Question

Calculating an equilibrium constant from a partial equilibrium composition Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 500 ml flask with 2.9 atm of ammonia gas at 41. °C. He then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 3.9 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. x 5 ?

Answer 1

Ans- given Reaction 2NH3 = N2 + 3H₂ 2.9 initial pressure of NH3 = 2.9 atm a eguilibrium р-хих ан, г 3-9 dTM So, 2NH3 Ž N2 + 3H2 initial after 2.9-8 a 3n So, given 3 x= [PH2] 374= 3.9. 2=1-3 Now, Kp = [Na] [H2 33 - [PN Hz] 2 So, [PNH? = 2.9-1.3=1.6 [PN ] = 1.3 and [PH2] = 3.9 Now, som (1.6)2 Kp> (1967:19 [Kp= 30