Question

Ammonium Iodide dissociates reversibly to ammonia and hydrogen iodide:

NH4I(s) ⇋ NH3(g) + HI(g)Kp = 0.215 at 400°C
Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.
A.0.103 atm
B.0.215 atm
C.0.232 atm
D.0.464 atm
E.2.00 atm

Answer 1

To calculate the partial pressure of ammonia at equilibrium, multiply the equilibrium constant (Kp) by the initial pressure of ammonium iodide.

Step-by-step explanation:

To calculate the partial pressure of ammonia at equilibrium, we can use the equilibrium constant expression and the given value of Kp. The equilibrium constant expression for this reaction is Kp = [NH3] / [NH4I]. Since we are given the value of Kp as 0.215, we can rearrange the equation to find the partial pressure of ammonia, [NH3] = Kp * [NH4I]. Given a sufficient quantity of ammonium iodide, we can assume that the initial pressure of ammonia is 0. Therefore, the partial pressure of ammonia at equilibrium is 0.215 atm, which corresponds to option B.