A reaction has an equillibrium constant of 0.98 at 300K and 1.2 at 400K. Select the incorrect option:

Acertain rection has equilibrium constant 10 and 100 at 300K and 400K respectively. The ratio of Delta G^(@) at 300K and 400K respectively

Acertain rection has equilibrium constant 10 and 100 at 300K and 400K respectively. The ratio of Delta G^(@) at 300K and 400K respectively

The equilibrium constant for the reaction is 10 at 300K. What will be the value of triangleG^@ ?

The ratio of rate constants of a reaction at 300K and 291K is 2. Calculate the energy of activation. ("Given "R = "8.314JK"^(-1)" mol"^(-1)) .

Equilibrium constant, K changes with temperature. At 300K, equilibrium constant is 25 and at 400K it is 10. Hence, backward reaction will have energy of activation

A reaction has value of Delta H = -40 kcal mol^(-1) at 400 K. Below 400 K the reaction is spontaneous and above 400 K it is not. The value of DeltaG and Delta S at 400 K are respectively

The equilibrium constant for a reaction is 100 what will be the value of ΔG^∘ at 300K?

At equillibrium if K_p =1 then :