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

DeltaH and DeltaS for the reaction Ag_(2)O_((s))rarr2Ag_((s))+1/2O_(2

1.	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
Answer» Solution :Given: `DELTAH=30.56 "kJ mol"^(-1)` `=30560 J mol^(-1)` `DeltaS=6.66 xx 10^(-3) kJ K^(-1) "mol"^(-1)` T=? At which `DeltaG=0` `DeltaG=DeltaH-TDeltaS` `0=DeltaH-TDeltaS` `T=(DeltaH)/(DeltaS)` `T=("30.56 kJ mol"^(-1))/(6.66xx10^(-3) kJ K^(-1) "mol"^(-1))` T=4589 K (i) At 4589 K , `DeltaG=0` , the reaction is in equilibrium . (ii)At temperature below 4598 K, `DeltaH > TDeltaS` `DeltaG=DeltaH-T DeltaS > 0`, the reaction in the FORWARD direction, is non-spontaneous. In other words the reaction occurs in the backward direction.