In the reaction ${B r O}_{3 (a q)}^{-} + {5 B r}_{(a q)}^{-} + 6 H^{+} \overset{}{\to} 3 {B r}_{2 (l)} + 3 H_{2} O_{(l)}$
The rate of appearance of $B r_{2}$ is related to rate of disappearance of bromide ions as following

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$\frac{d [B r_{2}]}{d t} = \frac{3}{5} \frac{d [{B r}^{-}]}{d t}$

$\frac{d [B r_{2}]}{d t} = - \frac{3}{5} \frac{d [B r^{-}]}{d t}$

$\frac{d [B r_{2}]}{d t} = - \frac{5}{3} \frac{d [{B r}^{-}]}{d t}$

$\frac{d [{B r}_{2}]}{d t} = \frac{5}{3} \frac{d [{B r}^{-}]}{d t}$

answer is B.

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Detailed Solution

$Rate = - \frac{1}{5} \frac{d [{Br}^{-}]}{d t} = + \frac{1}{3} \frac{d [{Br}_{2}]}{d t}$

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