THE RATE LAW FOR THE REACTION 2NO + 02 = 2NO2 IS FIRST ORDER IN OXYGEN AND SECOND ORDER IN NO. PROPOSE A MECHANISM IN WHICH EACH STEP IS BIMOLECULAR. SPECIFY THE SLOW STEP.

I HAVE NO IDEA WHAT TI DO. HELP PLEASE? THANKS.

Here is a proposed mechanism.

http://bouman.chem.georgetown.edu/S02/lect5/lect5.htm

To propose a mechanism for a given reaction, we need to break down the overall reaction into individual steps and determine which steps are likely to occur based on their reaction rates. In this case, we are looking for a mechanism with each step being bimolecular, meaning involving two molecules.

The given reaction is:
2NO + O2 → 2NO2

To propose a mechanism, we need to consider possible elementary steps. Here's one possible mechanism:

1. Step 1: NO + O2 → NO3 (bimolecular)
In this step, NO and O2 react to form NO3.

2. Step 2: NO3 + NO → 2NO2 (bimolecular)
In this step, NO3 reacts with another NO molecule to produce 2NO2.

The slow step in the proposed mechanism is typically the one that determines the overall rate of the reaction. In this case, when comparing the reaction rates of the two steps, we see that Step 1 involves O2, which is first-order according to the rate law. Thus, Step 1 is likely to be the slow step.

It's important to note that proposed mechanisms are not unique, and alternative mechanisms could exist. However, the mechanism proposed here satisfies the criteria of each step being bimolecular and being consistent with the given rate law.

Remember that proposing a mechanism involves some degree of creativity and understanding of chemical reactions. It's a good idea to consult your textbook, class notes, or a chemistry professor for further guidance and to verify your answer.