Fe ⁺³(aq) + SCN ⁻¹(aq) ⇆ FeSCN ⁺²(aq) + heat

Question

Based on the reaction above, which way will the equilibrium shift if a solution of Fe(NO ₃) ₃ is added?
(1 point)
The reaction will shift to the right, favoring the forward reaction because the concentration of the
Fe ion was increased.
The reaction will shift to the left, favoring the reverse reaction because the concentration of the
Fe ion was decreased.
There will be no change visible change in the reaction because it is not a reversible reaction.
The reaction will continue at equilibrium because an ion that is present in the reaction is being
introduced.

Answer 1

The reaction provided is:

\[ \text{Fe}^{3+}(aq) + \text{SCN}^-(aq) \rightleftharpoons \text{FeSCN}^{2+}(aq) + \text{heat} \]

When a solution of Fe(NO₃)₃ is added, it increases the concentration of \(\text{Fe}^{3+}\) ions in the solution. According to Le Chatelier's principle, if the concentration of a reactant in a reversible reaction is increased, the equilibrium will shift to favor the forward reaction in order to consume the added reactant.

Therefore, in this case, the equilibrium will shift to the right, favoring the formation of \(\text{FeSCN}^{2+}\) and effectively "using up" some of the added \(\text{Fe}^{3+}\) ions.

So the correct answer is: The reaction will shift to the right, favoring the forward reaction because the concentration of the Fe ion was increased.