To calculate the overall standard reduction potential for a series of redox reac tions, use the relationship \(∆G = −nFE^◦\) and combine the contributions from all steps.
The reactions are as follows:
The total Gibbs free energy for the combined reaction is:
\[ \Delta G_3 = \Delta G_1 + \Delta G_2 \]
Substitute \( \Delta G = -nFE^\circ \):
\[ -4FE^\circ_3 = -3F(2.2) + (-1F)(0.7) \]
Simplify the equation:
\[ 4E^\circ_3 = 6.6 + 0.7 = 7.3 \]
Divide by 4:
\[ E^\circ_3 = \frac{7.3}{4} = 1.825 \, \text{V} \]
Express in millivolts:
\[ E^\circ_3 = 1.825 \times 10^3 \, \text{mV} \]
The value of \( x \) is 1825.
The equilibrium constant for decomposition of $ H_2O $ (g) $ H_2O(g) \rightleftharpoons H_2(g) + \frac{1}{2} O_2(g) \quad (\Delta G^\circ = 92.34 \, \text{kJ mol}^{-1}) $ is $ 8.0 \times 10^{-3} $ at 2300 K and total pressure at equilibrium is 1 bar. Under this condition, the degree of dissociation ($ \alpha $) of water is _____ $\times 10^{-2}$ (nearest integer value). [Assume $ \alpha $ is negligible with respect to 1]
Match List-I with List-II: List-I