Reaction Quotient and Le Chatelier's Principle Practice Test

In a sealed flask at constant temperature, the equilibrium $\mathrm{2NO(g) + O_2(g) \rightleftharpoons 2NO_2(g)}$ has $K_p = 6.0\times10^1$. The system is initially at equilibrium. A small amount of $\mathrm{O_2(g)}$ is removed, and immediately afterward $Q_p$ is found to be $9.0\times10^1$. As equilibrium is reestablished, what shift occurs?

A sealed rigid container at constant temperature contains the system at equilibrium: $$\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g)$$ with $K_c = 0.50$. At equilibrium, the concentrations are $\text{N}_2\text{O}_4=0.40,\text{M}$ and $\text{NO}_2=0.45,\text{M}$. A small amount of $\text{NO}_2(g)$ is suddenly removed so that immediately after the stress $\text{NO}_2=0.30,\text{M}$ while $\text{N}_2\text{O}_4$ is unchanged at that instant. Based on comparing $Q_c$ to $K_c$, how will the system respond to reestablish equilibrium?