Question

The mechanism for the gas-phase reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be:
NO2 + NO2 -------> NO3 + NO
NO3 + CO ---------> NO2 + CO2
1. Write the rate law expected for this mechanism. What is the overall balanced equation of the reaction?

Answer 1

Explanation:

$NO_2 + NO_2 \rightarrow NO_3 + NO$ (slow)..(1)

$NO_3 + CO\rightarrow NO_2 + CO_2$ (fast)..(2)

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

The reaction occurring in more than 1 step , the rate of the reaction is determined from the reaction which is occurring at slow speed.

So, the rate of reaction for the given mechanism will be determine by step 1.

Rate law expression of the given mechanism is :

$R=k[NO_2][NO_2]$

The rate law expected for this mechanism:

$R=K[NO_2]^2$

The overall balanced equation of the reaction :

=  [1] + [2]

$NO_2+CO\rightarrow CO_2+NO$

Answer 2

The rate expression for the reaction has been $R=k\rm [NO_2]^2$. The overall balanced equation has been given as:

$\rm NO_2\;+\;CO\;\rightarrow\;NO_2\;+\;CO_2$

The rate law has been determined in dependence of rate of formation of product with the reactant concentration raised to the stoichiometric coefficient.

The rate of reaction has been given by the slow reaction in the multistep process. The slow reaction on the mechanism has been:

$\rm NO_2\;+\;NO_2\;\rightarrow\;NO_3\;+\;NO$

The rate law (R) for the reaction has been:

$R=k\rm [NO_2]\;[NO_2]\\\textit R=\textit k[NO_2]^2$

The rate expression for the reaction has been $R=k\rm [NO_2]^2$.

The overall balanced equation has been given as:

$\rm NO_2\;+\;CO\;\rightarrow\;NO_2\;+\;CO_2$

For more information about balanced equation, refer to the link:

https://brainly.com/question/7181548