STANDARDChemistry-Electrochemistry
STANDARD Chemistry Gibbs Free Energy and Cell Potential MCQ Question
Type: MCQ-numerical-Medium-Class 12
For the cell reaction: 2Fe³⁺(aq) + 2I⁻(aq) → 2Fe²⁺(aq) + I₂(aq) E°cell = 0.24 V at 298 K. The standard Gibbs energy (ΔG°) of the cell reaction is [Given that Faraday constant, F = 96500 C mol⁻¹]
A
23.16 kJ mol⁻¹
B
−46.32 kJ mol⁻¹
C
−23.16 kJ mol⁻¹
D
46.32 kJ mol⁻¹
Correct Answer
Option B
Detailed Explanation
The standard Gibbs' energy (ΔG°) is calculated using the formula ΔG° = −nFE°cell. For n = 2, ΔG° = −2 × 96500 × 0.24 = −46320 J = −46.32 kJ/mol.
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