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 ($\Delta G$) for a process is related to the cell potential ($E_{cell}$) and the number of moles of electrons transferred ($n$) by the equation $\Delta G = -nFE_{cell}$, where $F$ is the Faraday constant (approximately 96,485 C/mol or J/V·mol). Given that the cell potential is 1.20 V and assuming one mole of electrons is transferred, the free-energy change would be negative (indicating a spontaneous reaction), and its magnitude can be calculated using the given values. The correct option is the one that reflects a negative change in free energy with the correct sign and magnitude based on the cell potential.

If the Potential of a Voltaic Cell Is +1