The net reaction in a voltaic cell with E°cell = +0.726 V is, 2 Fe³⁺(aq) + 3 Zn(S) → 2 Fe(s) + 3 Zn²⁺(aq)
What is ΔG° for this reaction at 25°C?

Question

The net reaction in a voltaic cell with E°cell = +0.726 V is, 2 Fe³⁺(aq) + 3 Zn(S) → 2 Fe(s) + 3 Zn²⁺(aq) What is ΔG° for this reaction at 25°C?

Quizplus · Accepted Answer

ΔG° can be calculated using the formula ΔG° = -nFE°cell, where n is the number of moles of electrons transferred (6 in this case), F is Faraday's constant (96485 C/mol), and E°cell is the standard cell potential. Substituting the values gives ΔG° = -6 * 96485 * 0.726 = -420 kJ.

The Net Reaction in a Voltaic Cell with E°cell =