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° = -nFE°cell, where n is the number of moles of electrons transferred (6 in this case, from the balanced equation), F is the Faraday constant (96485 C/mol), and E°cell is the cell potential (0.726 V). Calculating gives ΔG° = -6 * 96485 * 0.726 = -420 kJ.

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

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