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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.

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Answer:

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.

User Omid Roshani
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