The two pictures shown below represent starting conditions for the following reaction: O3 (g) + NO(g) → O2 (g) + NO2 (g) with a rate law: Rate = k (O3 )(NO) Which flask will react faster than the other? Determine how much faster the fast one reacts compared to the slow one? Explain your answers in terms of molecular collisions.

How do I find the answer to this? My thinking is that box a will react more since there's equal amounts of reactants but box b will react faster since there's so much NO to collide with the O3 molecules. Thanks.