The reaction rate for the reaction\ $\left[\mathrm{PtCl}_{4} ight]^{2-}+\mathrm{H}_{2} \mathrm{O}

Question

The reaction rate for the reaction\ $\left[\mathrm{PtCl}_{4}ight]^{2-}+\mathrm{H}_{2} \mathrm{O} ightleftharpoons\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}ight) \mathrm{Cl}_{3}ight]^{-}+\mathrm{Cl}^{-}$\ was measured as a function of concentrations of different species. It was observed that $$ \begin{aligned} \frac{-d\left[\left[\mathrm{PtCl}_{4}ight]^{2-}ight]}{d t}= & 4.8 	imes 10^{-5}\left[\left[\mathrm{PtCl}_{4}ight]^{2-}ight] \ & -2.4 	imes 10^{-3}\left[\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}ight) \mathrm{Cl}_{3}ight]^{-}ight]\left[\mathrm{Cl}^{-}ight] \end{aligned} $$ where square brackets are used to denote molar concentrations. The equilibrium constant $K_{c}=$ _______. (Nearest integer)\

Professor PC Thomas Classes · Answer

(0) :\ $K_{c}=\frac{K_{f}}{K_{b}}=\frac{4.8 	imes 10^{-5}}{2.4 	imes 10^{-3}}=2 	imes 10^{-2} \approx 0.02 \approx 0$\