We’re being asked to determine the pressure of NO2(g) at equilibrium for the following reaction:
2 NO2(g) ⇌ 2 NO(g) + O2(g) Kp = 158
Recall that the equilibrium constant is the ratio of the products and reactants.
We use Kp when dealing with pressure and Kc when dealing with concentration:
Note that solid and liquid compounds are ignored in the equilibrium expression.
A sample of pure NO2 gas heated to 1000 K decomposes:
2NO2(g) ⇌ 2NOg) + O2(g) Kp = 158
Analysis shows that the partial pressure of O2 is 0.25 atm at equilibrium. Calculate the pressure of NO2(g) at equilibrium.
A. 0.090 atm
B. 0.015 atm
C. 0.020 atm
D. 0.038 atm
E. 0.075 atm
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