# 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)

#### 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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