Reaction Quotient and Le Chatelier's Principle Practice Test

A mixture of gases in a rigid container is at equilibrium for the reaction $$\mathrm{H_2(g) + I_2(g) \rightleftharpoons 2HI(g)}$$. At this temperature, $K_c = 50$. Some $\mathrm{HI(g)}$ is removed, and immediately afterward $Q_c = 8$. As the system returns to equilibrium, what net shift will occur?

In a closed flask at constant temperature, the system is initially at equilibrium for $$\mathrm{CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g)}$$. At this temperature, $K_c = 1.6$. A small amount of $\mathrm{CO_2(g)}$ is added, and immediately after the addition the reaction quotient is $Q_c = 4.0$. Which shift will occur as equilibrium is reestablished?