Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)3(s)+ 3e- Cr(s)+ 3OH-(aq);E° = -1.48 V SnO2(s)+ 2H2O(l)+ 4e- Sn(s)+ 4OH-(aq);E° = -0.945 V MnO2(s)+ 4H+(aq)+ 2e- Mn2+(aq)+ 2H2O(l);E° = 1.224 V Hg2SO4(s)+ 2e- 2Hg(l)+ SO42-(aq);E° = 0.613 V

A) Cr(s) B) Sn(s) C) Mn2+(aq) D) Hg(l) E) OH-(aq) A) Cr(s) B) Sn(s) C) Mn2+(aq) D) Hg(l) E) OH-(aq) C

A voltaic cell consists of a Hg/Hg22+ electrode (E°= 0.85 V)and a Sn/Sn2+ electrode (E°= -0.14 V).Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25°C.

A) 0.0001 M B) 0.0007 M C) 0.005 M D) 0.03 M E) 0.05 M A) 0.0001 M B) 0.0007 M C) 0.005 M D) 0.03 M E) 0.05 M

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s)+ 2e- Pb(s)+ 2I-(aq);E° = -0.365 V Ca2+(aq)+ 2e- Ca(s);E° = -2.868 V Pt2+(aq)+ 2e- Pt(s);E° = 1.18 V Br2(l)+ 2e- 2Br-(aq);E° = 1.066 V

A) Pb(s) B) Ca(s) C) Pt(s) D) Br-(aq) E) Pt2+(aq) A) Pb(s) B) Ca(s) C) Pt(s) D) Br-(aq) E) Pt2+(aq)

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq)+ 2H+(aq)+ 2e- 2H2O(l);E° = 1.77 V Fe3+ (aq)+ e- Fe2+(aq);E° = 0.77 V Overall reaction: 2Fe3+(aq)+ 2H2O(l) $\to$ H2O2(aq)+ 2H+(aq)+ 2Fe2+(aq)

A) E°cell = -1.00 V,nonspontaneous B) E°cell = -1.00 V,spontaneous C) E°cell = 1.00 V,nonspontaneous D) E°cell = 1.00 V,spontaneous E) E°cell = -0.23 V,nonspontaneous A) E°cell = -1.00 V,nonspontaneous B) E°cell = -1.00 V,spontaneous C) E°cell = 1.00 V,nonspontaneous D) E°cell = 1.00 V,spontaneous E) E°cell = -0.23 V,nonspontaneous

Consider the reaction in the lead-acid cell Pb(s)+ PbO2(s)+ 2H2SO4(aq) $\to$ 2PbSO4(aq)+ 2H2O(l) For which E°cell = 2.04 V at 298 K.$\Delta$G° for this reaction is

A) -3.94 $\times$ 105 kJ B) -3.94 $\times$ 102 kJ C) -1.97 $\times$ 105 kJ D) -7.87 $\times$ 102 kJ E) None of these choices is correct. A) -3.94 $\times$ 105 kJ B) -3.94 $\times$ 102 kJ C) -1.97 $\times$ 105 kJ D) -7.87 $\times$ 102 kJ E) None of these choices is correct.

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq)+ e- Co2+(aq);E° = 1.82 V MnO4-(aq)+ 2H2O(l)+ 3e- MnO2(s)+ 4OH-(aq);E° = 0.59 V Overall reaction: MnO4-(aq)+ 2H2O(l)+ 3Co2+(aq) $\to$MnO2(s)+ 3Co3+(aq)+ 4OH-(aq)

A) E°cell = -1.23 V,spontaneous B) E°cell = -1.23 V,nonspontaneous C) E°cell = 1.23 V,spontaneous D) E°cell = 1.23 V,nonspontaneous E) E°cell = -0.05 V,nonspontaneous A) E°cell = -1.23 V,spontaneous B) E°cell = -1.23 V,nonspontaneous C) E°cell = 1.23 V,spontaneous D) E°cell = 1.23 V,nonspontaneous E) E°cell = -0.05 V,nonspontaneous

Calculate $\Delta$G° for the reaction of iron(II)ions with one mole of permanganate ions. MnO4-(aq)+ 8H+(aq)+ 5e- Mn2+(aq)+ 4H2O(l);E° = 1.51 V Fe3+(aq)+ e- Fe2+(aq);E°= 0.77 V

A) -71.4 kJ B) -286 kJ C) -357 kJ D) -428 kJ E) None of these choices is correct. A) -71.4 kJ B) -286 kJ C) -357 kJ D) -428 kJ E) None of these choices is correct.

A voltaic cell consists of a Mn/Mn2+ electrode (E°= -1.18 V)and a Fe/Fe2+ electrode (E°= -0.44 V).Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25°C.

A) 0.040 M B) 0.24 M C) 1.1 M D) 1.8 M E) None of these choices is correct. A) 0.040 M B) 0.24 M C) 1.1 M D) 1.8 M E) None of these choices is correct.

Exam 21: Electrochemistry: Chemical Change and Electrical Work

In the electrolyte of an electrochemical cell,current is carried by anions moving toward the anode and cations moving in the opposite direction.

Free

(True/False)

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Question 1

Correct Answer:

Verified

True

The chlor-alkali process produces chlorine,Cl₂(g),in large quantities.What other industrially important substances are produced in this process?

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)₃(s)+ 3e^- Cr(s)+ 3OH^-(aq);E° = -1.48 V SnO₂(s)+ 2H₂O(l)+ 4e^- Sn(s)+ 4OH^-(aq);E° = -0.945 V MnO₂(s)+ 4H⁺(aq)+ 2e^- Mn²⁺(aq)+ 2H₂O(l);E° = 1.224 V Hg₂SO₄(s)+ 2e^- 2Hg(l)+ SO₄^2-(aq);E° = 0.613 V

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Question 3

Correct Answer:

Verified

Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V;all E° values refer to the M²⁺/M half-cell reactions.

(Multiple Choice)

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Question 4

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E°= 0.85 V)and a Sn/Sn²⁺ electrode (E°= -0.14 V).Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

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Question 5

A battery is considered "dead" when

(Multiple Choice)

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Question 6

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s)+ 2e^- Pb(s)+ 2I^-(aq);E° = -0.365 V Ca²⁺(aq)+ 2e^- Ca(s);E° = -2.868 V Pt²⁺(aq)+ 2e^- Pt(s);E° = 1.18 V Br₂(l)+ 2e^- 2Br^-(aq);E° = 1.066 V

(Multiple Choice)

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Question 7

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H₂O₂(aq)+ 2H⁺(aq)+ 2e^- $Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq)+ 2H+(aq)+ 2e- 2H2O(l);E° = 1.77 V Fe3+ (aq)+ e- Fe2+(aq);E° = 0.77 V Overall reaction: 2Fe3+(aq)+ 2H2O(l) \to H2O2(aq)+ 2H+(aq)+ 2Fe2+(aq)$ 2H₂O(l);E° = 1.77 V Fe³⁺ (aq)+ e^- $Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq)+ 2H+(aq)+ 2e- 2H2O(l);E° = 1.77 V Fe3+ (aq)+ e- Fe2+(aq);E° = 0.77 V Overall reaction: 2Fe3+(aq)+ 2H2O(l) \to H2O2(aq)+ 2H+(aq)+ 2Fe2+(aq)$ Fe²⁺(aq);E° = 0.77 V Overall reaction: 2Fe³⁺(aq)+ 2H₂O(l) $\to$ H₂O₂(aq)+ 2H⁺(aq)+ 2Fe²⁺(aq)

(Multiple Choice)

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Question 8

A secondary cell (battery)can operate either as a galvanic or an electrolytic cell.

(True/False)

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Question 9

Which one of the following is not a redox reaction?

(Multiple Choice)

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Question 10

Consider the reaction in the lead-acid cell Pb(s)+ PbO₂(s)+ 2H₂SO₄(aq) $\to$ 2PbSO₄(aq)+ 2H₂O(l) For which E°_cell = 2.04 V at 298 K. $\Delta$ G° for this reaction is

(Multiple Choice)

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Question 11

In one or two short sentences each,explain what is meant by the following terms. a.galvanic or voltaic cell b.electrolytic cell c.salt bridge d.secondary battery or cell e.primary battery or cell f.glass electrode

(Essay)

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Question 12

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co³⁺(aq)+ e^- $Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq)+ e- Co2+(aq);E° = 1.82 V MnO4-(aq)+ 2H2O(l)+ 3e- MnO2(s)+ 4OH-(aq);E° = 0.59 V Overall reaction: MnO4-(aq)+ 2H2O(l)+ 3Co2+(aq) \to MnO2(s)+ 3Co3+(aq)+ 4OH-(aq)$ Co²⁺(aq);E° = 1.82 V MnO₄^-(aq)+ 2H₂O(l)+ 3e^- $Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq)+ e- Co2+(aq);E° = 1.82 V MnO4-(aq)+ 2H2O(l)+ 3e- MnO2(s)+ 4OH-(aq);E° = 0.59 V Overall reaction: MnO4-(aq)+ 2H2O(l)+ 3Co2+(aq) \to MnO2(s)+ 3Co3+(aq)+ 4OH-(aq)$ MnO₂(s)+ 4OH^-(aq);E° = 0.59 V Overall reaction: MnO₄^-(aq)+ 2H₂O(l)+ 3Co²⁺(aq) $\to$ MnO₂(s)+ 3Co³⁺(aq)+ 4OH^-(aq)

(Multiple Choice)

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Question 13

Calculate $\Delta$ G° for the reaction of iron(II)ions with one mole of permanganate ions. MnO₄^-(aq)+ 8H⁺(aq)+ 5e^- $Calculate \Delta G° for the reaction of iron(II)ions with one mole of permanganate ions. MnO4-(aq)+ 8H+(aq)+ 5e- Mn2+(aq)+ 4H2O(l);E° = 1.51 V Fe3+(aq)+ e- Fe2+(aq);E°= 0.77 V$ Mn²⁺(aq)+ 4H₂O(l);E° = 1.51 V Fe³⁺(aq)+ e^- $Calculate \Delta G° for the reaction of iron(II)ions with one mole of permanganate ions. MnO4-(aq)+ 8H+(aq)+ 5e- Mn2+(aq)+ 4H2O(l);E° = 1.51 V Fe3+(aq)+ e- Fe2+(aq);E°= 0.77 V$ Fe²⁺(aq);E°= 0.77 V

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Question 14

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics.If E°_cell = 1.587 V and E° of the cathode half-cell is 0.536 V,what is E° of the anode half-cell? S₂O₈^2-(aq)+ 2H⁺ + 2I^-(aq) $\to$ 2HSO₄^-(aq)+ I₂(aq)

(Multiple Choice)

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Question 15

A voltaic cell consists of a Mn/Mn²⁺ electrode (E°= -1.18 V)and a Fe/Fe²⁺ electrode (E°= -0.44 V).Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25°C.

(Multiple Choice)

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Question 16

Which of the following statements about voltaic and electrolytic cells is correct?

(Multiple Choice)

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Question 17

Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.

(Essay)

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Question 18

Consider the following redox equation Mn(OH)₂(s)+ MnO₄^-(aq) $\to$ MnO₄^2-(aq)(basic solution) When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH^-(aq)and on which side of the equation is OH^-(aq)present?

(Multiple Choice)

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Question 19

What product forms at the cathode during the electrolysis of molten NaCl in the Downs cell?

(Multiple Choice)

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Question 20

Showing 1 - 20 of 97

In the electrolyte of an electrochemical cell,current is carried by anions moving toward the anode and cations moving in the opposite direction.

The chlor-alkali process produces chlorine,Cl₂(g),in large quantities.What other industrially important substances are produced in this process?

Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V;all E° values refer to the M²⁺/M half-cell reactions.

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E°= 0.85 V)and a Sn/Sn²⁺ electrode (E°= -0.14 V).Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

A battery is considered "dead" when

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s)+ 2e^- Pb(s)+ 2I^-(aq);E° = -0.365 V Ca²⁺(aq)+ 2e^- Ca(s);E° = -2.868 V Pt²⁺(aq)+ 2e^- Pt(s);E° = 1.18 V Br₂(l)+ 2e^- 2Br^-(aq);E° = 1.066 V

A secondary cell (battery)can operate either as a galvanic or an electrolytic cell.

Which one of the following is not a redox reaction?

Consider the reaction in the lead-acid cell Pb(s)+ PbO₂(s)+ 2H₂SO₄(aq) $\to$ 2PbSO₄(aq)+ 2H₂O(l) For which E°_cell = 2.04 V at 298 K. $\Delta$ G° for this reaction is

In one or two short sentences each,explain what is meant by the following terms. a.galvanic or voltaic cell b.electrolytic cell c.salt bridge d.secondary battery or cell e.primary battery or cell f.glass electrode

A voltaic cell consists of a Mn/Mn²⁺ electrode (E°= -1.18 V)and a Fe/Fe²⁺ electrode (E°= -0.44 V).Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25°C.

Which of the following statements about voltaic and electrolytic cells is correct?

Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.

Consider the following redox equation Mn(OH)₂(s)+ MnO₄^-(aq) $\to$ MnO₄^2-(aq)(basic solution) When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH^-(aq)and on which side of the equation is OH^-(aq)present?

What product forms at the cathode during the electrolysis of molten NaCl in the Downs cell?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Exam 21: Electrochemistry: Chemical Change and Electrical Work

In the electrolyte of an electrochemical cell,current is carried by anions moving toward the anode and cations moving in the opposite direction.

The chlor-alkali process produces chlorine,Cl2(g),in large quantities.What other industrially important substances are produced in this process?

Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)3(s)+ 3e- Cr(s)+ 3OH-(aq);E° = -1.48 V SnO2(s)+ 2H2O(l)+ 4e- Sn(s)+ 4OH-(aq);E° = -0.945 V MnO2(s)+ 4H+(aq)+ 2e- Mn2+(aq)+ 2H2O(l);E° = 1.224 V Hg2SO4(s)+ 2e- 2Hg(l)+ SO42-(aq);E° = 0.613 V

Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°Fe = -0.44 V;all E° values refer to the M2+/M half-cell reactions.

A voltaic cell consists of a Hg/Hg22+ electrode (E°= 0.85 V)and a Sn/Sn2+ electrode (E°= -0.14 V).Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25°C.

A battery is considered "dead" when

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s)+ 2e- Pb(s)+ 2I-(aq);E° = -0.365 V Ca2+(aq)+ 2e- Ca(s);E° = -2.868 V Pt2+(aq)+ 2e- Pt(s);E° = 1.18 V Br2(l)+ 2e- 2Br-(aq);E° = 1.066 V

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq)+ 2H+(aq)+ 2e- 2H2O(l);E° = 1.77 V Fe3+ (aq)+ e- Fe2+(aq);E° = 0.77 V Overall reaction: 2Fe3+(aq)+ 2H2O(l) →\to→ H2O2(aq)+ 2H+(aq)+ 2Fe2+(aq)

A secondary cell (battery)can operate either as a galvanic or an electrolytic cell.

Which one of the following is not a redox reaction?

Consider the reaction in the lead-acid cell Pb(s)+ PbO2(s)+ 2H2SO4(aq) →\to→ 2PbSO4(aq)+ 2H2O(l) For which E°cell = 2.04 V at 298 K. Δ\DeltaΔ G° for this reaction is

In one or two short sentences each,explain what is meant by the following terms. a.galvanic or voltaic cell b.electrolytic cell c.salt bridge d.secondary battery or cell e.primary battery or cell f.glass electrode

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq)+ e- Co2+(aq);E° = 1.82 V MnO4-(aq)+ 2H2O(l)+ 3e- MnO2(s)+ 4OH-(aq);E° = 0.59 V Overall reaction: MnO4-(aq)+ 2H2O(l)+ 3Co2+(aq) →\to→ MnO2(s)+ 3Co3+(aq)+ 4OH-(aq)

Calculate Δ\DeltaΔ G° for the reaction of iron(II)ions with one mole of permanganate ions. MnO4-(aq)+ 8H+(aq)+ 5e- Mn2+(aq)+ 4H2O(l);E° = 1.51 V Fe3+(aq)+ e- Fe2+(aq);E°= 0.77 V

A voltaic cell consists of a Mn/Mn2+ electrode (E°= -1.18 V)and a Fe/Fe2+ electrode (E°= -0.44 V).Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25°C.

Which of the following statements about voltaic and electrolytic cells is correct?

Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.

Consider the following redox equation Mn(OH)2(s)+ MnO4-(aq) →\to→ MnO42-(aq)(basic solution) When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH-(aq)and on which side of the equation is OH-(aq)present?

What product forms at the cathode during the electrolysis of molten NaCl in the Downs cell?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

The chlor-alkali process produces chlorine,Cl₂(g),in large quantities.What other industrially important substances are produced in this process?

Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V;all E° values refer to the M²⁺/M half-cell reactions.

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E°= 0.85 V)and a Sn/Sn²⁺ electrode (E°= -0.14 V).Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s)+ 2e^- Pb(s)+ 2I^-(aq);E° = -0.365 V Ca²⁺(aq)+ 2e^- Ca(s);E° = -2.868 V Pt²⁺(aq)+ 2e^- Pt(s);E° = 1.18 V Br₂(l)+ 2e^- 2Br^-(aq);E° = 1.066 V

Consider the reaction in the lead-acid cell Pb(s)+ PbO₂(s)+ 2H₂SO₄(aq) $\to$ 2PbSO₄(aq)+ 2H₂O(l) For which E°_cell = 2.04 V at 298 K. $\Delta$ G° for this reaction is

A voltaic cell consists of a Mn/Mn²⁺ electrode (E°= -1.18 V)and a Fe/Fe²⁺ electrode (E°= -0.44 V).Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25°C.

Consider the following redox equation Mn(OH)₂(s)+ MnO₄^-(aq) $\to$ MnO₄^2-(aq)(basic solution) When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH^-(aq)and on which side of the equation is OH^-(aq)present?