For the water gas reaction,
`C(s) +H_(2)O(g) hArr CO(g)+H_(2)(g)`
the standard Gobbs free energy of reaction (at `1000K)` is `-8.1 kJ mol^(-1)`. Calculate its equilibrium constant.

Explanation

We know that:
`Delta_(r)G^(Theta) = - 2.303 RT log K`
or `logK = (-Delta_(r)G)/(2.303 RT)`
`Delta_(r)G^(Theta) =- 8.1 kJ mol^(-1), T = 1000K`,
`R = 8.314 xx 10^(-3) kJ mol^(-1)K^(-1)`
`:. Log K =- (8.1)/(2.303 xx 8.314 xx 10^(-3) xx 1000) = 0.423`
or `K = 2.64`