Question

In the following reaction, how is the rate of appearance of the product Bromine related to the rate of disappearance of the reactant Bromide?

$Br{O}_{3\left(aq\right)}^{⊝}+5B{r}_{\left(aq\right)}^{⊝}+6H_{\left(aq\right)}^{\oplus }\to 3B{r}_{2\left(l\right)}+3H_2{O}_{\left(l\right)}$

• A. $\frac{d}{dt}\left[B{r}_2\right]=\frac{-5}{3}\frac{d}{dt}\left[B{r}^{⊝}\right]$
• B. $\frac{d}{dt}\left[B{r}_2\right]=\frac{d}{dt}\left[B{r}^{⊝}\right]$
• C. $\frac{d}{dt}\left[B{r}_2\right]=\frac{-d}{dt}\left[B{r}^{⊝}\right]$
• D. $\frac{d}{dt}\left[B{r}_2\right]=\frac{-3}{5}\frac{d}{dt}\left[B{r}^{⊝}\right]$

Answer 1

The correct option is D

$\frac{d}{dt}\left[B{r}_2\right]=\frac{-3}{5}\frac{d}{dt}\left[B{r}^{⊝}\right]$

$\text{Rate}=\frac{-1}{5}\frac{d}{dt}\left[B{r}^{⊝}\right]=+\frac{1}{3}\frac{d}{dt}\left[B{r}_2\right]\frac{d}{dt}\left[B{r}_2\right]=\frac{-3}{5}\frac{d}{dt}\left[B{r}^{⊝}\right]$