The reaction of $N{O}_2$ with ozone produces $N{O}_3$ in a second order over all reaction. $N{O}_2(g)+O_3(g)N{O}_3(g)+O_2(g)$

a$.$ Write the rate law for the reaction if the reaction is first order in each reactant.

b$.$ The rate constant for the reaction is $1\mathrm{.}93{10}^4{M}^{-1}{s}^{-1}$ at $298K.$ What is the rate of reaction when $[N{O}_2]=$

$1\mathrm{.}8{10}^{-8}M$ and $[O_3]=1\mathrm{.}4{10}^{-7}M?$

c$.$ What is the rate of formation of $N{O}_3$ under these conditions?

d$.$ What happens to the rate of the reaction if the concentration of $O_3$ is doubled?The reaction of NO$2$ with ozone produces NO$3$ in a second order over all reaction. NO$2($g$)+$ O$3($g$)$ NO$3($g$)+$ O$2($g$)$

a$.$ Write the rate law for the reaction if the reaction is first order in each reactant.

b$.$ The rate constant for the reaction is $1\mathrm{.}93$x$104$ M$-1$ s$-1$ at $298$K$.$ What is the rate of reaction when $[$NO$2]=$

$1\mathrm{.}8$x$10-8$ M and $[$O$3]=1\mathrm{.}4$x$10-7$ M$?$

c$.$ What is the rate of formation of NO $3$ under these conditions?

d$.$ What happens to the rate of the reaction if the concentration of O$3$ is doubled?