`Delta G^(@)` for the reaction `X+Y hArr Z` is -4.606 kcal. The value of equilibrium constant of the reaction at `227^(@)C` is (R = 2 Cal/mol K)

Delta G^(0) for the reaction x + y hArr z is -4.606 kcal. The value of equilibrium constant of the reaction at 227^(@)C

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

Delta H^(@) for the reaction X_((g))+Y_((g))hArrZ_((g)) is -4.6 kcal , the valueof DeltaU^(@) of th e reaction at 227^(@)C is (R=2 cal.mol^(-1)K^(-1)) :

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:

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:

What will be the value of Delta G .If equilibrium constant for a reaction is 10 at 300K

For the reaction A hArr B, DeltaE for the reaction is –33.0 kJ mol^(–1) . Calculate equilibrium constant K_C for the reaction at 300 K