If the potential of a voltaic cell is +1.20 V, what is the free-energy change when one mole of electrons is transferred in the oxidation-reduction reaction?

Question

Quizplus · Accepted Answer

The free-energy change (ΔG) for a voltaic cell can be calculated using the equation ΔG = -nFE, where n is the number of moles of electrons transferred, F is the Faraday constant (96,485 C/mol), and E is the cell potential.

In this case, n = 1 (since one mole of electrons is transferred), F = 96,485 C/mol, and E = +1.20 V. Plugging these values into the equation, we get:

ΔG = -nFE = -(1 mol)(96,485 C/mol)(+1.20 V) = -116,082 J = -116 kJ

Therefore, the free-energy change when one mole of electrons is transferred in the oxidation-reduction reaction is -116 kJ. The correct answer is D.

If the Potential of a Voltaic Cell Is +1