In a chamber filled with air (look up the partial pressures of nitrogen and oxygen gases) at 2200 °C, the reaction that generates nitrogen monoxide from nitrogen gas and oxygen gas has a Kp = 0.050. What are the equilibrium partial pressures of the three gases in the above reaction?

The equilibrium partial pressure of nitrogen gas, oxygen gas and nitrogen dioxide are 0.7934 atm, 0.1668 atm and 0.0332 atm respectively.

Explanation:

We know that:

Partial pressure of nitrogen gas at 2200°C = 0.81 atm

Partial pressure of oxygen gas at 2200°C = 0.20 atm

The chemical equation for the formation of nitrogen dioxide follows:

Initial:              0.81       0.20

At eqllm:        0.81-x    0.20-2x           2x

The expression of for above equation follows:

We are given:

Putting values in above equation, we get:

Neglecting the negative value of 'x' because partial pressure cannot be negative

So, equilibrium partial pressure of nitrogen dioxide = 2x = 2(0.0166) = 0.0332 atm

Equilibrium partial pressure of nitrogen gas = (0.81 - x) = (0.81 - 0.0166) = 0.7934 atm

Equilibrium partial pressure of oxygen gas = (0.20 - 2x) = [0.20 - 2(0.0166)] = 0.1668 atm

Hence, the equilibrium partial pressure of nitrogen gas, oxygen gas and nitrogen dioxide are 0.7934 atm, 0.1668 atm and 0.0332 atm respectively.

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