Question

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

Answer 1

Kp = 2.2 x 10-2

Step-by-step explanation:

The equation for the decomposition of NH3 is as follows:

2NH3(g) <-------------> N2(g) + 3H2(g)

Initially only NH3 present

PNH3 = 2.3 atm

at equilibroum

PH2 = 3 x PN2 = 0.69 atm;

Therefore;

PN2 = 0.69 atm/3

= 0.23 aatm

PNH3 = 2.3 - 2(0.23) = 1.84 atm

Kp = (PN2) (PH2)3 / (PNH3)2

Kp = (0.23) (0.69)3 / (1.84)2

Kp = (0.23) (0.33) / (3.39)

Kp = 0.6912 / 1.44

Kp = 0.0224

Kp = 2.2 x 10-2