A reaction attains equilibrium state under standard conditions, then
A) equilibrium constant K=0
B) equilibrium constant "K=1
C) `Delta G^(o)=0` and `Delta H^(o)=T Delta S^(o)`
D) `Delta G=0` and `Delta H` = T `Delta S`

In an equilibrium reaction for which Delta G^(@) = 0 , the equilibrium constant K =

Which of the equilibrium constant is measured through the value of Delta G^(@) ?

For a cyclic process,the condition is (A) Delta U=0 only (B) Delta H=0 only (C) Delta U>0 and Delta H>0 (D) both Delta U=0 and Delta H=0

Ths standard free energy change Delta G^(@) is related to K (equilibrium constant ) as

A gaseous reaction A(g) hArrB(g) is at equilibrium under standard condition and 200 K. Calculate the equilibrium constant of the reaction at 400 K if DeltaS_("reaction")^(@)=6xx10^(-5) T^(2) cal//K , where T is temperature in kelvin. [Given : R = 2 cal//mol K " and " "In " 2=0.7 ]

For a spontaneous reaction the Delta G , Equilibrium cosntant (K) and E_(cell)^(@) will be respectively :

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

The equilibrium constant K_(p) for a reaction at "300K" was found to be 10^(4) What will be Delta G^(@) for reaction at same temperature