles O₂
D) 16.0 moles O₂
E) 1.00 moles O₂

Question 80

How many moles of BCl₃ are needed to produce 25.0 g of HCl(aq)in the following reaction? BCl₃(g)+ 3 H₂O(l)→ 3 HCl(aq)+ B(OH)₃(aq)

A) 0.229 mol
B) 0.686 mol
C) 2.06 mol
D) 4.38 mol