The cell in which the following reaction occurs

Asked by admin @ 29/08/2021 in Chemistry viewed by 303 People

The cell in which the following reaction occurs:

2Fe 3+ (aq) + 21" (aq) →2Fe2+ (aq) +1, (s) has E = 0.236 V at 298 K.Calculate the standard Gibbs energy and the equilibrium constant of thecell reaction.

Answered by admin @ 29/08/2021

Given :

E° of the cell = 0.236 V

Temperature (T) = 298 K

To Find :

Standard Gibbs energy

Equilibrium constant of the reaction

Solution :

The cell reaction is

$2Fe^{3+}(aq)+2I^-(aq)\rightarrow 2Fe^{2+}(aq)+I_{2}(s)$

The standard Gibbs energy for the reaction

$\Delta G_{0}=-nFE^{0}_{cell}$

$\Delta G_{0}=-2\times0.236 \times96487$

$\Delta G_{0}= -45.54 kJ/mol$

The Gibb’s energy for the reaction is -45.54 kJ/mol.

We know the relation

$logK_{c}=\frac{nFE^{0}_{cell)}}{2.303RT}$

$logK_{c}=\frac{2\times96487 \times0.326}{2.303 \times8.31 \times298}$

$logK_{c}=7.9854$

$K_{c}=9.62\times10^{7}$

The equilibrium constant for the reaction is 9.62×10⁷.

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