Consider the reaction of iodine with manganese dioxide 3I2(s) + 2MnO2(s) + 8OH-(aq) ⇄ 6I−(aq) + 2MnO4(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 × 10−7. Calculate E°cell for the reaction at 25°C.

A) −0.36 V B) −0.18 V C) −0.12 V D) −0.060 V E) None of these choices are correct. A) −0.36 V B) −0.18 V C) −0.12 V D) −0.060 V E) None of these choices are correct. D

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode?

A) Cu( s)→ Cu 2+( aq)+ 2e − B) Cu 2+( aq)+ 2e − → Cu( s) C) Ag( s)→ Ag +( aq)+ e − D) Ag +( aq)+ e − → Ag( s) E) Cu( s)+ 2Ag +( aq)→ Cu 2+( aq)+ 2Ag( s) A) Cu( s)→ Cu 2+( aq)+ 2e − B) Cu 2+( aq)+ 2e − → Cu( s) C) Ag( s)→ Ag +( aq)+ e − D) Ag +( aq)+ e − → Ag( s) E) Cu( s)+ 2Ag +( aq)→ Cu 2+( aq)+ 2Ag( s)

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

A) −3.94 × 10 5 kJ. B) −3.94 × 10 2 kJ. C) −1.97 × 10 5 kJ. D) −7.87 × 10 2 kJ. E) None of these choices are correct. A) −3.94 × 10 5 kJ. B) −3.94 × 10 2 kJ. C) −1.97 × 10 5 kJ. D) −7.87 × 10 2 kJ. E) None of these choices are correct.

A concentration cell consists of two Al/Al3+electrodes. The electrolyte in compartment A is 0.050 M Al(NO3)3 and in compartment B is 1.25 M Al(NO3)3. What is the voltage of the cell at 25°C?

A) 0.083 V B) 0.062 V C) 0.041 V D) 0.028 V E) None of these choices are correct. A) 0.083 V B) 0.062 V C) 0.041 V D) 0.028 V E) None of these choices are correct.

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following reactions occurs at the anode?

A) Al( s)→ Al 3+( aq)+ 3e − B) Al 3+( aq)+ 3e → Al( s) C) Ni( s)→ Ni 2+( aq)+ 2e − D) Ni 2+( aq)+ 2e − → Ni( s) E) None of these choices are correct. A) Al( s)→ Al 3+( aq)+ 3e − B) Al 3+( aq)+ 3e → Al( s) C) Ni( s)→ Ni 2+( aq)+ 2e − D) Ni 2+( aq)+ 2e − → Ni( s) E) None of these choices are correct.

Consider the following balanced redox reaction Mn2+(aq) + S2O82−(aq) + 2H2O(l) → MnO2(s) + 4H(aq) + 2SO42−(aq) Which of the following statements is true?

A) Mn 2+( aq)is the oxidizing agent and is reduced. B) Mn 2+( aq)is the oxidizing agent and is oxidized. C) Mn 2+( aq)is the reducing agent and is oxidized. D) Mn 2+( aq)is the reducing agent and is reduced. E) Manganese does not change its oxidation number in this reaction. A) Mn 2+( aq)is the oxidizing agent and is reduced. B) Mn 2+( aq)is the oxidizing agent and is oxidized. C) Mn 2+( aq)is the reducing agent and is oxidized. D) Mn 2+( aq)is the reducing agent and is reduced. E) Manganese does not change its oxidation number in this reaction.

A voltaic cell is based on the following two half-reactions: Ni+2(aq) + 2e− → Ni(s) E° = −0.25 V Cr+3(aq) + 3e- → Cr(s) E° = -0.74 V Sketch the cell and then select the correct statement about it.

A) Cr serves as the cathode. B) The direction of electron flow through the external wire is from the Ni to the Cr electrode. C) Anions in solution will migrate toward the Ni +2/Ni electrode. D) The net cell reaction is 3Ni +2( aq)+ 2Cr( s)→ 3Ni( s)+ 2Cr +3( aq) E) = 0.99 V A) Cr serves as the cathode. B) The direction of electron flow through the external wire is from the Ni to the Cr electrode. C) Anions in solution will migrate toward the Ni +2/Ni electrode. D) The net cell reaction is 3Ni +2( aq)+ 2Cr( s)→ 3Ni( s)+ 2Cr +3( aq) E) = 0.99 V

Calculate ΔG° 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 are correct. A) −71.4 kJ B) −286 kJ C) −357 kJ D) −428 kJ E) None of these choices are correct.

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Consider the reaction of iodine with manganese dioxide 3I₂(s) + 2MnO₂(s) + 8OH^-(aq) ⇄ 6I⁻(aq) + 2MnO₄(aq) + 4H₂O(l) The equilibrium constant for the overall reaction is 8.30 × 10⁻⁷. Calculate E°_cell for the reaction at 25°C.

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

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? S₂O₈²⁻(aq) + 2H⁺ + 2I⁻(aq) → 2HSO₄⁻(aq) + I₂(aq)

Free

(Multiple Choice)

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Question 3

Correct Answer:

Verified

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 10⁵. Calculate ΔG° for the reaction at 25°C.

(Multiple Choice)

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Question 4

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = −0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

(Multiple Choice)

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Question 5

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I⁻(aq) + NO₃⁻(aq) → NO(g) + I₂(s) (acidic solution)

(Multiple Choice)

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Question 6

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

(Multiple Choice)

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Question 7

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

(Multiple Choice)

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Question 8

A concentration cell consists of two Al/Al³⁺electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃)₃and in compartment B is 1.25 M Al(NO₃)₃. What is the voltage of the cell at 25°C?

(Multiple Choice)

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Question 9

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO₄(aq) + OH⁻(aq) → Al₂O₃(s) + S²⁻(aq) + H₂O(l)

(Multiple Choice)

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Question 10

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e⁻⇄ Cu(s) E° = 0.34 V Sn⁴⁺(aq) + 2e⁻ ⇄ Sn²⁺(aq) E° = 0.13 V

(Multiple Choice)

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Question 11

In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

(True/False)

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Question 12

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

(Multiple Choice)

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Question 13

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈²⁻(aq) + 2H₂O(l) → MnO₂(s) + 4H(aq) + 2SO₄²⁻(aq) Which of the following statements is true?

(Multiple Choice)

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Question 14

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

(Multiple Choice)

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Question 15

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) ⇄ Sn(s) + Fe²⁺(aq)

(Multiple Choice)

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Question 16

The following half-reactions occur in the mercury battery used in calculators. If E°_cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25°C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H₂O(l) + 2e⁻ ⇄ Hg(l) + 2OH⁻(aq) ZnO(s) + H₂O(l) + 2e⁻ ⇄ Zn(s) + 2OH⁻(aq)

(Multiple Choice)

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Question 17

A voltaic cell is based on the following two half-reactions: Ni⁺²(aq) + 2e⁻ → Ni(s) E° = −0.25 V Cr⁺³(aq) + 3e^- → Cr(s) E° = -0.74 V Sketch the cell and then select the correct statement about it.

(Multiple Choice)

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Question 18

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be __________. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

(Multiple Choice)

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Question 19

Calculate ΔG° 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

(Multiple Choice)

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Question 20

Showing 1 - 20 of 101

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Consider the reaction of iodine with manganese dioxide 3I2(s) + 2MnO2(s) + 8OH-(aq) ⇄ 6I−(aq) + 2MnO4(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 × 10−7. Calculate E°cell for the reaction at 25°C.

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 105. Calculate ΔG° for the reaction at 25°C.

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = −0.44 V; all E° values refer to the M2+/M half-cell reactions.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I−(aq) + NO3−(aq) → NO(g) + I2(s) (acidic solution)

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode?

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

A concentration cell consists of two Al/Al3+electrodes. The electrolyte in compartment A is 0.050 M Al(NO3)3 and in compartment B is 1.25 M Al(NO3)3. What is the voltage of the cell at 25°C?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO4(aq) + OH−(aq) → Al2O3(s) + S2−(aq) + H2O(l)

A voltaic cell can be prepared from copper and tin. What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq) + 2e− ⇄ Cu(s) E° = 0.34 V Sn4+(aq) + 2e− ⇄ Sn2+(aq) E° = 0.13 V

In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following reactions occurs at the anode?

Consider the following balanced redox reaction Mn2+(aq) + S2O82−(aq) + 2H2O(l) → MnO2(s) + 4H(aq) + 2SO42−(aq) Which of the following statements is true?

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

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.30 V Sn2+(aq) + Fe(s) ⇄ Sn(s) + Fe2+(aq)

A voltaic cell is based on the following two half-reactions: Ni+2(aq) + 2e− → Ni(s) E° = −0.25 V Cr+3(aq) + 3e- → Cr(s) E° = -0.74 V Sketch the cell and then select the correct statement about it.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be __________. I2(s) + HNO3(aq) → HIO3(aq) + NO2(g) + H2O(l)

Calculate ΔG° 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

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

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 Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

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 Reaction Direction

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Consider the reaction of iodine with manganese dioxide 3I₂(s) + 2MnO₂(s) + 8OH^-(aq) ⇄ 6I⁻(aq) + 2MnO₄(aq) + 4H₂O(l) The equilibrium constant for the overall reaction is 8.30 × 10⁻⁷. Calculate E°_cell for the reaction at 25°C.

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 10⁵. Calculate ΔG° for the reaction at 25°C.

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = −0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I⁻(aq) + NO₃⁻(aq) → NO(g) + I₂(s) (acidic solution)

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

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

A concentration cell consists of two Al/Al³⁺electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃)₃and in compartment B is 1.25 M Al(NO₃)₃. What is the voltage of the cell at 25°C?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO₄(aq) + OH⁻(aq) → Al₂O₃(s) + S²⁻(aq) + H₂O(l)

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e⁻⇄ Cu(s) E° = 0.34 V Sn⁴⁺(aq) + 2e⁻ ⇄ Sn²⁺(aq) E° = 0.13 V

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈²⁻(aq) + 2H₂O(l) → MnO₂(s) + 4H(aq) + 2SO₄²⁻(aq) Which of the following statements is true?

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) ⇄ Sn(s) + Fe²⁺(aq)

A voltaic cell is based on the following two half-reactions: Ni⁺²(aq) + 2e⁻ → Ni(s) E° = −0.25 V Cr⁺³(aq) + 3e^- → Cr(s) E° = -0.74 V Sketch the cell and then select the correct statement about it.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be __________. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

Calculate ΔG° 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