For a given reversible reaction at a fixed temperature, equilibrium constants `K_(p)` and `K_(c)` are related by ………

STATEMENT-1: For a given reaction at fixed temperatures, equlibrium constants K_(rho)and K_(c) are realated as K_(rho)=K_(c)(RT)^(Deltan) STATEMENT-2: Deltan =No. of moles of product - No of moles of reactants.

For a gaseous reaction 2B rarr A , the equilibrium constant K_(p) is ……… to // than K_(c) .

For a reversible reaction at 298 K the equilibrium constant K is 200. What is value of DeltaG^(@) at 298 K ?

For a given exothermic reaction , K_P and K_p' are the equilibrium constant at temperature T_1 and T_2 respectively .Assuming that heat of reaction is constant in temperature range between T_1 and T_2 , it is readly observed that

Vant's Hoff's equation shows the effect of temperature on equilibrium constants K_(c) and K_(p) .The K_(P) varies with tempertaure according to the relation:

Prove alpha=sqrt((K_(p)/(P+K_(p)))) for PCl_(5) hArr PCl_(3)+Cl_(2) where alpha is the degree of dissociation at temperature when equilibrium constant is K_(p) .

Which is correct relationship between K_(p) and K_(c) for following reversible reaction at 10 K temperature ? K_(p) and K_(c) in untis of atm and M respectively A_(2)(g)+3B_(2)(g)hArr 2AB_(3)(g)

The equilibrium constant of a reversible reaction at a given temperature

Which is the correct relationship between DeltaG^(@) and equilibrium constant K_(p) ?

The equilibrium constant (K) for the reaction. A+2BhArr2C+D is: