Calculate the standard free energy change (DeltaG^(@)) of the following reaction and say whether it is feasible at 373 K or not 1/2K_(2_((g)))+1/2I_(2_((g)))rarrHI_((g)),DeltaH_(r)^(@) " is " 25.95 kJ mol^(-1)standard entropies of HI_((g)) , H_(2_((g))) and I_(2_((g))) are 206.3 ,140.6 and 118.7 Jk^(-1) mol^(-1) Given S_(I_(2))^(@)=118.7 JK^(-1) mol ^(-1),S_(HI)^(@)=206.3JK^(-1) mol^(-1),S_(H_(2))^(@)=140.6 JK^(-1) mol^(-1) Formula : DeltaS^(@)=S_(HI)^(@)1/2(S_(H_(2))^(@)+S_(I_(2)^(@))) Delta G^(@)=DeltaH^(@) -TDeltaS^(@)

Calculate the standard free energy change (DeltaG^(@)) of the followin

1.	Calculate the standard free energy change (DeltaG^(@)) of the following reaction and say whether it is feasible at 373 K or not 1/2K_(2_((g)))+1/2I_(2_((g)))rarrHI_((g)),DeltaH_(r)^(@) " is " 25.95 kJ mol^(-1)standard entropies of HI_((g)) , H_(2_((g))) and I_(2_((g))) are 206.3 ,140.6 and 118.7 Jk^(-1) mol^(-1) Given S_(I_(2))^(@)=118.7 JK^(-1) mol ^(-1),S_(HI)^(@)=206.3JK^(-1) mol^(-1),S_(H_(2))^(@)=140.6 JK^(-1) mol^(-1) Formula : DeltaS^(@)=S_(HI)^(@)1/2(S_(H_(2))^(@)+S_(I_(2)^(@))) Delta G^(@)=DeltaH^(@) -TDeltaS^(@)
Answer» SOLUTION :`DeltaH_(f)^(@)=+25.95kjmol^(-1)` `DeltaS^(@)=sumS_("PRODUCTS")^(@)-sumS_("Reactants")^(@)` `=206.3-1/2(140+118.7)` `=206.3-129.65` `DeltaS^(@)=76.65kJ^(-1)MOL^(-1)` `DeltaG=DeltaG-TDeltaG` `=25.95-(373xx76xx10^(-3)` `=25.95-28.59` `=-2.640kJ^(-1)mol^(-1)`