The mechanism for the reaction of nitrogen dioxide with...

The mechanism for the reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be $$ \begin{aligned} \mathrm{NO}_{2}+\mathrm{NO}_{2} \longrightarrow \mathrm{NO}_{3}+\mathrm{NO} & \text { Slov } \\ \mathrm{NO}_{3}+\mathrm{CO} \longrightarrow \mathrm{NO}_{2}+\mathrm{CO}_{2} & \text { Fast } \end{aligned} $$ Write the rate law expected for this mechanism. What is the overall balanced equation for the reaction?

The mechanism for the reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be
$$
\begin{aligned}
\mathrm{NO}_{2}+\mathrm{NO}_{2} \longrightarrow \mathrm{NO}_{3}+\mathrm{NO} & \text { Slov } \\
\mathrm{NO}_{3}+\mathrm{CO} \longrightarrow \mathrm{NO}_{2}+\mathrm{CO}_{2} & \text { Fast }
\end{aligned}
$$
Write the rate law expected for this mechanism. What is the overall balanced equation for the reaction?

Key Concepts

Reaction Mechanism

A reaction mechanism is a detailed, step-by-step description of the sequence of elementary reactions by which overall chemical change occurs. It provides insight into how reactants transform into products through the formation and consumption of intermediate species.

Rate-Determining Step

The rate-determining step is the slowest step in a reaction mechanism, effectively setting the pace for the overall reaction. Because this step limits the total reaction rate, the rate law is typically based on the molecularity and stoichiometry of this step.

Rate Law Formulation

The rate law formulates the relationship between the reaction rate and the concentrations of the reacting species. For elementary steps, the law can be written directly from the stoichiometry, with the overall rate law often reflecting the concentration dependence of the rate-determining step.

Overall Reaction Equation

The overall reaction equation is obtained by summing the elementary steps of the mechanism and canceling any intermediates. This equation represents the net chemical transformation, summarizing the reactants and final products without including transient species.

Transcript

00:01 We have given a reaction mechanism that can be written as no2 plus no2 and this gives no3 plus no and that is slow step.

00:19 Then in second step i have no3 plus co and this gives no2 plus co2 that is 5.

00:32 Past step.

00:34 Now we have here two parts.

00:36 First of all we have to write the rate law.

00:39 Now rate law or reaction is determined by slow step.

01:12 Okay? always keep this in mind.

01:14 Whenever you have to find the rate law.

01:17 So rate of the reaction, that is, determined by the slowest step and so to write the rate law you will consider the slow step okay so the slow step was this right so i am considering this so now the rate law can be written as rate law is or rate equation is that the rate of the reaction is directly proportional to the concentration of reactants okay this is called rate law so now for this reaction so rate so that is directly proportional to concentration of no2 and now since no2 is being repeated for two times here right so this will be here raise to power 2 okay so now or removing this proportionality sign i can write rate is equal to k multiplied by k is the rate constant and no two raise to power two okay so this is the rate now we have second part and second part so in this we have to write the overall balanced equation so that can be written as you have two equations here add them considering this as equation first this as equation second adding 1 and 2.

03:04 So now this will be nno 2 plus n0 2 okay plus n0 3 plus co okay i added the species of one side now this gives n0 3 plus n0 2 plus n0 2 plus and no 2 plus co2.

03:36 Now, no2 to this no2 will be cancelled out, okay? and no3 to this no3 will be cancelled out.

03:49 So now we have all no2 plus co, which gives nno plus co2.

04:04 Okay? now, is this co2 plus co2? okay.

04:06 Now, is this reaction? i have that is balanced or not.

04:11 So on left side i have only one nitrogen atom and on right side also...

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