The rate of a certain reaction is given by the following rate law:

rate $=k[N_2{]}^3[O_3]$

Use this information to answer the questions below.

$\backslash$table$[[$What is the reaction order in $N_2?,],[$What is the reaction order in $O_3?,],[$What is overall reaction order?,$],[\backslash$table$[[$At a certain concentration of $N_2$ and $O_3,$ the initial rate of$],[$reaction is $96\mathrm{.}0\frac{M}{s}.$ What would the initial rate of the$],[$reaction be if the concentration of $N_2$ were halved? Round$],[$your answer to $3$ significant digits.$]],],[\backslash$table$[[$The rate of the reaction is measured to be $0\mathrm{.}320\frac{M}{s}$ when$],[[N_2]=1\mathrm{.}5M$ and $[O_3]=1\mathrm{.}6M.$ Calculate the value of the rate$],[$constant$.$ Round your answer to $2$ significant digits.$]],k=M^{-3}*s^{-1}$