The value of E°_cell for the reaction
2Cr³⁺(aq) + 6Hg(l) $\to$ 2Cr(s) + 3Hg₂²⁺(aq)
Is 1.59 V.Calculate $\Delta$ G° for the reaction.

Question

The value of E°_cell for the reaction 2Cr³⁺(aq)+ 6Hg(l) $\to$ 2Cr(s)+ 3Hg₂²⁺(aq) Is 1.59 V.Calculate $\Delta$G° for the reaction.

Quizplus · Accepted Answer

The correct answer is A because the value of E°cell is positive, indicating that the reaction is spontaneous and the value of ΔG° is negative, indicating that the reaction is exergonic. The magnitude of ΔG° is calculated as -nFE°cell, where n is the number of moles of electrons transferred in the reaction and F is the Faraday constant. In this case, n = 6 and F = 96,485 C/mol, so ΔG° = -6 × 96,485 C/mol × 1.59 V = -921 kJ/mol.

The Value of E°cell for the Reaction 2Cr3+(aq)+ 6Hg(l) →\to→ 2Cr(s)+ 3Hg22+(aq) Is 1

The Value of E°_cell for the Reaction
2Cr³⁺(aq)+ 6Hg(l) $\to$ 2Cr(s)+ 3Hg₂²⁺(aq)
Is 1