Question Bank › Inorganic Chemistry › Coordination Chemistry › ABC26IN1093ABC26IN1093 · Coordination Chemistry Subject: Inorganic Chemistry · Chapter: Coordination Chemistry · Topic: Reaction Mechanisms Substitution · Exam: NET DEC 2016 · Marks: 2 · Difficulty: Medium
In the following redox reaction with an equilibrium constant $\mathrm{K}=2.0 \times 10^{8}$ \[ \left[\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}+\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}_{6}\right)\right]^{3+} \rightarrow\left[\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}+\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \]
the self exchange rates for oxidant and reductant are $5.0\ \mathrm{M}^{-1}\mathrm{s}^{-1}$ and $4.0 \times 10^{3}\ \mathrm{M}^{-1}\mathrm{s}^{-1}$ respectively. The approximate rate constant $\left(\mathrm{M}^{-1} \mathrm{s}^{-1}\right)$ for the reaction is (a) $3.16 \times 10^{6}$
(b) $2.0 \times 10^{6}$
(c) $6.32 \times 10^{6}$
(d) $3.16 \times 10^{6}$
Answer Explanation No explanation was printed for this question.
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