The reaction rate for the reaction [{\PtCl}_{4}]^{2-}+{\H}_{2} {\O} ⇌ [{\Pt}({\H}_{2} {\O}) {\Cl}_{3}]^{-}+{\Cl}^{-} was measured as a function of concentrations of different species. It was observed that {-d[({\PtCl}_{4})^{2-}]}/{d t} =4.8 \times10^{-5}[({\PtCl}_{4})^{2-}]=2.4 \times10^{-3}[{{\Pt}({\H}_{2} {\O}) {\Cl}_{3}\}^{-}][{\Cl}^{-}] where, square brackets are used to denote molar concentrations. The equilibrium constant, \K_{c}=......... (Nearest integer) [26 Aug 2021 Shift 2]

Chemical Equilibrium

Section: Chemistry

Question : 54 of 114

Marks: +1, -0

The reaction rate for the reaction
[PtCl4]2−+H2O⇌[Pt(H2O)‌Cl3]−+Cl− was measured as a function of concentrations of different species. It was observed that

−d[(PtCl4)2−]

=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)

[26 Aug 2021 Shift 2]

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