The equilibrium constant for decomposition of $\text{H}_2\text{O(g)} \text{H}_2\text{O(g)} \rightleftharpoons \text{H}_2\text{(g)} + \frac{1}{2}\text{O}_2\text{(g)} \quad (\Delta G^\circ = 92.34 \, \text{kJ mol}^{-1})$ is $8.0 \times 10^{-3}$ at 2300 K and total pressure at equilibrium is 1 bar. Under this condition, the degree of dissociation ($\alpha$) of water is $\underline{\hspace{2cm}}\times 10^{-2}$(nearest integer value). [Assume $\alpha$ is negligible with respect to 1]