\(\text{Given:}\) Equilibrium constant of the reaction (\(K\)) = \(1.2 \times 10^6\). \(\text{To find: Standard potential of cell } (E_{\text{cell}}^\circ)\) \(\text{Formulae: } E_{\text{cell}}^\circ = \frac{0.0592 \, \text{V}}{n} \log_{10} K\) \(\text{Calculation:}\) For the given reaction, \(n = 1\). Using the formula, \[E_{\text{cell}}^\circ = \frac{0.0592}{1} \log_{10} (1.2 \times 10^6)\] \[E_{\text{cell}}^\circ = 0.0592 \times 6.079 = 0.36 \, \text{V}\] The standard cell potential of the cell is \(0.36 \, \text{V}\).