`Delta G^(@)` for a reaction is `46.06 kcal mol^(-)`. `K_(P)` for the reaction at `300 K` is

Delta G^(@) of a reaction is 120 kJ mol^(-1) . Calculate the K_(p) at 20^(@)C .

The ratio K_(p) to K_( c) of a reaction is 24.63 L atm mol^(-1) at 27^(@) C. If heat of reaction at constant pressure is 98.8 kcal, what is the heat of reaction (in kcal) at constant volume?

The ratio K_(p) to K_( c) of a reaction is 24.63 L atm mol^(-1) at 27^(@) C. If heat of reaction at constant pressure is 98.8 kcal, what is the heat of reaction (in kcal) at constant volume?

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

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^(@) 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)

Calculate Delta_(r )G^(@) for the reaction for which the value of K_(p) is 1.5 xx 10^(10) at 300 K.

Delta G^(0) and Delta H^(0) for a reaction at 300K is -66.9kJmol^(-1) and -41.8kJmol^(-1) respectively. Delta S^(0) for the same reaction at 300K 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: