For the following reaction, the equilibrium constant $\mathrm{K}_{\mathrm{c}}$ at 298 K is $1.6 \times 10^{17}$. $$ \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{S}^{2-}(\mathrm{aq}) \rightleftharpoons \mathrm{FeS}(\mathrm{~s}) $$ When equal volumes of $0.06 \mathrm{M} \mathrm{Fe}^{2+}(\mathrm{aq})$ and $0.2 \mathrm{M} \mathrm{S}^{2-}(\mathrm{aq})$ solutions are mixed, the equilibrium concentration of $\mathrm{Fe}^{2+}(\mathrm{aq})$ is found to be $\mathbf{Y} \times 10^{-17} \mathbf{M}$. The value of $\mathbf{Y}$ is $\_\_\_\_$