`DeltaH and DeltaS` for the reaction
`Ag_(2)O_((s))rarr2Ag_((s))+1/2O_(2_((g))) " are "30.56 kJ mol^(-1)`
and `66.0 Jk^(-1) mol^(-1)` respectively. Calculate the temperature at which the free energy for this reaction will be zero. What will be the direction of reaction at this temperature and at temperature below this and why ?
Given: `DeltaH=30.56kJ mol^(-1)=30560 J mol^(-1)`
`DeltaS=66.0JK^(-1)mol^(-1)`
`DeltaG=0`

Explanation

`DeltaG=DeltaH-TDeltaS` `T=(DeltaH-DeltaG)/(DeltaS)=(30560-0)/(66)=463`
`T=463K.`
At 463 K, the reaction is at equilibrium
At `Tgt463 K , DeltaG` will have positive value hence backward reaction is favoured.