Question

Q1:a) for the following mechanism:

Step 1: NO₂(g)+NO₂(g) →NO(g) +NO3(g) Step 2: NO3(g) + CO (g) NO₂ (g) + CO₂(g)

Experimentally the rate law is found to be: Rate = k[NO₂]².

1-Write the equation for the overall reaction:

2-Identify the intermediate: (slow) (fast)

3- What is the molecularity of the rate-determining step?​

Answer 1

1-The overall reaction is the combination of the two steps, so the equation for the overall reaction can be written as:

NO₂(g) + NO₂(g) + CO(g) → NO₂(g) + CO₂(g)

2-The intermediate is the species produced in the first step and consumed in the second step, so it can be identified as:

NO3(g)

3-The rate-determining step is the slowest step in the reaction mechanism, so the molecularity of the rate-determining step is:

2 (because the rate law is found to be Rate = k[NO₂]², which implies that the rate is dependent on the concentration of two NO₂ molecules)

Step-by-step explanation:

Just tell me if you kinda confuse

ALLEN