Consider the reaction between bromate ions and bromide ions in acidic aqueous solution as given by the

equation below:

$Br{O}_3^{-{?}_{(aq)}}+5B{r}_{(aq)}^{-}+6H_{(aq)}^{+}3B{r}_2(l)+3H_2{O}_{(l)}$

The results from four experiments to study the reaction are shown provided.

a$.$ Determine the rate law expression for this reaction.

b$.$ What is the overall reaction order?

c$.$ Calculate the value of $k$ at this temperature.

d$.$ Determine the rate of disappearance of $B{r}_{(aq)}$ in Experiment $2.$

e$.$ What is the initial rate of appearance of $B{r}_2$ at the following initial concentrations: $[Br{O}_3^{-}]=0\mathrm{.}045M,[B{r}^{-}]=$

$0\mathrm{.}22M$ and $[H^{+}]=0\mathrm{.}05M?$