500℃ N2(g) + 3H2(g) ⇌ 2NH3(g) Kp = 1.45×10^(-5)

0.432 atm N2 and 0.928 atm H2

For the Haber process, N2(g) + 3H2(g) ⇌ 2NH3(g),

Kp = 1.45×10^(-5) at 500℃.

In an eqm mixture of the three gases at 500℃,

the partial pressure of H2 is 0.928 atm

and that of N2 is 0.432 atm.

What is the partial pressure(atm) of NH3

in this eqm mixture?

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N2(g) + 3H2(g) ⇌ 2NH3(g)

Kp = (P_NH3)^2 / ((P_N2) (P_H2)^3)

( 참고 https://ywpop.tistory.com/7136 )

(P_NH3)^2 = [Kp × ((P_N2) (P_H2)^3)]

P_NH3 = [Kp × ((P_N2) (P_H2)^3)]^(1/2)

= [(1.45×10^(-5)) × ((0.432) (0.928)^3)]^(1/2)

= 0.00224 atm

= 2.24×10^(-3) atm

답: 2.24×10^(-3) atm

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500℃ N2(g) + 3H2(g) ⇌ 2NH3(g) Kp = 1.45×10^(-5)

평형 혼합물에서 43.77 bar N2 and 94.03 bar H2 이다.

NH3의 부분 압력은 얼마인가?

P_NH3 = [Kp × ((P_N2) (P_H2)^3)]^(1/2)

= [(1.45×10^(-5)) × ((43.77) (94.03)^3)]^(1/2)

= 22.97 bar

답: 22.97 bar

[키워드] N2(g) + 3H2(g) ⇌ 2NH3(g) 평형 기준