Infer shifts in equilibrium reactions using equilibrium constants (Kc) and reaction quotients (Q).

For the reaction: $\mathrm{N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)}$, the equilibrium constant is $K_c = 0.50 \text{ mol}^{-2}\text{dm}^6$ at 450 K. At a given moment, the reaction quotient is calculated as $Q = 0.15 \text{ mol}^{-2}\text{dm}^6$. In which direction will the reaction shift to reach equilibrium?

For the reaction $$\ce{N2O4(g) <=> 2NO2(g)}$$ at 298 K, $$K_c = 0.142$$. At a particular moment, the concentrations are $$[\ce{N2O4}] = 0.080 \text{ mol L}^{-1}$$ and $$[\ce{NO2}] = 0.025 \text{ mol L}^{-1}$$. Determine whether the reaction will shift to the left or to the right to reach equilibrium, and explain your reasoning.

The system $$\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)$$ has $$K_c = 0.50$$ at a particular temperature. At a given moment, the reaction quotient $$Q = 0.20$$. Which statement correctly describes how the equilibrium will shift?