The cell in which the following reaction occurs:
`2Fe^(3+) (aq) + 2I^(-) (aq) ---> 2Fe^(2+) (aq) + I_2 (s)` has `E_"cell"^@` = 0.236 V at 298 K. Calculate the standard Gibbs energy of the cell reaction. (Given : 1 F = 96,500 C mol−1)
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Solution
Here n = 2, `E_"cell"^@ = 0.236 V`, T = 298 K
We know that
`triangle G^@ = -nFE_"cell"^@`
= −2 × 96500 × 0.236
= −45548 J mol−1
= −45.548 kJ mol−1
Concept: Nernst Equation - Electrochemical Cell and Gibbs Energy of the Reaction
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