The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in…
Chemistry · NEET · NTA Exams — Chemical Kinetics
The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acidic solution is \(\mathrm{ZBr}^{-}+\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{ZH}^{+} \longrightarrow \mathrm{Br}_{2}+\mathrm{ZH}_{2} \mathrm{O}\)
\(r=k\left[H_{2} \mathrm{O}_{2}\right]\left[\mathrm{H}^{+}\right]\left[\mathrm{Br}^{-}\right]\)
If, by the addition of water, the total volume were doubled, what would be the effect on the rate of disappearance of Br- and rate of reaction?
- Rate of disappearance of Br- becomes 1/8 times and rate of reaction 1/4 times.
- Rate of disappearance of Br- becomes 1/4 times and rate of reaction 1/8 times.
- Both rate of disappearance of Br- and rate of reaction becomes 1/8 times.
- Rate of disappearance of Br- becomes 4 times and rate of reaction 8 times.
Answer
(C) Both rate of disappearance of Br - and rate of reaction becomes 1/8 times.
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