The reaction rate for the reaction
`[PtCl_4]^(2-) + H_2O = [Pt(H_2O)Cl_3]^(-) + Cl^-`
was measured as a function of conccntrations of different species. It was observed that
`(-d[[PtCl_4]^(2-)])/dt = 4.8 xx 10^(-5) [[PtCl_4]^(2-)] -2.4 xx 10^(-3) [[Pt(H_2O)Cl_3]^-][Cl^-]`
where square brackets arc used to denote molar concentrations. The equilibrium constant `K_c` = ___________. (Nearest integer)

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.

The approach to the following equilibrium was observed kinetically from both directions Pt Cl_(4)^(2-) +H_(2)O hArr Pt (H_(2)O) Cl_(3)^(-) +Cl^(-) "at " 25^(@)C . It was found that - (d[PtCl_(4)^(2-)])/(dt) = (3.9 xx10^(-5)) [Pt Cl_(4)^(2-)] - (2.1 xx10^(-3)) [ Pt (H_(2)O) Cl_(3)^(-) ] [Cl^(-)] Calculate the equilibrium constant for the complexation of the fourth Cl^(-) by Pt(II) .

The approach to the following equilibrium was observed kinetically form both directions: [PtCl_(4)]^(2-) +H_(2)O hArr [Pt(H_(2)O)Cl_(3)]^(ɵ)+Cl^(ɵ) At 25^(@)C it was found that at 0.3 inoic strength - (Delta [PtCl_(4)]^(2-))/(Delta t) = (3.9 xx 10^(-5)s^(-1))[PtCl_(4)]^(2-) - (2.1 xx 10^(-3) L mol^(-1) s^(-1))[Pt(H_(2)O)Cl_(3)]^(ɵ)[Cl_(3)^(ɵ)] What is the value of k for the complexation of the fourth Cl^(ɵ) by Pt(II) at 0.3 ionic strenght.

The approach to the following equilibrium was observed kinetically from both directions : PtCl_(4)^(2-) + H_(2)O ? [Pt(H_(2)O)Cl_(3)^(-)]+Cl^(-)" at "25^(@)C , it was found that -(Delta)/(Delta t) [PtCl_(4)^(2-)]=[3.9xx10^(-5)" sec"^(-1)] [PtCl_(4)^(2-)]-[2.1xx10^(-3)" L. mol"^(-1)" sec"^(-1)]xx[Pt(H_(2)O)Cl_(3)]^(-)[Cl^(-)] What is the value of equilibrium constant for the complexation of the fourth Cl^(–) by Pt(II) ?

For the following question , enter the correct numerical value, ( in decimal - notation , truncated / rounded - off to the second decimal place , e.g., 6*25, 7*00 -0*33, 30*27, -127*30) using the mouse and the onscreen virtual nemeric keypad in the place designed to enter the answer. The approach of the following equilibrium was observed kinetically from both direction : PtCl_(4)^(2-) + H_(2)O hArr Pt (H_(2)O) hArr Pt (H_(2)O) Cl_(3)^(-) + Cl^(-) At 25^(@)C , it was found that (d[PtCl_(4)^(-)])/dt=(3*90 xx10^(-5)s^(-1) ) [PtCl_(4)^(2-)] - (2*1 xx 10^(-3) mol^(-1)s^(-1)) [Pt(H_(2)O ) Cl_(3)^(-)] The value of the equilibrium constant when fourth Cl^(-) ion is complexed , i.e., for the step involving backward reaction will be ......... .

In the reaction HCl + H_(2)O to H_(3)^(+)O +Cl^(-)

In the reaction :Cl_(2)+OH^(-)rarrCl^(-)+ClO_(4)^(-)+H_(2)O :-