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