If ?_rG° for the following reaction is -22.2 kJ/mol-rxn, calculate $E _ { \text {cell } } ^ { \circ }$ for the following reaction: Cu²⁺(aq) + 2 Ag(s) + 2 Cl^-(aq) ? Cu(s) + 2 AgCl(s)

Question

Quizplus · Accepted Answer

The relationship between Gibbs free energy change and cell potential is given by the equation: ΔG° = -nFE°cell. Here, ΔG° = -22.2 kJ/mol = -22200 J/mol, n = 2 (since 2 electrons are transferred), and F = 96485 C/mol. Solving for E°cell gives E°cell = -ΔG°/(nF) = 22200/(2*96485) = +0.115 V.

If ?rG° for the Following Reaction Is -22 Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​

If ?_rG° for the Following Reaction Is -22 $E _ { \text {cell } } ^ { \circ }$