Respuesta :
Answer: 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:
[tex]N_2(g)+2O_2(g)\rightleftharpoons 2NO_2(g)[/tex]
Initial: 0.81 0.20
At eqllm: 0.81-x 0.20-2x 2x
The expression of [tex]K_p[/tex] for above equation follows:
[tex]K_p=\frac{(p_{NO_2})^2}{(p_{O_2})^2\times p_{N_2}}[/tex]
We are given:
[tex]K_p=0.050[/tex]
Putting values in above equation, we get:
[tex]0.050=\frac{(2x)^2}{(0.20-2x)^2\times (0.81-x)}\\\\x=-18.98,-0.0256,0.0166[/tex]
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.
