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

Question

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

Accepted Answer

−23.16 kJ mol⁻¹

Answer

46.32 kJ mol⁻¹

Answer

23.16 kJ mol⁻¹

Answer

−46.32 kJ mol⁻¹

NEET 2019 Chemistry Gibbs Free Energy MCQ Question

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