1. The problem statement, all variables and given/known data Is this first or second order rate? Calculate the rate constant and be certain to give its units. A-->products Chart A (mM) / Time 1 / 0 .5 / 11 .25 / 20 .1 / 48 .05 / 105 2. Relevant equations Well wikipedia has both the first and second order integrated reactions there http://en.wikipedia.org/wiki/Rate_equation but I have a feeling that this is some sort of weird rate reaction. 3. The attempt at a solution At first glance it looks like a second order rate but If I plug in in an attempt to find k none of the K values match. I also tried a first order reaction and that didn't work as well. Also due to the fact that the first three concentrations go down by half and the time is not consistent it is most likely not a simple first order exponential decay. You just need to trust me that plugging the times into the regular second order rate equation does not come out with a homogeneous rate constant. Well thanks guys in advanced i'm stumped.