For the cell reaction:
2Fe
3+
(aq)+2I
−
(aq)→2Fe
2+
(aq)+I
2
(aq)
E
Cell
∘
=0.24V at 298K. The standard Gibbs energy (Δ
r
G
∘
) of the cell reaction is:
- A−46.32kJ mol
−1 - B−23.16kJ mol
−1 - C46.32kJ mol
−1 - D23.16kJ mol
−1
Solution & Step-by-step Explanation
The relationship between standard Gibbs energy and cell potential is:
Δ
r
G
∘
=−nFE
Cell
∘
From the reaction, 2 electrons are transferred per mole of reaction (n=2).
F=96500C mol
−1
and E
Cell
∘
=0.24V.
Δ
r
G
∘
=−2×96500×0.24=−46320J mol
−1
Δ
r
G
∘
=−46.32kJ mol
−1
Δ
r
G
∘
=−nFE
Cell
∘
From the reaction, 2 electrons are transferred per mole of reaction (n=2).
F=96500C mol
−1
and E
Cell
∘
=0.24V.
Δ
r
G
∘
=−2×96500×0.24=−46320J mol
−1
Δ
r
G
∘
=−46.32kJ mol
−1