The reaction rate for the reaction| $$ \left[\mathrm{PtCl}_4\right]^{2-}+\mathrm{H}_2 \mathrm{O} \rightleftharpoons\left[\mathrm{Pt}\left(\mathrm{H}_2 \mathrm{O}\right) \mathrm{Cl}_3\right]^{-}+\mathrm{Cl}^{-} $$ was measured as a function of concentrations of different species. It was observed that $$ \frac{-\mathrm{d}\left[\left[\mathrm{PtCl}_4\right]^{2-}\right]}{\mathrm{dt}}=4.8 \times 10^{-5}\left[\left[\mathrm{PtCl}_4\right]^{2-}\right]-2.4 \times 10^{-3}\left[\left[\mathrm{Pt}\left(\mathrm{H}_2 \mathrm{O}\right) \mathrm{Cl}_3\right]^{-}\right]\left[\mathrm{Cl}^{-}\right] . $$ where square brackets are used to denote molar concentrations. The equilibrium constant $\mathrm{K}_{\mathrm{c}}=$ $\_\_\_\_$ . (Nearest integer)