The experimental rate law for the reaction, NO2+CO ⟶CO2+NO, is rate =k[NO2]^2. If the mechanism

step 1 So the equation for the reaction between N -O -2 and CO forms CO2 and N -O. And the experimental

The experimental rate law for the reaction, NO2+CO ⟶CO2+NO,...

The experimental rate law for the reaction, $\mathrm{NO}_{2}+\mathrm{CO} \longrightarrow \mathrm{CO}_{2}+\mathrm{NO}$, is rate $=k\left[\mathrm{NO}_{2}\right]^{2}$. If the mechanism is show that the predicted rate law is the same as the experimental rate law.

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Key Concepts

Rate-Determining Step

The rate-determining step is the slowest step in a multi-step reaction mechanism, controlling the overall reaction rate. Because its kinetics limit the entire process, the rate law for this step often mirrors the experimentally observed rate law.

Elementary Reaction Steps

Elementary reaction steps are the individual, fundamental reactions that occur in a single collision or event and follow the law of mass action. Their simple form helps in deriving the predicted rate law when combined appropriately in a mechanism.

Rate Law

The rate law expresses the quantitative relationship between the reaction rate and the concentrations of the reactants. It indicates the overall order of the reaction and is determined experimentally, revealing how changes in concentrations affect the speed of the reaction.

Reaction Mechanism

A reaction mechanism is a proposed sequence of elementary steps that collectively describe the process by which reactants transform into products. It must yield the overall balanced reaction and explains the observed rate law through the contributions of each step.

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