1. The problem statement, all variables and given/known data 1. According to the mechanism below, what is the correct expression for the rate of consumption of A? In the mechanism, M is a molecule that collides with A and A* is a highly-energized form of A. Step 1 (reversible): A + M <---> A* + M rate constants k1 and k-1 Step 2 (irreversible): A* ---> C rate constant k2 Select one of the following: Rate = k1 [A] [M] / (k-1[M] + k2) Rate = [A] / [C] Rate = k1k2 [A] [M] / (k-1[M] + k2) Rate = k1k2 [A] Rate = k1[A] Rate = (k1 [A] [M] + k-2[C] ) / (k-1[M] + k2) Rate=k1k2 / (k-1+k-2) Rate = (k1+k2-k-1-k-2) [A] Rate = k1k2 [A] / (k-1+k2[M]) Rate=k1+k2-k-1-k-2 Rate = [C] / [A] Rate = k1k2 [A] [M] / k-1 2. Relevant equations 3. The attempt at a solution I tried to assume a steady-state approximation as I'm not sure which is the slow step. I found the overall rate of reaction and assumed it to be equivalent to the consumption of A.