Table 20.1 Half Reaction E°(V) FS1U1B12S1U1B0 (g) + 2eS1U1P1-S1S1P0 → 2FS1U1P1-S1S1P0 (aq)+2.87 ClS1U1B12S1U1B0 (g) + 2eS1U1P1-S1S1P0 → 2ClS1U1P1-S1S1P0 (aq)+1.359 BrS1U1B12S1U1B0 (l) + 2eS1U1P1-S1S1P0 → 2BrS1U1P1-S1S1P0 (aq)+1.065 OS1U1B12S1U1B0 (g) + 4HS1U1P1+S1S1P0 (aq) + 4eS1U1P1-S1S1P0 → 2HS1U1B12S1U1B0O (l) +1.23 AgS1U1P1+S1S1P0 + eS1U1P1-S1S1P0 → Ag (s)+0.799 FeS1U1P13S1S1P0S1U1P1+S1S1P0 (aq) + eS1U1P1-S1S1P0 → FeS1U1P12+S1S1P0 (aq)+0.771 IS1U1B12S1U1B0 (s) + 2eS1U1P1-S1S1P0 → 2IS1U1P1-S1S1P0 (aq)+0.536 CuS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Cu (s)+0.34 2HS1U1P1+S1S1P0 + 2eS1U1P1-S1S1P0 → HS1U1B12S1U1B0 (g) 0 PbS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Pb (s)-0.126 NiS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Ni (s)-0.28 LiS1U1P1+S1S1P0 + eS1U1P1-S1S1P0 → Li (s)-3.05 -Which of the halogens in Table 20.1 is the strongest oxidizing agent?

A) Cl2 B) Br2 C) F2 D) I2 E) All of the halogens have equal strength as oxidizing agents. A) Cl2 B) Br2 C) F2 D) I2 E) All of the halogens have equal strength as oxidizing agents.

Which element is reduced in the reaction below? Fe2+ + H+ + Cr2O72- → Fe3+ + Cr3+ + H2O

A) Fe B) Cr C) O D) H A) Fe B) Cr C) O D) H

________ is the oxidizing agent in the reaction below. Cr2O72- + 6S2O32- + 14H+ → 2Cr3+ + 3S4O62- + 7H2O

A) Cr2O72- B) S2O32- C) H+ D) Cr3+ E) S4O62- A) Cr2O72- B) S2O32- C) H+ D) Cr3+ E) S4O62-

Which element is reduced in the following reaction? Fe2S3 + 12HNO3 → 2Fe(NO3)3 + 3S + 6NO2 + 6H2O

A) N B) S C) H D) O E) NO2 A) N B) S C) H D) O E) NO2

Table 20.1 Half Reaction E°(V) FS1U1B12S1U1B0 (g) + 2eS1U1P1-S1S1P0 → 2FS1U1P1-S1S1P0 (aq)+2.87 ClS1U1B12S1U1B0 (g) + 2eS1U1P1-S1S1P0 → 2ClS1U1P1-S1S1P0 (aq)+1.359 BrS1U1B12S1U1B0 (l) + 2eS1U1P1-S1S1P0 → 2BrS1U1P1-S1S1P0 (aq)+1.065 OS1U1B12S1U1B0 (g) + 4HS1U1P1+S1S1P0 (aq) + 4eS1U1P1-S1S1P0 → 2HS1U1B12S1U1B0O (l) +1.23 AgS1U1P1+S1S1P0 + eS1U1P1-S1S1P0 → Ag (s)+0.799 FeS1U1P13S1S1P0S1U1P1+S1S1P0 (aq) + eS1U1P1-S1S1P0 → FeS1U1P12+S1S1P0 (aq)+0.771 IS1U1B12S1U1B0 (s) + 2eS1U1P1-S1S1P0 → 2IS1U1P1-S1S1P0 (aq)+0.536 CuS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Cu (s)+0.34 2HS1U1P1+S1S1P0 + 2eS1U1P1-S1S1P0 → HS1U1B12S1U1B0 (g) 0 PbS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Pb (s)-0.126 NiS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Ni (s)-0.28 LiS1U1P1+S1S1P0 + eS1U1P1-S1S1P0 → Li (s)-3.05 -Which one of the following types of elements is most likely to be a good oxidizing agent?

A) alkali metals B) lanthanides C) alkaline earth elements D) transition elements E) halogens A) alkali metals B) lanthanides C) alkaline earth elements D) transition elements E) halogens

What is the coefficient of Fe3+ when the following equation is balanced? CN- + Fe3+ → CNO- + Fe2+ (basic solution)

A) 1 B) 2 C) 3 D) 4 E) 5 A) 1 B) 2 C) 3 D) 4 E) 5

How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30.0 amp for 8.0 hours?

A) 17.9 B) 359 C) 0.0622 D) 179 E) 89.7 A) 17.9 B) 359 C) 0.0622 D) 179 E) 89.7

What is the oxidation number of sulfur in the S2O32- ion?

A) +2 B) +1 C) 0 D) -1 E) -2 A) +2 B) +1 C) 0 D) -1 E) -2

Exam 20: Electrochemistry

Table 20.1 Half Reaction E°(V) F₂ (g) + 2e^- → 2F^- (aq)+2.87 Cl₂ (g) + 2e^- → 2Cl^- (aq)+1.359 Br₂ (l) + 2e^- → 2Br^- (aq)+1.065 O₂ (g) + 4H⁺ (aq) + 4e^- → 2H₂O (l) +1.23 Ag⁺ + e^- → Ag (s)+0.799 Fe³⁺ (aq) + e^- → Fe²⁺ (aq)+0.771 I₂ (s) + 2e^- → 2I^- (aq)+0.536 Cu²⁺ + 2e^- → Cu (s)+0.34 2H⁺ + 2e^- → H₂ (g) 0 Pb²⁺ + 2e^- → Pb (s)-0.126 Ni²⁺ + 2e^- → Ni (s)-0.28 Li⁺ + e^- → Li (s)-3.05 -Which of the halogens in Table 20.1 is the strongest oxidizing agent?

(Multiple Choice)

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Question 61

In a half reaction, the amount of a substance that is reduced or oxidized is directly proportional to the number of electrons generated in the cell.

(True/False)

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Question 62

One of the differences between a voltaic cell and an electrolytic cell is that in an electrolytic cell, ________.

(Multiple Choice)

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Question 63

Galvanized iron is iron coated with ________.

(Multiple Choice)

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Question 64

The lead-containing reactant(s)consumed during recharging of a lead-acid battery is/are ________.

(Multiple Choice)

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Question 65

Which element is reduced in the reaction below? Fe²⁺+ H⁺ + Cr₂O₇²^- → Fe³⁺ + Cr³⁺ + H₂O

(Multiple Choice)

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Question 66

Which substance is serving as the reducing agent in the following reaction? 14H⁺ + Cr₂O₇^2- + 3Ni → 3Ni²⁺ + 2Cr³⁺ + 7H₂O

(Multiple Choice)

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Question 67

________ is the oxidizing agent in the reaction below. Cr₂O₇^2- + 6S₂O₃^2- + 14H⁺ → 2Cr³⁺ + 3S₄O₆^2- + 7H₂O

(Multiple Choice)

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Question 68

Which element is reduced in the following reaction? Fe₂S₃ + 12HNO₃ → 2Fe(NO₃)₃ + 3S + 6NO₂ + 6H₂O

(Multiple Choice)

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Question 69

Table 20.1 Half Reaction E°(V) F₂ (g) + 2e^- → 2F^- (aq)+2.87 Cl₂ (g) + 2e^- → 2Cl^- (aq)+1.359 Br₂ (l) + 2e^- → 2Br^- (aq)+1.065 O₂ (g) + 4H⁺ (aq) + 4e^- → 2H₂O (l) +1.23 Ag⁺ + e^- → Ag (s)+0.799 Fe³⁺ (aq) + e^- → Fe²⁺ (aq)+0.771 I₂ (s) + 2e^- → 2I^- (aq)+0.536 Cu²⁺ + 2e^- → Cu (s)+0.34 2H⁺ + 2e^- → H₂ (g) 0 Pb²⁺ + 2e^- → Pb (s)-0.126 Ni²⁺ + 2e^- → Ni (s)-0.28 Li⁺ + e^- → Li (s)-3.05 -Which one of the following types of elements is most likely to be a good oxidizing agent?

(Multiple Choice)

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Question 70

The major product of a hydrogen fuel cell is ________.

(Short Answer)

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Question 71

What is the coefficient of Fe³⁺ when the following equation is balanced? CN^- + Fe³⁺ → CNO^- + Fe²⁺ (basic solution)

(Multiple Choice)

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Question 72

Table 20.2 -The standard cell potential (E°_cell)for the voltaic cell based on the reaction below is ________ V. 3Sn⁴⁺ (aq) + 2Cr (s) → 2Cr³⁺ (aq) + 3Sn²⁺ (aq)

(Multiple Choice)

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Question 73

In the electrochemical cell using the redox reaction below, the cathode half-reaction is ________. 2H⁺ (s) + Sn (s) → Sn²⁺ (aq) + H₂ (g)

(Multiple Choice)

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Question 74

In the galvanic cell using the redox reaction below, the reduction half-reaction is ________. Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)

(Multiple Choice)

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Question 75

The electrode where reduction occurs is called the anode.

(True/False)

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Question 76

How many grams of Ca metal are produced by the electrolysis of molten CaBr₂ using a current of 30.0 amp for 8.0 hours?

(Multiple Choice)

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Question 77

How many grams of Cu are obtained by passing a current of 12 A through a solution of CuSO₄ for 15 minutes?

(Multiple Choice)

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Question 78

What is the oxidation number of sulfur in the S₂O₃^2- ion?

(Multiple Choice)

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Question 79

How many kilowatt-hours of electricity are used to produce 4.50 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 5.00 V?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 114

Exam 20: Electrochemistry

In a half reaction, the amount of a substance that is reduced or oxidized is directly proportional to the number of electrons generated in the cell.

One of the differences between a voltaic cell and an electrolytic cell is that in an electrolytic cell, ________.

Galvanized iron is iron coated with ________.

The lead-containing reactant(s)consumed during recharging of a lead-acid battery is/are ________.

Which element is reduced in the reaction below? Fe2+ + H+ + Cr2O72- → Fe3+ + Cr3+ + H2O

Which substance is serving as the reducing agent in the following reaction? 14H+ + Cr2O72- + 3Ni → 3Ni2+ + 2Cr3+ + 7H2O

________ is the oxidizing agent in the reaction below. Cr2O72- + 6S2O32- + 14H+ → 2Cr3+ + 3S4O62- + 7H2O

Which element is reduced in the following reaction? Fe2S3 + 12HNO3 → 2Fe(NO3)3 + 3S + 6NO2 + 6H2O

The major product of a hydrogen fuel cell is ________.

What is the coefficient of Fe3+ when the following equation is balanced? CN- + Fe3+ → CNO- + Fe2+ (basic solution)

Table 20.2 -The standard cell potential (E°cell)for the voltaic cell based on the reaction below is ________ V. 3Sn4+ (aq) + 2Cr (s) → 2Cr3+ (aq) + 3Sn2+ (aq)

In the electrochemical cell using the redox reaction below, the cathode half-reaction is ________. 2H+ (s) + Sn (s) → Sn2+ (aq) + H2 (g)

In the galvanic cell using the redox reaction below, the reduction half-reaction is ________. Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s)

The electrode where reduction occurs is called the anode.

How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30.0 amp for 8.0 hours?

How many grams of Cu are obtained by passing a current of 12 A through a solution of CuSO4 for 15 minutes?

What is the oxidation number of sulfur in the S2O32- ion?

How many kilowatt-hours of electricity are used to produce 4.50 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 5.00 V?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

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Which element is reduced in the reaction below? Fe²⁺+ H⁺ + Cr₂O₇²^- → Fe³⁺ + Cr³⁺ + H₂O

Which substance is serving as the reducing agent in the following reaction? 14H⁺ + Cr₂O₇^2- + 3Ni → 3Ni²⁺ + 2Cr³⁺ + 7H₂O

________ is the oxidizing agent in the reaction below. Cr₂O₇^2- + 6S₂O₃^2- + 14H⁺ → 2Cr³⁺ + 3S₄O₆^2- + 7H₂O

Which element is reduced in the following reaction? Fe₂S₃ + 12HNO₃ → 2Fe(NO₃)₃ + 3S + 6NO₂ + 6H₂O

What is the coefficient of Fe³⁺ when the following equation is balanced? CN^- + Fe³⁺ → CNO^- + Fe²⁺ (basic solution)

Table 20.2 -The standard cell potential (E°_cell)for the voltaic cell based on the reaction below is ________ V. 3Sn⁴⁺ (aq) + 2Cr (s) → 2Cr³⁺ (aq) + 3Sn²⁺ (aq)

In the electrochemical cell using the redox reaction below, the cathode half-reaction is ________. 2H⁺ (s) + Sn (s) → Sn²⁺ (aq) + H₂ (g)

In the galvanic cell using the redox reaction below, the reduction half-reaction is ________. Zn (s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s)

How many grams of Ca metal are produced by the electrolysis of molten CaBr₂ using a current of 30.0 amp for 8.0 hours?

How many grams of Cu are obtained by passing a current of 12 A through a solution of CuSO₄ for 15 minutes?

What is the oxidation number of sulfur in the S₂O₃^2- ion?

How many kilowatt-hours of electricity are used to produce 4.50 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 5.00 V?