# Problem: Calculate the pressures of NO, Cl 2, and NOCl in an equilibrium mixture produced by the reaction of a starting mixture with 4.0 atm NO and 2.0 atm Cl2. (Hint: KP is small; assume the reverse reaction goes to completion then comes back to equilibrium.)2NO(g) + Cl2(g) ⇌ 2NOCl(g)             K P = 2.5 × 10-3

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###### FREE Expert Solution

2 NO(g) + Cl2(g)  2 NOCl(g)

When dealing with equilibrium and Kp:

Kp → equilibrium units in terms of pressure
Kp is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}{\mathbf{=}}\frac{{{\mathbf{P}}_{\mathbf{NOCl}}}^{\mathbf{2}}}{{{\mathbf{P}}_{\mathbf{NO}}}^{\mathbf{2}}\mathbf{×}{\mathbf{P}}_{{\mathbf{Cl}}_{\mathbf{2}}}}}$

ICE Chart:

###### Problem Details

Calculate the pressures of NO, Cl 2, and NOCl in an equilibrium mixture produced by the reaction of a starting mixture with 4.0 atm NO and 2.0 atm Cl2. (Hint: KP is small; assume the reverse reaction goes to completion then comes back to equilibrium.)
2NO(g) + Cl2(g) ⇌ 2NOCl(g)             K P = 2.5 × 10-3

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Based on our data, we think this problem is relevant for Professor Sharpe Elles' class at KU.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.