The equilibrium constant (K_p$K_p$) for the thermal decomposition of water vapor: textH_2textO(g) rightleftharpoons textH_2text(g) + frac12textO_2text(g) quad (Delta G^circ = 92.34 text kJ mol^-1)$$\text{H}_2\text{O(g)} \rightleftharpoons \text{H}_2\text{(g)} + \frac{1}{2}\text{O}_2\text{(g)} \quad (\Delta G^\circ = 92.34 \text{ kJ mol}^{-1})$$ is evaluated as 8.0 times 10^-3$8.0 \times 10^{-3}$ at 2300 text K$2300 \text{ K}$ under a total pressure of 1 text bar$1 \text{ bar}$. Under these specific conditions, the degree of dissociation (alpha$\alpha$) of water is _________ times 10^-2$\times 10^{-2}$ (as the nearest integer value). [Assume alpha ll 1$\alpha \ll 1$].

### Related Formula K_C = frac[textProducts][textReactants]$$K_C = \frac{[\text{Products}]}{[\text{Reactants}]}$$ ### Core Logic K_C = fractextProducts ion conc.textReactants ion conc.$$K_C = \frac{\text{Products ion conc.}}{\text{Reactants ion conc.}}$$ K_C = frac[FeSCN^2+][Fe^3+][SCN^-]$$K_C = \frac{[FeSCN^{2+}]}{[Fe^{3+}][SCN^{-}]}$$ ### Evaluation Rubric / Model Answer null ### Chapter Mix Class 11 Chemistry: Equilibrium