For a concentrated solution of a weak electrolyte ($$\mathrm{K}_{\text {eq }}=$$ equilibrium constant) $$\mathrm{A}_{2} \mathrm{B}_{3}$$ of concentration '$$c$$', the degree of dissociation '$$\alpha$$' is :

The equilibrium constant for the reversible reaction

2A(g) $$\rightleftharpoons$$ 2B(g) + C(g) is K_{1}

$${3 \over 2}$$A(g) $$\rightleftharpoons$$ $${3 \over 2}$$B(g) + $${3 \over 4}$$C(g) is K_{2}.

K_{1} and K_{2} are related as :

4.0 moles of argon and 5.0 moles of PCl_{5} are introduced into an evacuated flask of 100 litre capacity at 610 K. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be 6.0 atm. The K_{p} for the reaction is :

[Given : R = 0.082 L atm K^{$$-$$1} mol^{$$-$$1}]

For a reaction at equilibrium

A(g) $$\rightleftharpoons$$ B(g) + $${1 \over 2}$$ C(g)

the relation between dissociation constant (K), degree of dissociation ($$\alpha$$) and equilibrium pressure (p) is given by :