28. The reduction potentials for Au³+ and Ni2+ are as follows: Au3+ + 3e → Au E° = +1.50 V Ni2+ + 2e- → Ni E°=-0.23 V Calculate AG° (at 25°C) for the reaction 2Au3+ + 3Ni→ 3Ni2+ + 2Au (A) -5.00 × 102 kJ (B) +5.00 × 102 kJ (C) -2140 kJ (D) +1.00 × 103 kJ (E) -1.00 × 103 kJ

28. The reduction potentials for Au³+ and Ni²⁺ are as follows:

Au³⁺+ 3e → Au E° = +1.50 V

Ni²⁺ + 2e^- → Ni E°=-0.23 V

Calculate AG° (at 25°C) for the reaction

2Au³⁺ + 3Ni→ 3Ni²⁺ + 2Au
(A) -5.00 × 10²kJ
(B) +5.00 × 10² kJ
(C) -2140 kJ
(D) +1.00 × 10³kJ
(E) -1.00 × 10³kJ

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統計： A(1), B(3), C(0), D(1), E(3) #3340073

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6. A strip of copper is placed in a 1 M solution of copper nitrate, and a strip of silver is placed in a 1 M solution of silver nitrate. The two metal strips are connected to a voltmeter by wires, and a salt bridge connects the solutions. The following standard reduction potentials apply: Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V Cu²⁺(aq) + 2e⁻ → Cu(s) E° = +0.34 V When the voltmeter is removed and the two electrodes are connected by a wire, which of the following does not take place? (A) Electrons flow in the external circuit from the copper electrode to the silver electrode. (B) The silver electrode increases in mass as the cell operates. (C) There is a net general movement of silver ions through the salt bridge to the copper half-cell. (D) Negative ions pass through the salt bridge from the silver half-cell to the copper half-cell. (E) Some positive copper ions pass through the salt bridge from the copper half-cell to the silver half-cell.

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