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

For the water gas reaction,
`C_((s)) + H_2O_((g)) to CO_((g)) + H_(2(g))` the standard Gibbs energy for the reaction at 1000 K is `-8.1 kJ mol^(-1)`. Calculate its equilibrium constant.

Text Solution

Verified by Experts

`DeltaG^@ = -2.303RT log K`
or `log K = (- Delta G^@)/(2.303 RT)`
`DeltaG^@ = -8.1 kJ mol^(-1) , T = 1000`
`R = 8.314 xx 10^(-3) kJ mol^(-1) K^(-1)`
`therefore log K = (-8.1)/(2.303 xx 8.314 xx 10^(-3) xx 1000) = 0.423`
`implies K = 2.65`
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