Consider the gaseous equilibrium 2 AB _ 2(g) 2 AB _ (g) + B _ 2(g) The expression relating the degree of dissociation ( ) and equilibrium constant ( K_p ) and total pressure P is:

Step-by-step solution

The given reaction is 2 AB _ 2(g) 2 AB _ (g) + B _ 2(g) Let the initial moles of AB ₂ be 2 . Moles at equilibrium: AB ₂ = 2(1- ) AB = 2 B ₂ = Total moles at equilibrium = 2(1- ) + 2 + = 2 + Partial pressures at equilibrium: P_ AB ₂ = 2(1- ) 2+ P P_ AB = 2 2+ P P_ B ₂ = 2+ P The equilibrium constant K_p is given by: K_p = (P_ AB )^2 P_ B ₂ (P_ AB ₂ )^2 Substituting the partial pressures: K_p = ( 2 2+ P )^2 ( 2+ P ) ( 2(1- ) 2+ P )^2 K_p = 4 ^2 P^2 (2+ )^2 P 2+ (2+ )^2 4(1- )^2 P^2 K_p = ^3 P (2+ )(1- )^2 Assuming is