To answer your question accurately, it is essential to know the context of the reaction involving \( \text{Fe}(\text{SCN})^{2+} \) (iron(II) thiocyanate complex). Generally, the equilibrium involving this complex can be represented as follows:
\[ \text{Fe}^{2+} + \text{SCN}^- \rightleftharpoons \text{Fe}(\text{SCN})^{2+} \]
If you remove \( \text{Fe}(\text{SCN})^{2+} \), you are effectively reducing the concentration of the product in this equilibrium. According to Le Chatelier's principle, the system will respond to this change by shifting the equilibrium to the right to produce more \( \text{Fe}(\text{SCN})^{2+} \) in order to counteract the decrease caused by the removal.
Thus, the reaction will proceed in the forward direction to re-establish equilibrium.