Direction of Reversible Reactions Practice Test

A reversible reaction occurs in a sealed container at constant temperature:

$\mathrm{PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)}$

A concentration-versus-time plot shows that at the displayed time (before equilibrium), $\mathrm{PCl_5}$ is increasing while both $\mathrm{PCl_3}$ and $\mathrm{Cl_2}$ are decreasing. In which direction will the net reaction proceed to reach equilibrium?

A sealed container at constant temperature contains the reversible reaction

$\mathrm{Fe^{3+}(aq) + SCN^-(aq) \rightleftharpoons FeSCN^{2+}(aq)}$

At a moment before equilibrium is reached, the concentrations are:

In which direction will the net reaction proceed to reach equilibrium?