Calculate the partial pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced when a sample of NOCl with initial pressure of 5.00 atm comes to equilibrium according to the following reaction. (Hint: use the repeated approximation method to obtain a better answer.) 2NOCl(g) ⇌ 2NO(g)+ Cl2(g); Kp= 4.0 x 10–4

Chemistry: The Molecular Science
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Author:John W. Moore, Conrad L. Stanitski
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Chapter12: Chemical Equilibrium
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Calculate the partial pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced when a sample of NOCl with initial pressure of 5.00 atm comes to equilibrium according to the following reaction. (Hint: use the repeated approximation method to obtain a better answer.)

2NOCl(g) ⇌ 2NO(g)+ Cl2(g); Kp= 4.0 x 10–4

Expert Solution
Step 1

Given,

Kp = 4.0 x 10-4

Initial pressure = 5.00 atm

Kp = equilibrium constant

The reaction is;

2NOCl (g) 2NO (g) + Cl2 (g)    ....(1)

 

 

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