Textbook Problem

At a certain temperature, nitrogen and oxygen gases combine to form nitrogen oxide gas.

${\text{N}}_2\left(g\right)+{\text{O}}_2\left(g\right)\rightleftharpoons 2\text{NO}\left(g\right)$When equilibrium is established, the partial pressures of the gases are: $P_{{\text{N}}_2}=1.200\text{atm},P_{{\text{O}}_2}=0.800\text{atm},P_{\text{NO}}=0.0220\text{atm}$.

(a) Calculate K at the temperature of the reaction.

(b) After equilibrium is reached, more oxygen is added to make its partial pressure 1.200 atm. Calculate the partial pressure of all gases when equilibrium is reestablished.