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For the reaction Ag2O(s) → 2Ag(s) + 1/2O2(g) : ∆H = 30.56 kJ mol-1 and ∆S = 6.66 JK-1 mol-1 (at 1 atm). Calculate the temperature at which AG is equal to zero. Also predict the direction of the reaction (i) at this temperature and (ii) below this temperature.

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∆H = 30.56 kJ mol-1 

∆H = 30560 J mol-1 

∆S = 6.66 x 10-3 kJ K-1 mol-1 

T = ? at which ∆G = 0 

∆G = ∆H – T∆S 

0 = ∆H – T∆S

T = ΔH / ΔS

t = 4589 K

(i) At 4589K ; ∆G = 0, the reaction is in equilibrium. 

(ii) At temperature below 4598 K, ∆H > T ∆ S ∆G = ∆H – T∆S > 0, the reaction in the forward direction, is non-spontaneous. In other words the reaction occurs in the backward direction.

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