A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V). Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

A) 0.001 M B) 0.002 M C) 0.01 M D) 0.02 M E) 0.04 M A) 0.001 M B) 0.002 M C) 0.01 M D) 0.02 M E) 0.04 M

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

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.

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)

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 ΔG° for the reaction at 25°C.

A) -15.1 kJ B) -34.7 kJ C) 15.1 kJ D) 34.7 kJ E) None of these choices are correct. A) -15.1 kJ B) -34.7 kJ C) 15.1 kJ D) 34.7 kJ E) None of these choices are correct.

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu2+(aq) + 2e- → Cu(s) and Ag+(aq) + e- → Ag(s) For every 1.00 g of copper produced in the first process, how many grams of silver will be Produced in the second one?

A) 0.294 g B) 0.588 g C) 0.850 g D) 1.70 g E) 3.40 g A) 0.294 g B) 0.588 g C) 0.850 g D) 1.70 g E) 3.40 g

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 zinc and iodine has the following cell notation. Zn(s) | Zn2+(aq) || I-(aq) | I2(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

A) 2I-(aq) + Zn2+(aq) → I2(s) + Zn(s) B) I2(s) + Zn(s) → 2I-(aq) + Zn2+(aq) C) 2I-(aq) + Zn(s) → I2(s) + Zn2+(aq) D) I2(s) + Zn2+(aq) → 2I-(aq) + Zn(s) E) None of these choices are correct. A) 2I-(aq) + Zn2+(aq) → I2(s) + Zn(s) B) I2(s) + Zn(s) → 2I-(aq) + Zn2+(aq) C) 2I-(aq) + Zn(s) → I2(s) + Zn2+(aq) D) I2(s) + Zn2+(aq) → 2I-(aq) + Zn(s) E) None of these choices are correct.

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr2+(aq) + 2e- Cr(s) E° = -0.913 V Fe2+(aq) + 2e- Fe(s) E° = -0.447 V Sr2+(aq) + 2e- Sr(s) E° = -2.89 V Co2+(aq) + 2e- Co(s) E° = -0.28 V

A) Cr2+(aq) B) Fe(s) C) Fe2+(aq) D) Sr2+(aq) E) Co2+(aq) A) Cr2+(aq) B) Fe(s) C) Fe2+(aq) D) Sr2+(aq) E) Co2+(aq)

Exam 21: Electrochemistry Chemical Change and Electrical Work

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/Cu²⁺ electrode (E° = 0.34 V). Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

(Multiple Choice)

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Question 81

Which of the following types of electrochemical cell is most likely to find use in the future as a power source for electric vehicles?

(Multiple Choice)

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Question 82

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 83

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.

(Multiple Choice)

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Question 84

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

(Multiple Choice)

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Question 85

A battery that cannot be recharged is a

(Multiple Choice)

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Question 86

In the absence of oxygen, iron will rust as long as moisture is present.

(True/False)

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Question 87

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 88

Which of the following conditions is most likely to apply to a fully-charged secondary cell?

(Multiple Choice)

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Question 89

Which one of the following statements about electrochemical cells is correct?

(Multiple Choice)

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Question 90

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 ΔG° for the reaction at 25°C.

(Multiple Choice)

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Question 91

A buried iron pipe can be protected against corrosion by connecting it to a rod of copper.

(True/False)

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Question 92

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu²⁺(aq) + 2e^- → Cu(s) and Ag⁺(aq) + e_- → Ag(s) For every 1.00 g of copper produced in the first process, how many grams of silver will be Produced in the second one?

(Multiple Choice)

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Question 93

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 94

Calculate the potential of a voltaic cell (E°_cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

(Multiple Choice)

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Question 95

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

(Multiple Choice)

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Question 96

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?

(Multiple Choice)

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Question 97

A primary battery is one that can be recharged.

(True/False)

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Question 98

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²₊(aq) || I^-(aq) | I₂(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

(Multiple Choice)

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Question 99

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^- Cr(s) E° = -0.913 V Fe²⁺(aq) + 2e^- Fe(s) E° = -0.447 V Sr²⁺(aq) + 2e^- Sr(s) E° = -2.89 V Co²⁺(aq) + 2e^- Co(s) E° = -0.28 V

(Multiple Choice)

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Question 100

Showing 81 - 100 of 100

Exam 21: Electrochemistry Chemical Change and Electrical Work

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V). Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

Which of the following types of electrochemical cell is most likely to find use in the future as a power source for electric vehicles?

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.

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.

A battery that cannot be recharged is a

In the absence of oxygen, iron will rust as long as moisture is present.

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

Which of the following conditions is most likely to apply to a fully-charged secondary cell?

Which one of the following statements about electrochemical cells is correct?

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 ΔG° for the reaction at 25°C.

A buried iron pipe can be protected against corrosion by connecting it to a rod of copper.

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.

Calculate the potential of a voltaic cell (E° cell) if it is required to do 5.43 × 10-3 kJ of work when a charge of 2.50 C is transferred.

Which of the following statements about voltaic and electrolytic cells is 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 primary battery is one that can be recharged.

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn2+(aq) || I-(aq) | I2(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr2+(aq) + 2e- Cr(s) E° = -0.913 V Fe2+(aq) + 2e- Fe(s) E° = -0.447 V Sr2+(aq) + 2e- Sr(s) E° = -2.89 V Co2+(aq) + 2e- Co(s) E° = -0.28 V

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Organic Compounds and the Atomic Properties of Carbon

Kinetics Rates and Mechanisms of Chemical Reactions

Equilibrium the Extent of Chemical Reactions

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Ionic Equilibria in Aqueous Systems

Thermodynamics Entropy, Free Energy, and Reaction Direction

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

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A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/Cu²⁺ electrode (E° = 0.34 V). Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

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.

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.

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 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 ΔG° for the reaction at 25°C.

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.

Calculate the potential of a voltaic cell (E°_cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

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 voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²₊(aq) || I^-(aq) | I₂(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^- Cr(s) E° = -0.913 V Fe²⁺(aq) + 2e^- Fe(s) E° = -0.447 V Sr²⁺(aq) + 2e^- Sr(s) E° = -2.89 V Co²⁺(aq) + 2e^- Co(s) E° = -0.28 V