The reaction rate for the reaction [ PtCl_4]^2-+ H_2 O ⇌[ Pt ( H_2 O ) Cl_3]^-+ Cl^- was measured as a function of concentrations of different…

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 $\displaystyle \mathrm{K}_{\mathrm{c}}=$ \_\_\_\_. (Nearest integer)