Questions: C. The reaction of NO2(g) and CO(g) is thought to occur in two steps: Step 1 slow NO2(g)+NO2(g) → NO(g)+NO3(g) Step 2 Fast NO3(g)+CO(g)+NO2(g)+CO2(g) What is the molecularity of Step 2? bimolecular termolecular unimolecular (d) The reaction of NO2(g) and CO(g) is thought to occur in two steps: Step 1 Slow NO2(g)+NO2(g) → NO(g)+NO3(g) Step 2 Fast NO3(g)+CO(g) → NO2(g)+CO2(g) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? rate =k[NO2] rate =k[NO2]^2 rate =k[NO2][CO]

C. The reaction of NO2(g) and CO(g) is thought to occur in two steps:

Step 1 slow
NO2(g)+NO2(g) → NO(g)+NO3(g)

Step 2 Fast
NO3(g)+CO(g)+NO2(g)+CO2(g)

What is the molecularity of Step 2?
bimolecular
termolecular
unimolecular

(d) The reaction of NO2(g) and CO(g) is thought to occur in two steps:

Step 1 Slow
NO2(g)+NO2(g) → NO(g)+NO3(g)

Step 2 Fast
NO3(g)+CO(g) → NO2(g)+CO2(g)

For this mechanism to be consistent with kinetic data, what must be the experimental rate equation?
rate =k[NO2]
rate =k[NO2]^2
rate =k[NO2][CO]

Transcript text: C. The reaction of $\mathrm{NO}_{2}(g)$ and $\mathrm{CO}(g)$ is thought to occur in two steps: Step 1 slow \[ \mathrm{NO}_{2}(g)+\mathrm{NO}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{NO}_{3}(g) \] Step 2 Fast \[ \mathrm{NO}_{3}(g)+\mathrm{CO}(g)+\mathrm{NO}_{2}(g)+\mathrm{CO}_{2}(g) \] What is the molecularity of Step 2? bimolecular termolecular unimolecular (d) The reaction of $\mathrm{NO}_{2}(g)$ and $\mathrm{CO}(g)$ is thought to occur in two steps: Step 1 Slow \[ \mathrm{NO}_{2}(g)+\mathrm{NO}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{NO}_{3}(g) \] Step 2 Fast \[ \mathrm{NO}_{3}(g)+\mathrm{CO}(g) \rightarrow \mathrm{NO}_{2}(g)+\mathrm{CO}_{2}(g) \] For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? rate $=\mathrm{k}\left[\mathrm{NO}_{2}\right]$ rate $=k\left[\mathrm{NO}_{2}\right]^{2}$ rate $=k\left[\mathrm{NO}_{2}\right][\mathrm{CO}]$

Solution

Solution Steps

Step 1: Identify the Molecularity of Step 2

The molecularity of a reaction step refers to the number of reactant molecules involved in that step. For Step 2: \[ \mathrm{NO}_{3}(g) + \mathrm{CO}(g) \rightarrow \mathrm{NO}_{2}(g) + \mathrm{CO}_{2}(g) \] There are two reactant molecules: $\mathrm{NO}_{3}(g)$ and $\mathrm{CO}(g)$. Therefore, the molecularity of Step 2 is bimolecular.

Final Answer

$\boxed{\text{bimolecular}}$

Step 2: Determine the Experimental Rate Equation

To determine the experimental rate equation, we need to consider the rate-determining step (slow step) and how it relates to the overall reaction. The given steps are:

Step 1 (Slow): \[ \mathrm{NO}_{2}(g) + \mathrm{NO}_{2}(g) \rightarrow \mathrm{NO}(g) + \mathrm{NO}_{3}(g) \]

Step 2 (Fast): \[ \mathrm{NO}_{3}(g) + \mathrm{CO}(g) \rightarrow \mathrm{NO}_{2}(g) + \mathrm{CO}_{2}(g) \]

Since Step 1 is the slow step, it determines the rate of the overall reaction. The rate law for Step 1 is: \[ \text{rate} = k[\mathrm{NO}_{2}]^2 \]

Final Answer

$\boxed{\text{rate} = k[\mathrm{NO}_{2}]^2}$

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