For the reaction at `27^(@)``C,X_(2)O_(4("liquid"))rarr2XO_(2(gas))` if `Delta U=1.8kcal`,`Delta S=20calK^(-1)` find magnitude of`` Delta G` in kcal

For the reaction at 25^(@)C, C_(2)O_(4)(l) rarr 2XO_(2)(g) Delta H =2.1 kcal and DeltaS=20 cal K^(-1) . The reaction would be :

For the reaction: X_(2)O_(4)(l)rarr2XO_(2)(g) DeltaU=2.1 cal , DeltaS =20 "cal" K^(-1) "at" 300 K Hence DeltaG is

For the reaction, X_(2)O_(4)(I) rightarrow 2XO_(2)(g) Delta cup = 2.1 k cal, Delta S = 20 cal K^(-1) at 300 K hence, DeltaG is

For the reaction, X_(2)O_(4)(l)rarr2XO_(2)(g),DeltaE=2.1Kcal , DeltaS=20cal//K at 300K . Hence DeltaG is

Gibbs-Helmoholtz equation relates the free energy change to the enthalpy and entropy changes of the process as (DeltaG)_(PT) = DeltaH - T DeltaS The magnitude of DeltaH does not change much with the change in temperature but the enrgy factor T DeltaS changes appreciably. Thus, spontaneity of a process depends very much on temperature. For the reaction at 25^(2)C, X_(2)O_(4)(l) rarr 2XO_(2) DeltaH = 2.0 kcal and DeltaS = 20 cal K^(-1) . the reaction would be