Consider the following chemical equilibrium of the gas phase reaction at a constant temperature : A(g) B(g) + C(g) If p being the total pressure, Kp is the pressure equilibrium constant and is the deg

Question

Consider the following chemical equilibrium of the gas phase reaction at a constant temperature : A(g) B(g) + C(g) If p being the total pressure, Kp is the pressure equilibrium constant and is the degree of dissociation, then which of the following is true at equilibrium ?

(A) When p increases increases
(B) When p increases decreases
(C) If p value is extremely high compared to Kp, 1
(D) If Kp value is extremely high compared to p, becomes much less than unity

Prashant Kotian · Accepted Answer

Correct answer: B. A(g) B(g) + C(g) Kp = 2 p    On increase in pressure,  decreases. (According to LCP towards lesser number of gaseous moles as well as to keep Kp constant)

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