Question

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 500. ML flask with 3.0 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.90 atm . Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

Answer 1

12. is the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture.

Step-by-step explanation:

`2NH_3(g)\rightleftharpoons N_2(g)+3H_2(g)`

initially

3.0 atm 0 0

At equilibrium

(3.0-2p) p 3p

Equilibrium partial pressure of nitrogen gas = p = 0.90 atm

The expression of a pressure equilibrium constant will be given by :

`K_p=(p_(N_2)* (p_(H_2))^3)/((p_(NH_3))^2)`

`K_p=(p* (3p)^3)/((3.0-2p)^2)`

`=(0.90 atm* (3* 0.90 atm)^3)/((3.0-2* 0.90 atm)^2)`

`K_p=12.30\approx 12.`

12. is the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture.