Other booUILIBRIUMUsing the Arenius equation to calculate Ea from k versus T d...CiaphaThe rate constant k for a certain reaction is measured at two different temperatures:temperature k258.0 °C4.6 x 1011356.0 °C2.1 x 102Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction.d.D.Round your answer to 2 significant digits.ArkJE = ||x10molదాంత

Name: Other booUILIBRIUMUsing the Arenius equation to calculate Ea from k v
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Description: Other booUILIBRIUMUsing the Arenius equation to calculate Ea from k versus T d...CiaphaThe rate constant k for a certain reaction is measured at two different temperatures:temperature k258.0 °C4.6 x 1011356.0 °C2.1 x 102Assuming the rate constant ob

Chemical kinetics is the branch of chemistry that mainly deals with the rate of reaction and change…

Answered: Other boo UILIBRIUM Using the Arenius…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.60E

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
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.
The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at various temperatures. Plot the natural logarithm of k versus l/T and from the graph obtain the energy of activation. Temperature (oC) k (L/mol s) 320 0.527 330 0.776 340 1.121 350 1.607
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4

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