Addition of inert gas to system at equilibrium changes only `K_(p)` not `K_(c)`.

Assertion : The additions of an inert gas at constant volume to a system at equilibrium does not affect the state of equilibrium Reason: The inert gas does not react with any of the reactants or products.

Addition of inert gas to system N_(2)(g) + 3H_(2)(g) at equillibrium at constant volume. Then

Assertion :- Addition of inert gas at const pressure to equilibrium of PCl_(5)hArrPCl_(3)+Cl_(2) favourd forward reaction. Reason :- K_(c)=(alpha^(2))/((1-prop)V) for the equilibrium of PCl_(5)hArrPCl_(3)+Cl_(2)

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:

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

In a chemical equilibrium, K_(c)=K_(p) when

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

At a certain temperature and 2 atm pressure equilibrium constant (K_(p)) is 25 for the reaction SO_(2)(g)+NO_(2)(g)hArrSO_(3)(g)+NO(g) Initially if we take 2 moles of each of the four gases and 2 moles of inert gas, what would be the equilibrium partial pressure of NO_(2) ?

The figure shows the change in concentration of species A and B as a function of time. The equilibrium constant K_(c) for the reaction A(g)hArr2B(g) is :

For a gaseous reaction aA(g)+bB(g)hArrcC(g)+dD(g) equilibrium constants K_(c),K_(p) and K_(x) are represented by the following reation K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)),K_(p)=(Pc^(c).P_(D)^(d))/P_(A)^(a) and Kx=(x_(C)^(c).x_(D)^(d))/(x_(A)^(a).x_(B)^(b) where [A] represents molar concentrationof A,p_(A) represents partial pressure of A and P represents total pressure, x_(A) represents mole fraction of For the following equilibrium relation betwen K_(c) and K_(c) (in terms of mole fraction) is PCl_(3)(g)+Cl_(2)(g)hArrPCl_(5)(g)