Δ H and Δ S for the reaction, Ag 2 O ( s ) ⟶ 2 Ag ( s ) + 2 1 O 2 ( g ) , are 30.56 kJ mol − 1 and 66.00 JK − 1 mol − 1 respectively. The temperature at which the free energy change for the reac

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Δ H and Δ S for the reaction, Ag 2 ​ O ( s ) ⟶ 2 Ag ( s ) + 2 1 ​ O 2 ​ ( g ) , are 30.56 kJ mol − 1 and 66.00 JK − 1 mol − 1 respectively. The temperature at which the free energy change for the reaction will be zero, is

TestHub · Accepted Answer

From the Gibb's - Helmholtz equation, Δ G = Δ H − T Δ S At equilibrium, Δ G = 0 Hence, Δ H − T Δ S = 0 or, Δ H = T Δ S Or, T = Δ S Δ H ​ Given that, Δ H = 30.56 kJ mol − 1 ∴ Δ S ∴ T ​ = 30560 J mol − 1 = 66.0 J K − 1 mol − 1 = 66.0 30560 ​ = 463 K ​

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