Question

What is the relation between Kp and Kx ? (Chemical equilibrium)

Answer 1

Answer-S : Kc, Kp and Kx are the equilibrium constants of a reaction in terms of concentration, pressure and mole fraction respectively. E : Kc and Kp do not depend on equilibrium pressure but Kx depends upon equilibrium pressure if Δn=0.

Answer 2

Answer:

The relation between Kp and Kx is $\mathrm{K_{p}=K_{x}(RT)^{\Delta n}}$    .

Explanation:

When both forward and reverse reactions move at the same rate, a reversible reaction is said to be in chemical equilibrium. The equilibrium state is the point in a reversible reaction where the concentrations of the reactants and products remain constant over time.

• The equilibrium constant for a perfect gaseous mixture is Kp and Kx.
• When equilibrium concentrations are stated in atmospheric pressure, the equilibrium constant is Kp, and when they are expressed in molarity, the equilibrium constant is Kx.
• And the relation is given as,

$\mathrm{K_{p}=K_{x}(RT)^{\Delta n}}$               (1)

Where,

Kp=equilibrium constant at constant pressure

Kx=equilibrium constant in molarity

R=universal gas consatnt

T=temperature at which reaction is carried out

Δn = product - reactant in moles only for gas molecule types

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