RE-NEET 2024 Chemistry Gibbs Free Energy MCQ Question
The standard cell potential of the following cell Zn|Zn²⁺ (aq)|Fe²⁺(aq)|Fe is 0.32 V. Calculate the standard Gibbs energy change for the reaction : Zn(s) + Fe²⁺(aq) → Zn²⁺(aq) + Fe(s) (Given : 1 F = 96487 C)
−61.75 kJ mol⁻¹
+5.006 kJ mol⁻¹
−5.006 kJ mol⁻¹
+61.75 kJ mol⁻¹
Correct Answer
Detailed Explanation
The standard Gibbs energy change (ΔG°) is calculated using the formula ΔG° = −nFE°. Here, n = 2, F = 96487 C/mol, and E° = 0.32 V. Substituting these values gives ΔG° = −2 × 96487 × 0.32 = −61.75 kJ/mol.
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