Chemical Kinetics - Result Question 16
####16. In the following reaction, how is the rate of appearance of the underlined product related to the rate of disappearance of the underlined reactant?
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$BrO_3^{-}(aq)+\underline{5 Br^{-}}(aq)+6 H^{+}(aq)$
$\longrightarrow 3 Br_2(l)+3 H_2 O(l)$
(a) $\frac{d[Br_2]}{d t}=-\frac{5}{3} \frac{d[Br^{-}]}{d t}$
(b) $\frac{d[Br_2]}{d t}=-\frac{d[Br^{-}]}{d t}$
(c) $\frac{d[Br_2]}{d t}=\frac{3}{5} \frac{d[Br^{-}]}{d t}$
(d) $\frac{d[Br_2]}{d t}=-\frac{3}{5} \frac{d[Br^{-}]}{d t}$
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Solution:
- (d) Rate of reaction
$ \begin{aligned} & -\frac{1}{5} \frac{d[Br^{-}]}{d t}=+\frac{1}{3} \frac{d[Br_2]}{d t} \\ & \frac{d[Br_2]}{d t}=-\frac{3}{5} \frac{d[Br^{-}]}{d t} \end{aligned} $
