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:

Step-by-step solution

∆ 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