Question

Step 1: (slow)
Step 2: NO3(g) + CO(g) + NO2(g) + CO2(g) (fast)
Overall: NO2(g) + CO(g) + NO(g) + CO2(g)
A two-step reaction mechanism is proposed for a gas-phase reaction, as represented above. Which of the following correctly identifies both the chemical equation for step 1 and the rate law for the overall reaction?
A) The chemical equation for step 1 is 2 NO2(g) → NO(g) + NO3(g), and the rate law is rate = (NO,].
B) The chemical equation for step 1 is NO2(g) + CO(g) + NO(g) + CO2(g), and the rate law is rate = [NO2][CO).
C) The chemical equation for step 1 is NO3(g) + 2 CO(g) + NO(g) + 2 CO2(g), and the rate law is rate = [NO2][CO).
D) The chemical equation for step 1 is NO3(g) + NO2(g) + 2 CO(g) + NO(g) + NO2(g) + 2 CO2(g), and the rate law is rate = [NO3][NO2][CO]".

Answer 1

Answer:

The chemical equation for step 1 is 2 NO2(g) → NO(g) + NO3(g), and the rate law is rate = k[NO2]^2

Explanation:

We know that the rate determining step is the slowest step in a sequence of non elementary reactions.

As we can see, the first reaction is slow so it is the rate determining step. From here we obtain the rate equation.

Also, the specie NO3 is absent in the overall reaction equation indicating that it is merely an intermediate produced in step 1 and used up in step 2.

Answer 2

The chemical equation for step 1 is $2 NO_2(g) \rightarrow NO(g) + NO_3(g)$, and the rate law is $rate = k[NO_2]^{2}$.

The rate -determining step is the slowest step in a sequence of non -elementary reactions.  The first reaction is slow so it is the rate determining step. From here we obtain the rate law.

Also, the specie $NO_3$  is absent in the overall reaction equation indicating that it is merely an intermediate produced in step 1 and used up in step 2.

So, the chemical equation for step 1 is $2 NO_2(g) \rightarrow NO(g) + NO_3(g)$, and the rate law is $rate = k[NO_2]^{2}$.

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