4. The following data were obtained for the hypothetical reaction 2A + B → products.[A]0.20.20.6a) The order with respect to reactant A =b) The order with respect to reactant B =Overalld) Rate Law =이이이[B]0.10.20.1reaction order = 2 - 1Rate (M/s)520452 bederordere) Determine the value of the rate constant k with the correct units

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4. The following data were obtained for the hypothetical reaction 2A + B → products. [A] 0.2 0.2 0.6 [B] 0.1 0.2 0.1 a) The order with respect to reactant A = b) The order with respect to reactant B = Overall reaction order = Rate Law = Rate (M/s) 5 20 45 order c) d) e) Determine the value of the rate constant k with the correct units

4. The following data were obtained for the hypothetical reaction 2A + B → products. [A] 0.2 0.2 0.6 [B] 0.1 0.2 0.1 a) The order with respect to reactant A = b) The order with respect to reactant B = Overall reaction order = Rate Law = Rate (M/s) 5 20 45 order c) d) e) Determine the value of the rate constant k with the correct units

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 12QAP: A reaction has two reactants Q and P. What is the order with respect to each reactant and the...

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The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?
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You are studying the kinetics of the reaction H2(g) + F2(g) 2HF(g) and you wish to determine a mechanism for the reaction. You run the reaction twice by keeping one reactant at a much higher pressure than the other reactant (this lower-pressure reactant begins at 1.000 atm). Unfortunately, you neglect to record which reactant was at the higher pressure, and you forget which it was later. Your data for the first experiment are: Pressure of HF (atm) Time(min) 0 0 0.300 30.0 0.600 65.8 0.900 110.4 1.200 169.1 1.500 255.9 When you ran the second experiment (in which the higher pressure reactant was run at a much higher pressure), you determine the values of the apparent rate constants to be the same. It also turns out that you find data taken from another person in the lab. This individual found that the reaction proceeds 40.0 times faster at 55C than at 35C. You also know, from the energy-level diagram, that there are three steps to the mechanism, and the first step has the highest activation energy. You look up the bond energies of the species involved and they are (in kJ/mol): H8H (432), F8F (154), and H8F (565). a. Sketch an energy-level diagram (qualitative) that is consistent with the one described previously. Hint: See Exercise 106. b. Develop a reasonable mechanism for the reaction. c. Which reactant was limiting in the experiments?
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