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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) - Chemistry

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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