Question

The rate law for the reaction: \({{\bf{H}}_{\bf{2}}}\) (g) + 2\({\bf{NO}}\) (g) ⟶\({\bf{N}}2{\bf{O}}\) (g) + \({{\bf{H}}_{\bf{2}}}\)O(g) has been determined to be rate = k(\({\bf{NO}}\))² (\({{\bf{H}}_{\bf{2}}}\)). What are the orders with respect to each reactant, and what is the overall order of the reaction?

Short answer

The orders with respect to each reactant order in \({\bf{NO}}\)= 2; order in \({{\bf{H}}_{\bf{2}}}\)= 1; and the overall order of the reaction overall order = 3.

Step-by-step solution

Rate of a Reaction

The rate of reaction may be defined as the speed of the reactant reacting to obtaina product in a particular reaction at a particular time. The concentration of the reactant and product are represented in terms of mole/L.

\({\bf{rate = k}}{\left( {\bf{A}} \right)^{\bf{m}}}{\left( {\bf{B}} \right)^{\bf{n}}}\)

Explanation

Here m = 2 and n =1

\({\bf{rate = k(NO}}\left) {^{\bf{2}}} \right({\bf{H2)}}{\bf{.}}\)

Therefore:

The orders with respect to each reactant order in \({\bf{NO}}\) = 2; order in \({{\bf{H}}_{\bf{2}}}\)= 1; and the overall order of the reaction overall order = 3.