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 equilibrium constant.

For the water gas reaction: `C(s) +H_(2)O(g) hArr CO(g) +H_(2)(g)` the

1.	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 equilibrium constant.
Answer» `-DeltaG^(@)=2.303RTlogK_(C)` `+8.1xx10^(3)=2.303xx8.314xx1000 logK_(C)` `K_(C)=2.648mol litre^(-1)`

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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 equilibrium constant.

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