Please don't Provide handwritten solution ....... Fraction of moleculesThe exponential term in the Arrhenius equation is equal to the fraction of molecules, f, with kinetic energy greater than or equal tothe activation energy:f=e-E₂/(RT)Most scientific calculators have an ex function as the second function of the LN button.Part BA certain reaction with an activation energy of 105 kJ/mol was run at 465 K and again at 485 K. What is the ratio of f at thehigher temperature to f at the lower temperature?Express your answer numerically using one significant figure.▸ View Available Hint(s)fusfusSubmitVE ΑΣΦΑ

Given:Activation energy (Ea) = The reaction is run at two different temperatures:lower temperature…

Answered: Fraction of molecules The exponential…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 62QRT

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Experiments during a recent summer on a number of fireflies (small beetles, Lampyridaes photinus) showed that the average interval between flashes of individual insects was 16.3 s at 21.0C and 13.0 sat 27.8C. a. What is the apparent activation energy of the reaction that controls the flashing? b. What would be the average interval between flashes of an individual firefly at 30.0C? c. Compare the observed intervals and the one you calculated in part b to the rule of thumb that the Celsius temperature is 54 minus twice the interval between flashes.
For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min at 728C. (a) What is the activation energy of the reaction? (b) What is k at 485C? (c) At what temperature is k, the rate constant, equal to 11.6 L/mol min?
Consider the following hypothetical reaction: X( g )Y( g ) A 200.0-mL flask is filled with 0.120 moles of X. The disappearance of X is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the appearance of Y. (b) Calculate the average disappearance of X in M/S in the first two 20-minute intervals. (c) What is the average rate of appearance of Y between the 20- and 60-minute intervals?
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
For the reaction QW+X, the following data were obtained at 30 C: [Q]initial (M) 0.170 0.212 0.357 Rate(mol/L/s) 6.68103 1.04102 2.94102 (a) What is the order of the reaction with respect to [Q], and what is the rate equation? (b) What is the rate constant?
A study of the rate of the reaction represented as 2AB gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [A](M) 1.00 0.775 0.625 0.465 0.350 0.205 0.230 (a) Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s. (b) Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus [A]. What are theunits of this rate? (c) Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.
Bacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.
For the reaction AB+C, the following data were obtained at 30 C: [A] (M) 0.230 0.356 0.557 Rate (moI/L/s) 4.17104 9.99104 2.44103 (a) What is the order of the reaction with respect to [A], and what is the rate equation? (b) What is the rate constant?

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