Model: Kinetics of a Unimolecular Reaction

Under certain conditions ozone in the atmosphere decomposes by dissociation $(O_3{O}_2+O)$ with the

kinetics given below. The data in the graph $($fig$.1)$ and in table $1$ are described by the three equations below.

Equations that describe the decomposition of ozone, $O_3$ :

Equation $1.$ reaction rate $=-\frac{O_3}{}t$

Equation $2.$ rate law: Rate$=\frac{O_3}{}t=-k[O_3]$

Equation $3.$ integrated rate law: $Ln(\frac{O_3}{[O_3{]}_0})=-kt,$ Where: $[O_3{]}_o=$ conc. of $O_3$@$t=0$

Use figure $1$ to determine how long it takes for half the ozone to decompose. What is the concentration of

ozone after that time?

Use figure $1$ to determine initial reaction rate of the ozone decomposition. Provide both the magnitude

and the units.

Use figure $1$ to determine the approximate rate of the reaction after $1\mathrm{.}92$ hours have passed.

Referring to figure $1,$ how does the rate of the reaction change with time? Why does the rate change with

time?

The reaction is

order of the reaction with respect to ozone.

Overall, the decomposition of ozone reaction i

If the concentration of ozone were doubled, the reaction rate would

What parameter in the integrated rate law determines the slope of the straight line in the graph?

Table $1.$ Data on Ozone Decomposition $($half$-$life time $=1270s)$