The e.m.f. of the cell `Cd(s)|CdCl_(2)(0.1M)||AgCl(s)|Ag(s)` in which the cell reaction is `Cd(s)+2AgCl(s)to2Ag(s)+Cd^(2+)(aq)+2Cl^(-)(aq)`
is 0.6915 V at `0^(@)C` and 0.6753 at `25^(@)C`. Calculate the enthalpy change of the reaction at `25^(@)C`.

Explanation

To calculate the enthalpy change (ΔH) of the reaction at 25°C for the cell reaction \( \text{Cd}(s) + 2\text{AgCl}(s) \rightarrow 2\text{Ag}(s) + \text{Cd}^{2+}(aq) + 2\text{Cl}^-(aq) \), we will follow these steps:

### Step 1: Calculate the change in cell potential (ΔE)
The cell potentials at two different temperatures are given:
- \( E_1 = 0.6915 \, V \) at \( T_1 = 0^\circ C = 273 \, K \)
- \( E_2 = 0.6753 \, V \) at \( T_2 = 25^\circ C = 298 \, K \)

The change in cell potential is:
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