The following reaction mechanism has been proposed for a reaction:

(slow) NO2 + NO2-> NO3 + NO
(fast) NO3 + CO -> CO2 + NO2

A. Write the equation for the overall reaction from the mechanism above.

B.Write the rate law for the reaction

A. To obtain the overall reaction from the proposed mechanism, we need to cancel out the intermediates NO3 and NO2.

Adding the two proposed reactions together:
(NO2 + NO2) + (NO3 + CO) -> (NO3 + NO) + (CO2 + NO2)

Simplifying, we get:
2NO2 + NO3 + CO -> CO2 + 2NO

Therefore, the overall reaction from the mechanism above is:
2NO2 + NO3 + CO -> CO2 + 2NO

B. The rate law for a reaction is determined by the slowest step in the mechanism. As given, the slow step in this mechanism is the first one:
(slow) NO2 + NO2 -> NO3 + NO

The rate-determining step involves the collision between NO2 and NO2. Assuming the rate of this step depends on the concentration of NO2, the rate law for the reaction can be written as:

Rate = k[NO2]^2

Where k is the rate constant and [NO2] represents the concentration of NO2.

A. To write the overall reaction, we need to cancel out any species that appear both as reactants and products. In this case, NO2 appears in both the reactant and product sides of the first step. Thus, we can simplify the mechanism to:

(slow) NO2 -> NO3 + NO
(fast) NO3 + CO -> CO2 + NO2

Now, we can combine these two steps to write the overall reaction:

NO2 + CO -> CO2 + NO

B. To write the rate law for the reaction, we need to determine the rate-determining step from the mechanism. In this case, the slow step is the rate-determining step.

Based on the rate-determining step, we can determine the rate law by looking at the stoichiometry of the reactants involved. In the slow step, the reactant NO2 is involved. Therefore, the rate law can be written as:

Rate = k[NO2]^[y]

The exponent, y, represents the order of the reaction with respect to NO2, which can be determined experimentally.