Chapter 14, Problem 15QP

The rate law for the reaction:

$\text{N}{\text{H}}_{\text{4}}^{\text{+}}\text{(}aq\text{)+N}{\text{O}}_{\text{2}}^{\text{-}}\text{(}aq\text{)}\to {\text{N}}_{\text{2}}\text{(}g\text{)+2}{\text{H}}_{\text{2}}\text{O(}l\text{)}$

Is given by rate $\text{=}k\text{[N}{\text{H}}_{\text{4}}^{\text{+}}\text{][N}{\text{O}}_{\text{2}}^{\text{-}}\text{]}$. At $\text{25°C,}$ the rate constant is $3.0\times {10}^{-4}/M\cdot \text{s}$. Calculate the rate of the reaction at this temperature if $\text{[N}{\text{H}}_{\text{4}}^{\text{+}}\text{]=0}\text{.36 M and [N}{\text{O}}_{\text{2}}^{\text{-}}\text{]=0}\text{.075}M\text{.}$