A reaction, A(g) + 2B(g) ⇌ 2C(g) + D(g), was studied using an initial concentration of B which was 1.5 times that of A. However, the equilibrium concentrations of A and B were found to be equal. The v

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A reaction, A(g) + 2B(g) ⇌ 2C(g) + D(g), was studied using an initial concentration of B which was 1.5 times that of A. However, the equilibrium concentrations of A and B were found to be equal. The value of K p ​ for the equilibrium is:

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A ( g ) + 2 B ( g ) ⇌ 2 C ( g ) + D ( g ) Initial conc. x 1.5 x 0 0 At equilibrium x − y 1.5 x − 2 y 2 y y Given: x − y = 1.5 x − 2 y ; y = 0.5 x . Thus, at equilibrium [ A ] = 0.5 x [ B ] = 0.5 x [ C ] = x [ D ] = 0.5 x ∴ K c ​ = K p ​ = ( 0.5 x ) ( 0.5 x ) 2 ( x 2 ) ( 0.5 x ) ​ = 4.

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