Consider the reaction

$5B{r}^{-}(aq)+Br{O}_3^{-}(aq)+6H^{+}(aq)3B{r}_2(aq)+3H_{2}O(l)$

The average rate of consumption of $B{r}^{-}$is $1\mathrm{.}26{10}^{-4}\frac{M}{s}$ over the first two minutes. What is the average rate of formation of

$B{r}_2$ during the same time interval?

Rate of formation of $B{r}_2=$