The rate of reversible reaction (change in concentration per second):
`PrCl_(4)^(2-)+H_(2)OhArrPt(H_(2)O)Cl_(3)^(-)+Cl^(-)`,
was observed at `0.3 ionic` strength at `25^(@)C` and noticed that
`(Delta[PtCl_(4)^(2-)])/(Delta t)=3.9xx10^(-5)[PtCl_(4)^(2-)]-2.1xx10^(-3)[Pt(H_(2)O)Cl_(3)^(-)][Cl^(-)]`
Calculate: (`a`) Rate constant for forward and backward reaction.
(`b`) The equilibrium constant for the complexation of fourth `Cl^(-)` at `0.3 ionic` strength.

Explanation

(`a`) Rate constant for forward reaction
`K_(f)=3.9xx10^(-5)sec^(-1)`
Rate constant for backward reaction
`K_(b)=2.1xx10^(-3)litremol^(-1)sec^(-1)`
(`b`) Equilibrium constant for the complexation of fourth `Cl^(-)` is equilibrium constant for backward reaction i.e.,
`K_(c)=(K_(b))/(K_(f))=(2.1xx10^(-3))/(3.9xx10^(-5))=53.85 litre mol^(-1)`