Question

(A). You study the following reaction in a series of experiments: (CH),COH(aq) + HCl(aq) → (CH3),CCl(aq) + H20(1) At 100 °C you obtained the following data: 1 Experiment (CH3)COH), M 0.100 2 0.200 3 0.200 4 0.300 [HCI), M 0.100 0.100 0.200 0.300 Initial Rate, M/s 5.0 x 10 4 1.0 x 10 1.0 x 10-3 1.5 x 10 Please do the following: a Write the rate law for the reaction b. Indicate the order of the reaction with respect to each of the reactants, c. Find the numerical value of the rate constant, k. (B). To confirm your results from the experiments and calculations) in problem #1, you perform two additional experiments, with the following conditions: a [(CH3),COH) = 1.00 x 10M (HCI)o = 1.00 M b. [(CH3),COH]o = 1.00 M; (HCI). = 1.00 x 10'M You obtain the following data: Experiment a: Experiment b: Time, s [(CH3),COH]. M Time, s CHCI), M 0 1.00 x 10 0 1.00 x 10 10.0 9.51 x 10+ 1.0 9.50 x 10+ 20.0 9.05 x 10 2.0 9.00 x 10 30.0 8.61 x 10 4.0 8.00 x 10 60.0 7.41 x 10 8.0 6.00 x 10- 90.0 6.38 x 10+ 16.0 2.00 x 10 1200 5.49 x 104 32.0 0 Do your data confirm your results from problem #1? Explain why or why not. (C). You find a catalyst that will catalyze the reaction from problems 1 and 2. If the catalyst increases the rate of reaction by a factor of 2.0 at 100°C, what is the difference in activation energy between the catalyzed and uncatalyzed reactions?

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please just Question A , b and c

please this is chemistry based on kinetics
there's no other subject

please if you don't know the calculation based on that question, allow other experts to help out for the solutions

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Helpful Hints:   Arrhenius Equation: k = Ae–Ea/RT Gas Constant: R = 8.314 J/mol·K

Integrated Rate Laws and Half-Lives:

• Zero order: [A] = –kt + [A]0 t1/2 = [A]0/2k

• First order: ln[A] = –kt + ln[A]0 t1/2 = 0.693/k

• Second order: 1/[A] = kt + 1/[A]0 t1/2 = 1/k[A]0

• Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law