1. Describe the process of a reaction using a differential equation assuming that the law of mass action is valid for this reaction: 2 A+B products which starts with concentrations ao = [A]t=o, bo = [B]t=0 = 2. In reaction 2NO + Br2 + 2NOBr the observed speed is: robs = 2k1 [NO][Br2] = Proposed mechanism NO + Br25 k-1 ki NOBr2 k2 NOBr2 + NO + 2NOBr Determine the overall reaction rate in terms of [NO] and [Br2] from the ] stage rates and assuming that the intermediate concentration is at steady state to remove it from the final product formation rate. Product forming speed: Describe how that speed would be in the cases k2[NO] k-1 = ki k-1 k2[NO] What is the determining stage in the reaction mechanism? 3. A+BS 2B U= = W= = d[A] - ki[A][B] - k-1[B] dt If k = ki > k-1 d[A] = k[A][B] dt Assume the initial reagent and catalyst concentrations are [A]o, [B], and o use the following balance [A]. [A] = [B] [B] to obtain an independent differential equation of [B]. Dimension the equa- tion obtained and determine if it complies with what is mentioned about the behavior of catalytic reactions at the beginning of this section. Suggestions for sizing: size with y = [A] [A]o' determine what are the dimensions of k[A]o; look for a dimensionless variable to substitute for time t