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

rate $=k[NO{]}^2[O_2]$

Use this information to answer the questions below.

$\backslash$table$[[$What is the reaction order in $NO?],[$What is the reaction order in $O_2?],[$What is overall reaction order?$],[$At a certain concentration of NO and $O_2,$ the initial rate of$],[$reaction is $99\mathrm{.}0\frac{M}{s}.$ What would the initial rate of the$],[$reaction be if the concentration of NO were doubled? Round$],[$your answer to $3$ significant digits.$],[$The rate of the reaction is measured to be $0\mathrm{.}590\frac{M}{s}$ when$],[=0\mathrm{.}75M$ and $[O_2]=1\mathrm{.}7M.$ Calculate the value of the$],[$rate constant. Round your answer to $2$ significant digits.$]]$