The rate law for the reaction A2Bm2 (aq) + 2A(aq) + 2D(aq) -> D2 (aq)  + 2A2Bm (aq) is rate = k[A2Bm2]2[D]. What is the overall order of the reaction?

2 A(aq) + 3 B(aq) A2B3(aq) An experiment is conducted at 25 C and the rate of appearance of the product ABa(aq) is measured as the concentrations of the reactants were varied. Data from the trials are shown below. Initial Rate of Trial [A] (M) [B] (M) Appearance of A2B3 (M/s) 5.0 x 10 4.5 x 10 1.0 x 10 0.200 0.300 0.200 0.900 0.400 0.300 4 0.135 0.225 ??? Determine the rate law for the reaction. Justify your answer. Determine the value of k, including units. Determine the rate of Trial 4. a. b. с. d. Determine the initial rate of disappearance of A for trial 2. A possible reaction mechanism has a 1" elementary step as shown below: e. A +BAB Could this first step be the rate determining step? Explain your reasoning. In the reaction mechanism the compound MnO2 appears. A student makes the claim f. "The order of MnO2 must be zero since it does not appear in the overall balanced equation". Do you agree or disagree with the student? Explain your reasoning. g. In trial 1, 10 mL of A and 10…

If you have a reaction A + B --> C, and the rate equation is Rate = k [A], what can you infer about the mechanism of the reaction?

a) What are the units of the rate constant for a zero-order reaction?b) What are the units of the rate constant if rate =k[A]5[B]3[C]?c) What is the order of reaction for part (b) of this question?