Question

Consider the reaction N₂​+3H₂​⇌2NH₃​. The equilibrium constant (Kp​) for the above reaction is Kp​. If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by:

a) Kp​
b) 2Kp​
c) √Kp​​
d) 1​/Kp​

Answer 1

The equilibrium constant (Kp) for the dissociation of ammonia into nitrogen and hydrogen relates to the partial pressure of ammonia at equilibrium. For the reaction in question, the partial pressure of ammonia at equilibrium can be expressed in terms of the equilibrium constant as 1⁄Kp.

Step-by-step explanation:

The student's question concerns the dissociation of pure ammonia (NH3) into nitrogen and hydrogen gases and how the equilibrium constant (Kp) relates to the partial pressure of ammonia at equilibrium. For the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g), the equilibrium constant expression can be written as:

Kp = ⁄((PNH3)2) ⁄((PN2)(PH2)3)

When pure ammonia dissociates, the reaction starts with only NH3 and the products of N2 and H2 form. The equilibrium constant helps predict the extent of the reaction. Assuming the dissociation has reached equilibrium, we can express the partial pressure of ammonia at equilibrium in terms of Kp as (PNH3) = ⁄1⁄⁄Kp.