The reaction rate for the reaction [ PtCl _ 4 ] ^ 2 - + H _ 2 O ⇌...

The reaction rate for the reaction

${\left[{PtCl}_{4}\right]}^{2 -} + {H}_{2}O ⇌ {\left[Pt\left({H}_{2}O\right){Cl}_{3}\right]}^{-} + {Cl}^{-}$

was measured as a function of concentrations of different species. It was observed that

$\dfrac{- d\left[{\left[{PtCl}_{4}\right]}^{2 -}\right]}{dt} = 4 . 8 \times {10}^{- 5}\left[{\left[{PtCl}_{4}\right]}^{2 -}\right] - 2 . 4 \times {10}^{- 3}\left[{\left[Pt\left({H}_{2}O\right){Cl}_{3}\right]}^{-}\right]\left[{Cl}^{-}\right]$

where square brackets are used to denote molar concentrations. The equilibrium constant

${K}_{c} = X$(Nearest integer)

Value of $\dfrac{1}{X}is$ (question is modified.)