For the reaction, A g + B g → C g + D g , ∆ H o and ∆ S o are, respectively, - 29.8 k J m o l - 1 and - 0.100 k J K - 1 m o l - 1 at 298 K. The equilibrium constant for the reaction at 298 k is:

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∆ G ° = ∆ H ° - T ∆ S ° ∆ G ° = - 29 .8 kJmol - 1 + 0 .1 × 298 kJmol - 1 = 0 ∆ G = ∆ G ° + R T l n Q a t E q u i l i b r i u m ∆ G = 0 & Q = k ∆ G ° = - R T l n( K) i f l n( K) = 0 , K = e 0 ∴ K = 1

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