불균일 평형. C(s) + CO2(g) ⇌ 2CO(g) 4.5 atm Kp 1.52 partial

불균일 평형. C(s) + CO2(g) ⇌ 2CO(g) 4.5 atm Kp 1.52 partial

 

 

Consider the heterogeneous equilibrium process:

C(s) + CO2(g) ⇌ 2CO(g)

At 700℃, the total pressure of the system is found to be 4.50 atm.

If the equilibrium constant Kp is 1.52,

calculate the equilibrium partial pressures of CO2 and CO.

 

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평형에서,

> P_tot = P_CO2 + P_CO = 4.50 atm

> P_CO2 = 4.50 – P_CO

 

 

 

P_CO를 x라 두면,

Kp = (P_CO)^2 / P_CO2

= x^2 / (4.50 – x) = 1.52

 

x^2 = (4.50)(1.52) - 1.52x

x^2 + 1.52x - (4.50)(1.52) = 0

 

 

 

근의 공식으로 x를 계산하면,

( 참고 https://ywpop.tistory.com/3302 )

 

x = 1.96

 

 

 

따라서

P_CO = x = 1.96 atm

P_CO2 = 4.50 – x = 4.50 – 1.96 = 2.54 atm