1. The problem statement, all variables and given/known data Consider the following reaction at 282 K. 2 A + 2 B → C + D where rate = rate=k[A]2. An experiment was performed for a certain number of seconds where [A]0 = 0.000303 M and 0 = 1.63 M. A plot of ln[A] vs time had a slope of -7.27. What will the rate of this reaction be when [A] = = 0.503 M? Rate (M/s)= The correct answer is 0.348 M/s. 2. Relevant equations I'm not sure where to start here, but I tried using these equations, because I was given the slope, and the slope for ln[A] vs time is given in a first order reaction: ln[A]t = -kt + ln[A]o Rate = k[A] k = -slope 3. The attempt at a solution Basically I just tried plugging into k = 7.27 into rate=k[A]2 were [A] and are both 0.503 M. Thank you for the help!