27. The standard cell potential for the reaction is 1.67 V at 298K. Calculate the standard Gibbs fre — Electrochemistry Chemistry Question
Question
27. The standard cell potential $E^\circ$ for the reaction $2Fe(s) + O_2(g) + 4H^+(aq) \rightarrow 2Fe^{2+}(aq) + 2H_2O(l)$ is 1.67 V at 298K. Calculate the standard Gibbs free energy change ($\Delta G^\circ$) in kJ/mol. (Use 1 F = 96500 C/mol)
Answer: B
💡 Solution & Explanation
The balanced redox reaction transfers 4 moles of electrons ($2Fe \rightarrow 2Fe^{2+} + 4e^-$), so $n=4$. $\Delta G^\circ = -nFE^\circ = -4 \times 96500 \times 1.67 = -644620$ J/mol = -644.6 kJ/mol.
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