For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35...

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For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35...

For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35 x 10^4.

Hydrogen at a partial pressure of 0.700 bar and chlorine at a partial pressure of 0.500 bar are placed in a vessel at 800oC and allowed to equilibrate. Find the final partial pressures of all three gases in this reaction in bar

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Answer 1

Answer #1

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------H₂(g) + Cl₂(g) 2 HCl(g)

I ----- 0.7 ---- 0.5 -------------- 0

C----- -x ----------- -x ----------------- +2x

E --- 0.7-x ------ 0.5-x ------------ 2x

Kp = P^2HCl/PH2*PCl2

4.35*10^4 = (2x)^2/(0.7-x)(0.5-x)

4.35*10^4(0.7-x)(0.5-x) = 4x^2

x = 0.499

PH2 = 0.7-x =0.7- 0.499 = 0.201bar

PCl2 =0.5-x =0.5- 0.499 = 0.001bar

PHCl = 2x = 2*0.499 bar = 0.998bar

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Answer 2

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For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35...

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