The reaction rate for the reaction \[ \left[\mathrm{PtCl}_{4}\right]^{2-}+\mathrm{H}_{2} \mathrm...
0The 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 function of concentrations of different species. It was observed that
\[
\begin{array}{l}
\frac{-\mathrm{d}\left[\mathrm{PtCl}_{4}\right]^{2-}}{\mathrm{dt}}=4.8 \times 10^{-5}\left[\mathrm{PtCl}_{4}\right]^{2-} \\
\left.=-2.4 \times 10^{-3}\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}_{3}\right]^{-}\right]\left[\mathrm{Cl}^{-}\right]
\end{array}
\]
where square brackets are used to denote molar concentrations. The equilibrium constant
\[
\mathrm{K}_{\mathrm{c}}=
\]
. (Nearest integer)
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