`DeltaG` for a reaction at `300 K` is `-16 kcal` and `DeltaH` is `-10 kcal`. The entropy of the reaction is

The Gibbs free energy change of a reaction at 27^(@)C is -26 Kcal. and its entropy change is -60 Cals/K. Delta H for the reaction is :-

The Gibbs free energy change of a reaction at 27^(@)C is -26 Kcal. and its entropy change is -60 Cals/K. Delta H for the reaction is :-

For a reaction A+2BtoC+D , if DeltaH=-25kcal , T=300 K and DeltaS=90 cal , then the reaction is

At 300 K, the enthalpy change and entropy change of a reaction are -10 kcal and -30 " cal". K^(-1) respectively. Does the reaction occur spontaneously at 400 K ? If not, then calculate the maximum temperature at which the reaction will occur spontaneously ?

The reaction A rarr B has Delta H = -10 kcal and E_a = 30 kcal . Find Ea^1 for the reverse reaction.

DeltaG^o for the reaction X + Y hArr Z IS -4.606 kcal. The equilibrium constant for the reaction at 227^Oc is:

DeltaG^(ɵ) for the reaction X+YhArrC is -4.606 kcal at 1000 K . The equilibrium constant for the reverse mode of the reaction will be: