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DeltaH and DeltaS for the reaction: Ag...

`DeltaH` and `DeltaS` for the reaction:
`Ag_(2)O(s) rarr 2Ag(s) +(1//2)O_(2)(g)`
are `30.56 kJ mol^(-1)` and `66.0 J JK^(-1) mol^(-1)` respectively. Calculate the temperature at which free energy change for the reaction will be zero. Predict whether the forward reaction will be favoured above or below this temperature.

Text Solution

Verified by Experts

According to Gibbs Helmholtz equation,
`DeltaG = DeltaH -TDeltaS`
For `DeltaG = 0`
`0 = DeltaH -TDeltaS` or `DeltaH = T DeltaS` or `T = (DeltaH)/(DeltaS)`
Here, `DeltaH = 30.56 kJ mol^(-1) = 30560 J mol^(-1), DeltaS = 6.6 J K^(-1) mol^(-1)`
`therefore T = (30560)/(6.6) = 4630 K`
(i) At 4630 K , the reaction will be at equilibrium because `DeltaG` is zero.
(ii) Below this temperature, `DeltaG` will be `+ve` because both `DeltaH` and `TDeltaS` are positive and `DeltaH gt TDeltaS (DeltaH - TDeltaS = + ve)`. Therefore, the reaction will not be spontaneous below this temperature.
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