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For the water gas reaction: <center> C(...

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.

Text Solution

Verified by Experts

We know
`DeltaG^@`=-2.303 RT log K
or log K= `(-G^@)/(2.303RT)`
`DeltaG^@=-8.1 "kJ mol"^(-1)`,T=1000 , `R=8.314xx10^(-3) "kJ mol"^(-1) K^(-1)`
`therefore log K=-(-8.1)/(2.303xx8.314xx10^(-3)xx1000)`
`=0.423`
or `K=2.64`
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