The reaction of ammonium ion with nitrite ion in aqueous solution

$N{H}_4^{+}+N{O}_2^{-}{N}_2+2H_{2}O$

is first order in

$N{H}_4^{+}$and first order in

$N{O}_2^{-}.$

Complete the rate law for this reaction in the box below.

Use the form

$k[A{]}^m[B{]}^n,$ where $\text{'}1\text{'}$ is understood for

$m,$

ndots $($don$\text{'}$t enter $1)$ and concentrations taken to the zero power do not appear.

Rate $=$

In an experiment to determine the rate law, the rate constant was determined to be $3\mathrm{.}81{10}^{-4}{M}^{-1}{s}^{-1}.$ Using this value for the

rate constant, the rate of the reaction when $[N{H}_4^{+}]=0\mathrm{.}682M$ and $[N{O}_2^{-}]=0\mathrm{.}0335M$ would be

M$/$s$.$