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InterviewSolution
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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 equilibriu constant. |
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Answer» 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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