Methanol is formed by the following gas phase homogeneous reaction: $$CO (g) + 2H_2 (g) \rightleftharpoons CH_3OH (g)$$ The standard Gibbs free energies of formation at $298\text{ K}$ for $CO$ and $CH_3OH$ are $-137\text{ kJ mol}^{-1}$ and $-162\text{ kJ mol}^{-1}$, respectively. The value of universal gas constant is $8.314\text{ J mol}^{-1}\text{ K}^{-1}$. The equilibrium constant for the given reaction at $298\text{ K}$ is _____ $\times 10^4$ (rounded off to one decimal place).