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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 equilibrium constant. (Multiply your answer with 100 and then write value)

Text Solution

Verified by Experts

The correct Answer is:
264
We know
`Delta_(r)G^(@) = -2.303 RT log K`
or `log K = (-Delta_(r)G)/(2.303 RT)`
`Delta_(r)G^(@) = -8.1 kJ mol^(-1), T = 1000K, `
`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`
or K = 2.64.
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