The following diagrams represent mixtures of NO(g) and O2(𝑔). These two substances react as follows:

2 NO(𝑔)+O2(𝑔)⟶2 NO2(𝑔)

It has been determined experimentally that the rate is second order in NO and first order in O2. Based on this fact, which of the following mixtures will have the fastest initial rate? [Section 14.2]

Video transcript

Hello everyone today. We have the following problem. The reaction A plus B equals C. Has been found to be first order in A. And second order and be the diagrams below are different mixtures of A and B. Which of the following mixtures will react the fastest. So first we want to know what the rate would be and so the rate is going to be a constant K. Times the concentration of A. Which is first order times the concentration of B. Which is second order. So that receives an exponent. And so essentially the more B. We have, the faster our rate will be. And so we have to look at which diagram has more molecules of B. So for the first one as far as A goes A. Is orange. We have 123456 molecules and B. We have 123456 molecules of B. For A. I mean for two the second one molecules of A. We have a four molecules of A. And for B We have eight molecules of B. And for the 3rd 1 we have nine molecules of a. and three molecules of B. So the one that has the most molecules of B is going to be two. And so this makes sure will react the fastest overall. I hope this helped until next time