Determine E°cell for the reaction: MnO4- + 8 H+ + 5 Fe2+ → Mn2+ + 4 H2O + 5 Fe3+. The half reactions are: Fe3+(aq) + e- → Fe2+(aq) &emsp; E° = +0.771 V MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) &emsp; E° = 1.507 V

A) -2.34 V B) -2.28 V C) 2.28 V D) -0.74 V E) 0.74 V A) -2.34 V B) -2.28 V C) 2.28 V D) -0.74 V E) 0.74 V

Consider the cell: Ni ∣ Ni2+ (?M) || Cu2+ (0.136 M) ∣ Cu Ni2+/Ni E° = -0.257 V Cu2+/Cu E° = 0.340 V The measured potential of the cell is 0.621 V. What is [Ni2+] at 25°C?

A) 2 × 10-2 M B) 1 M C) 4 × 10-42 M D) 0.05 M E) 0.4 M A) 2 × 10-2 M B) 1 M C) 4 × 10-42 M D) 0.05 M E) 0.4 M

For the reaction: Mg(s) + 2 AgNO3(aq) → 2 Ag(s) + Mg(NO3)2(aq) Write a voltaic diagram for the reaction.

A) Ag(s) | Ag(aq) || Mg2+(aq) | Mg(s) B) Mg(s) ∣ Mg2+ || Ag+ (aq) ∣ Ag (s) C) Mg(s) ∣ Mg2+ || Ag(s) ∣ Ag+ (aq) D) Ag(aq) ∣ Ag(s) || Mg(s) ∣ Mg2+ (aq) E) Ag(s) ∣ Mg2+ (aq) || Ag+ (aq) ∣ Mg(s) A) Ag(s) | Ag(aq) || Mg2+(aq) | Mg(s) B) Mg(s) ∣ Mg2+ || Ag+ (aq) ∣ Ag (s) C) Mg(s) ∣ Mg2+ || Ag(s) ∣ Ag+ (aq) D) Ag(aq) ∣ Ag(s) || Mg(s) ∣ Mg2+ (aq) E) Ag(s) ∣ Mg2+ (aq) || Ag+ (aq) ∣ Mg(s)

Determine E°cell for the reaction: 2 Al + 3 Zn2+ → 2 Al3+ + 3 Zn. The half reactions are: Al3+(aq) + 3 e- → Al(s) &emsp; E° = -1.676 V Zn2+(aq) + 2 e- → Zn(s) &emsp; E° = -0.763 V

A) 0.913 V B) -2.439 V C) 2.439 V D) -1.063 V E) -0.913 V A) 0.913 V B) -2.439 V C) 2.439 V D) -1.063 V E) -0.913 V

Two cells containing solutions of AgNO3 and CuSO4, respectively, were connected in series and electrolyzed. The cathode in the AgNO3 cell was found to gain 1.078 grams in weight. How much had the cathode in the other cell gained?

A) 0.127 g B) 0.6354 g C) 3.175 g D) 0.318 g E) 0.254 g A) 0.127 g B) 0.6354 g C) 3.175 g D) 0.318 g E) 0.254 g

Determine E°cell for the reaction: 2 Al3+ + 3 Zn → 2 Al + 3 Zn2+. The half reactions are: Al3+(aq) + 3 e- → Al(s) &emsp; E° = -1.676 V Zn2+(aq) + 2 e- → Zn(s) &emsp; E° = -0.763 V

A) 0.913 V B) -2.439 V C) 2.439 V D) -1.063 V E) -0.913 V A) 0.913 V B) -2.439 V C) 2.439 V D) -1.063 V E) -0.913 V

Determine E°cell for the reaction: I2 + Cu → 2 I- + Cu2+. The half reactions are: I2(s) + 2 e- → 2 I-(aq) &emsp; E° = +0.535 V Cu2+ + 2 e- → Cu &emsp; E° = 0.340 V

A) 0.730 V B) -0.875 V C) 0.875 V D) 0.195 V E) -0.195 V A) 0.730 V B) -0.875 V C) 0.875 V D) 0.195 V E) -0.195 V

What is the cell diagram for the spontaneous cell involving the Fe3+ ∣ Fe2+ (0.771V) half cell and the Zn2+ ∣ Zn (-0.763 V) half cell?

A) Fe2+(aq) ∣ Fe3+(aq) || Zn2+(aq) ∣ Zn(s) B) Pt(s) ∣ Fe2+(aq), Fe3+(aq) || Zn2+(aq) ∣ Zn(s) C) Zn(s) ∣ Zn2+(aq) || Fe3+(aq) ∣ Fe2+(aq) ∣ Pt(s) D) Zn(s) ∣ Zn2+(aq) || Fe3+(aq) ∣ Fe2+(aq) E) Zn(s) ∣ Zn2+(aq) || Fe3+(aq) ∣ Fe2+(aq) ∣ Zn(s) A) Fe2+(aq) ∣ Fe3+(aq) || Zn2+(aq) ∣ Zn(s) B) Pt(s) ∣ Fe2+(aq), Fe3+(aq) || Zn2+(aq) ∣ Zn(s) C) Zn(s) ∣ Zn2+(aq) || Fe3+(aq) ∣ Fe2+(aq) ∣ Pt(s) D) Zn(s) ∣ Zn2+(aq) || Fe3+(aq) ∣ Fe2+(aq) E) Zn(s) ∣ Zn2+(aq) || Fe3+(aq) ∣ Fe2+(aq) ∣ Zn(s)

For the cell reaction at 25°C Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq), E°cell = +1.100 V. What is the equilibrium constant for this reaction?

A) 3 × 10-19 B) 2 × 1037 C) 2 × 10-37 D) 3 × 1018 E) 3 × 10-18 A) 3 × 10-19 B) 2 × 1037 C) 2 × 10-37 D) 3 × 1018 E) 3 × 10-18

Exam 20: Electrochemistry

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Determine E°cell for the reaction: MnO₄^- + 8 H⁺+ 5 Fe²⁺ → Mn²⁺ + 4 H₂O + 5 Fe³⁺. The half reactions are: Fe³⁺(aq) + e- → Fe²⁺(aq) E° = +0.771 V MnO₄^-(aq) + 8 H⁺(aq) + 5 e- → Mn²⁺(aq) + 4 H₂O(l) E° = 1.507 V

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Question 81

Choose the INCORRECT statement.

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Question 82

3.53 L of 0.362 M CuCl₂(aq) solution are electrolyzed for 55.6 minutes with a current of 14.0-amperes. What is [CuCl₂] when the electrolysis ends?

(Multiple Choice)

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Question 83

What mass of silver can be deposited by the passage of a constant current of 5.00 A through a AgNO₃ solution for 2.00 hours?

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Question 84

Consider the cell: Ni ∣ Ni²⁺ (?M) || Cu²⁺(0.136 M) ∣ Cu Ni²⁺/Ni E° = -0.257 V Cu²⁺/Cu E° = 0.340 V The measured potential of the cell is 0.621 V. What is [Ni²⁺] at 25°C?

(Multiple Choice)

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Question 85

Zn+2(aq) + 2 e- → Zn(s) E° = -0.763 V

(Multiple Choice)

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Question 86

For the reaction: Mg(s) + 2 AgNO₃(aq) → 2 Ag(s) + Mg(NO₃)₂(aq) Write a voltaic diagram for the reaction.

(Multiple Choice)

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Question 87

Determine E°cell for the reaction: 2 Al + 3 Zn²⁺ → 2 Al³⁺ + 3 Zn. The half reactions are: Al³⁺(aq) + 3 e- → Al(s) E° = -1.676 V Zn²⁺(aq) + 2 e- → Zn(s) E° = -0.763 V

(Multiple Choice)

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Question 88

The hydrogen standard electrode is the most convenient standard electrode to use.

(True/False)

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Question 89

Two cells containing solutions of AgNO₃ and CuSO₄, respectively, were connected in series and electrolyzed. The cathode in the AgNO₃ cell was found to gain 1.078 grams in weight. How much had the cathode in the other cell gained?

(Multiple Choice)

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Question 90

Find Ecell at 25°C for the following voltaic cell: Cu(s) ∣ Cu2+(aq) (0.10 M) || Cu2+(aq) (0.85 M) ∣ Cu(s) The half-reaction is: Cu2+(aq) + 2 e- → Cu(s) E° = +0.377 volts

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Question 91

Determine E°cell for the reaction: 2 Al³⁺ + 3 Zn → 2 Al + 3 Zn²⁺. The half reactions are: Al3+(aq) + 3 e- → Al(s) E° = -1.676 V Zn²⁺(aq) + 2 e- → Zn(s) E° = -0.763 V

(Multiple Choice)

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Question 92

A primary battery is recharged by passing electricity through the battery.

(True/False)

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Question 93

Determine E°cell for the reaction: I₂ + Cu → 2 I- + Cu²⁺. The half reactions are: I₂(s) + 2 e- → 2 I-(aq) E° = +0.535 V Cu²⁺ + 2 e- → Cu E° = 0.340 V

(Multiple Choice)

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Question 94

What is the cell diagram for the spontaneous cell involving the Fe³⁺ ∣ Fe²⁺ (0.771V) half cell and the Zn²⁺ ∣ Zn (-0.763 V) half cell?

(Multiple Choice)

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Question 95

Choose the INCORRECT statement.

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Question 96

For the cell reaction at 25°C Cu²⁺(aq) + Zn(s) → Cu(s) + Zn²⁺(aq), E°cell = +1.100 V. What is the equilibrium constant for this reaction?

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Question 97

In the electrolysis of water, oxygen is evolved at the cathode.

(True/False)

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Question 98

What is Keq at 25°C of the spontaneous cell made from Ag⁺/Ag (0.80 V) and Cl₂/Cl- (1.36 V) half cells?

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Question 99

Choose the INCORRECT completion of the following sentence: "In the electrolysis of water...

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Question 100

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Exam 20: Electrochemistry

Determine E°cell for the reaction: MnO4- + 8 H+ + 5 Fe2+ → Mn2+ + 4 H2O + 5 Fe3+. The half reactions are: Fe3+(aq) + e- → Fe2+(aq) E° = +0.771 V MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) E° = 1.507 V

Choose the INCORRECT statement.

3.53 L of 0.362 M CuCl2(aq) solution are electrolyzed for 55.6 minutes with a current of 14.0-amperes. What is [CuCl2] when the electrolysis ends?

What mass of silver can be deposited by the passage of a constant current of 5.00 A through a AgNO3 solution for 2.00 hours?

Consider the cell: Ni ∣ Ni2+ (?M) || Cu2+ (0.136 M) ∣ Cu Ni2+/Ni E° = -0.257 V Cu2+/Cu E° = 0.340 V The measured potential of the cell is 0.621 V. What is [Ni2+] at 25°C?

Zn+2(aq) + 2 e- → Zn(s) E° = -0.763 V

For the reaction: Mg(s) + 2 AgNO3(aq) → 2 Ag(s) + Mg(NO3)2(aq) Write a voltaic diagram for the reaction.

Determine E°cell for the reaction: 2 Al + 3 Zn2+ → 2 Al3+ + 3 Zn. The half reactions are: Al3+(aq) + 3 e- → Al(s) E° = -1.676 V Zn2+(aq) + 2 e- → Zn(s) E° = -0.763 V

The hydrogen standard electrode is the most convenient standard electrode to use.

Two cells containing solutions of AgNO3 and CuSO4, respectively, were connected in series and electrolyzed. The cathode in the AgNO3 cell was found to gain 1.078 grams in weight. How much had the cathode in the other cell gained?

Find Ecell at 25°C for the following voltaic cell: Cu(s) ∣ Cu2+(aq) (0.10 M) || Cu2+(aq) (0.85 M) ∣ Cu(s) The half-reaction is: Cu2+(aq) + 2 e- → Cu(s) E° = +0.377 volts

Determine E°cell for the reaction: 2 Al3+ + 3 Zn → 2 Al + 3 Zn2+. The half reactions are: Al3+(aq) + 3 e- → Al(s) E° = -1.676 V Zn2+(aq) + 2 e- → Zn(s) E° = -0.763 V

A primary battery is recharged by passing electricity through the battery.

Determine E°cell for the reaction: I2 + Cu → 2 I- + Cu2+. The half reactions are: I2(s) + 2 e- → 2 I-(aq) E° = +0.535 V Cu2+ + 2 e- → Cu E° = 0.340 V

What is the cell diagram for the spontaneous cell involving the Fe3+ ∣ Fe2+ (0.771V) half cell and the Zn2+ ∣ Zn (-0.763 V) half cell?

Choose the INCORRECT statement.

For the cell reaction at 25°C Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq), E°cell = +1.100 V. What is the equilibrium constant for this reaction?

In the electrolysis of water, oxygen is evolved at the cathode.

What is Keq at 25°C of the spontaneous cell made from Ag+/Ag (0.80 V) and Cl2/Cl- (1.36 V) half cells?

Choose the INCORRECT completion of the following sentence: "In the electrolysis of water...

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Determine E°cell for the reaction: MnO₄^- + 8 H⁺+ 5 Fe²⁺ → Mn²⁺ + 4 H₂O + 5 Fe³⁺. The half reactions are: Fe³⁺(aq) + e- → Fe²⁺(aq) E° = +0.771 V MnO₄^-(aq) + 8 H⁺(aq) + 5 e- → Mn²⁺(aq) + 4 H₂O(l) E° = 1.507 V

3.53 L of 0.362 M CuCl₂(aq) solution are electrolyzed for 55.6 minutes with a current of 14.0-amperes. What is [CuCl₂] when the electrolysis ends?

What mass of silver can be deposited by the passage of a constant current of 5.00 A through a AgNO₃ solution for 2.00 hours?

Consider the cell: Ni ∣ Ni²⁺ (?M) || Cu²⁺(0.136 M) ∣ Cu Ni²⁺/Ni E° = -0.257 V Cu²⁺/Cu E° = 0.340 V The measured potential of the cell is 0.621 V. What is [Ni²⁺] at 25°C?

For the reaction: Mg(s) + 2 AgNO₃(aq) → 2 Ag(s) + Mg(NO₃)₂(aq) Write a voltaic diagram for the reaction.

Determine E°cell for the reaction: 2 Al + 3 Zn²⁺ → 2 Al³⁺ + 3 Zn. The half reactions are: Al³⁺(aq) + 3 e- → Al(s) E° = -1.676 V Zn²⁺(aq) + 2 e- → Zn(s) E° = -0.763 V

Two cells containing solutions of AgNO₃ and CuSO₄, respectively, were connected in series and electrolyzed. The cathode in the AgNO₃ cell was found to gain 1.078 grams in weight. How much had the cathode in the other cell gained?

Determine E°cell for the reaction: 2 Al³⁺ + 3 Zn → 2 Al + 3 Zn²⁺. The half reactions are: Al3+(aq) + 3 e- → Al(s) E° = -1.676 V Zn²⁺(aq) + 2 e- → Zn(s) E° = -0.763 V

Determine E°cell for the reaction: I₂ + Cu → 2 I- + Cu²⁺. The half reactions are: I₂(s) + 2 e- → 2 I-(aq) E° = +0.535 V Cu²⁺ + 2 e- → Cu E° = 0.340 V

What is the cell diagram for the spontaneous cell involving the Fe³⁺ ∣ Fe²⁺ (0.771V) half cell and the Zn²⁺ ∣ Zn (-0.763 V) half cell?

For the cell reaction at 25°C Cu²⁺(aq) + Zn(s) → Cu(s) + Zn²⁺(aq), E°cell = +1.100 V. What is the equilibrium constant for this reaction?

What is Keq at 25°C of the spontaneous cell made from Ag⁺/Ag (0.80 V) and Cl₂/Cl- (1.36 V) half cells?