A reaction occurs with the following stoichiometry
A + P -> AP
[A](nM) Time (s)
(a) There is no dependence of rate on P. What is the order of the reaction? Calculate the rate constant and give the units.
This part, I understand. Once the graph is plotted [A](M) vs. time(s). I can calculate the rate by taking the the slope at an instantaneous point. This reaction based on the graph is first order.
(b) Propose a two step mechanism that is consistent with the kinetics and stoichiometry of the reaction. Be sure to lable your steps descriptively, using words such as : slow, fast, and/or equilibrium. Show how your mechanism is consistent with the measured rate law. Relate the measured k to the k's in your mechanism.
(c) The data given above were measured at 10C. When the reaction was studied at 10C, that rate constant doubled. Calculate the activation energy in KJ/mol.
A -> A* (Slow)
A* + P -> AP (Fast)
Since the first reaction is the rate ...
The solution is short answers with equations.