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Calculate the rate of disappearance of \mathrm{Br}^{-} at the time when rate of appearance of \mathrm{Br}_2  during that time is 0.035 \mathrm{M} \mathrm{sec}^{-1}  in the given reaction:

\mathrm{5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+}\mathrm{6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{Cl)}\mathrm{6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{Cl}

Option: 1

\mathrm{0.025 \mathrm{Msec}^{-1}}


Option: 2

0.0583 \mathrm{Msec}^{-1}


Option: 3

\mathrm{0.075 \mathrm{Msec}^{-1}}


Option: 4

\mathrm{0.125 \mathrm{Msec}^{-1}}


Answers (1)

 Two rates are related as:

\mathrm{\begin{aligned} -\frac{1}{5} \frac{d\left[\mathrm{Br}^{-}\right]}{d t} & =\frac{1}{3} \frac{d\left[\mathrm{Br}_2\right]}{d t} \\ -\frac{d\left[\mathrm{Br}^{-}\right]}{d t} & =\frac{5}{3} \frac{d\left[\mathrm{Br} r_2\right]}{d t} \\ & =\frac{5}{3} \times 0.035 \\ & =0.0583 \mathrm{Msec}^{-1} \end{aligned}}

Posted by

Ramraj Saini

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