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For the water gas reaction: C(s) +H(2)...

For the water gas reaction:
`C(s) +H_(2)O(g) hArr CO(g) +H_(2)(g)`
the standard Gibbs enegry for the reaction at `1000K` is `-8.1 kJ mol^(-1)`. Calculate its equilibriu constant.

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Verified by Experts

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`
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