The reaction rate for the reaction[PtCl4]2- + H2O → [Pt(H2O)Cl3]- was measured as a function of concentrations of different species. It was observed that -dtPtCl42-dt= 4.8 × 10-5 [[PtCl4 ]2-] – 2.4 × 10-3 [[Pt(H2O)Cl3]-][Cl-] where square brackets are used to denote molar concentrations. The equilibrium constant Kc = (Nearest integer)

Keq = KfKb=4.8×10-52.4×10-3=Hence, the answer is 0.02.

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The reaction rate for the reaction
${[P t C l_{4}]}^{2 -} + H_{2} O \to {[P t (H_{2} O) C l_{3}]}^{-}$
was measured as a function of concentrations of different species. It was observed that $\frac{- d t {[P t C l_{4}]}^{2 -}}{d t} = 4.8 \times 10^{- 5} [{[P t C l_{4}]}^{2 -}] - 2.4 \times 10^{- 3} [{[P t (H_{2} O) C l_{3}]}^{-}] [C l^{-}]$ where square brackets are used to denote molar concentrations. The equilibrium constant Kc = (Nearest integer)

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answer is 0.02.

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$K_{e q} = \frac{K_{f}}{K_{b}} = \frac{4.8 \times 10^{- 5}}{2.4 \times 10^{- 3}} =$

Hence, the answer is 0.02.

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