Learning Goal:

To calculate average and relative reaction rates.

You can measure the rate of a reaction, just like

you can measure the speed a jogger runs. While a

jogger would be reported to run a specific number

of miles in an hour, miles$/$hour$,$ a reaction is

reported to form product or consume reagent in

molar concentration per second, $\frac{M}{s}.$

Reaction rate can be defined either as the increase

in the concentration of a product per unit time or as

the decrease of the concentration of a reactant per

unit time. By definition, reaction rate is a positive

quantity.

In the reaction $x2Y,$ for example, $Y$ is being

produced twice as fast as $x$ is consumed and thus

rate $ofx=\frac{1}{2}($ rate $ofY)$

Each rate can be expressed as the change in

concentration over the change in time, $t$ :

$\frac{-[x]}{t}=\frac{1}{2}(\frac{[Y]}{t})$

Rate of decomposition of $H_{3}P{O}_4=4\mathrm{.}00{10}^{-4}\frac{M}{s}$

Previous Answers

Correct

For every two moles of $H_{3}P{O}_4$ that disappear, only one mole of $P_2{O}_5$ is formed. The rate of

decomposition of $H_{3}P{O}_4$ is twice the rate of formation of $P_2{O}_5.$

Part C

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 $1\mathrm{.}66{10}^{-4}\frac{M}{s}$ over the first two minutes. What is the average

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

Express your answer with the appropriate units.

View Available Hint$($s$)$

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

M