7. Cyclobutane decomposes to ethene in a first-order reaction. From measurements of the rate constant (k) at various absolute temperatures (T), the accompanying Arrhenius plot was obtained (In k versus 1/T). | a. Calculate the energy of activation, Ea. b. Determine the value of the rate constant at -3 740. K. (In the plot, the units of k are s1.) -4 -5 -6 -7 -8 -9 0.00125 0.0013 0.00135 0.0014 0.00145 1/T (1/K) In k

7. Cyclobutane decomposes to ethene in a first-order reaction. From measurements of the rate constant (k) at various absolute temperatures (T), the accompanying Arrhenius plot was obtained (In k versus 1/T). | a. Calculate the energy of activation, Ea. b. Determine the value of the rate constant at -3 740. K. (In the plot, the units of k are s1.) -4 -5 -6 -7 -8 -9 0.00125 0.0013 0.00135 0.0014 0.00145 1/T (1/K) In k

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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17. Which of the following expressions corresponds to the integrated rate equation for a first-order decomposition reaction? (RESEARCH) a. [A] = -kt b. [A] = [A]o -kt c. In [A] = In [A]o –kt d. 1 = -kt [A] е. 1 1 - kt TAJO [A]
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4. What is the value of x, the order of the reaction with respect to [OH']? k'/k" = (1/0.5)* 5. What is the value for the rate constant, k? k= k'/1* = %3D k =k"/0.5*= SaD 6.
The following reaction is first order in respect to CH3OH and first order in respect to HCl. With this in mind, what is the rate constant for the reaction? Be sure you choose the answer with the right units. CH3OH(aq) + HCL(aq) ----> CH3CL(aq) + H2O(i) Reaction CH3OH conc. HCl conc. Initial Rate (M/s) 1 0.100 M 0.100 M 1.1 x 10-2
Explain further... thank you!
3. The time integrated rate law of a reaction involves a single reactant A of order (1/2) is:
15. The decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 10-2 s-1.By what factor will the pressure of sulfuryl chloride decrease after 6 half-lives? Note: The answer wants this value: (360. torr)/value = final pressure after decay _______ value
Imagine you are working with a decomposition reaction. This reaction was calculated to be an overall 2nd order reaction with a reaction rate of 1.65 Ms-1 with an initial concentration of 1.70 M. at 25* C. What is k? If the activation energy of this reaction is 82.5 kJ and you redo the reaction at 20* C, what is the new k value?
26. A reaction is second order with respect to reactant "A". Find the rate constant, k, if the initial concentration of A is 0.25 M and drops to 0.053 M in 30. seconds? Group of answer choices A. 5.0 x 10E(-1) /Ms B. 6.6 x 10E(-3) /Ms C. 5.2 x 10E(-2) /Ms D. 2.7 x 10E(-1) /Ms
Be sure to answer all parts. Consider the reaction A+BProducts From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. A. JA] (M) (BỊ (M) Rate (Mis) 1.50 1.50 3.20 x 10 1.50 2.50 3.20 x 10 Reaction 3.00 1.50 6.40 x 10
14. The overall order of reaction for the elementary reaction A + 2B a. 0 b. 1 c. 2 d. 3 * > Cis 15. If the volume of a container for the above reaction (Problem 14) is suddenly reduced to ½ its original volume with the moles of A, B & C maintained constant, the rate will increase by a factor of a. 2 b. 4 c. 8 d. 16
5.00 mL 4.50 M acetone + 10.0 mL 1.15 M HCl + 10.0 mL 0.00200 M I2 + 25.0 mL H2O A student found that it took 146 seconds for the color of the I to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of Iz in the reaction mixture, [I2]o. Then use the equation Rate At t M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H", and iodine to I2. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). Rate O[Ace] (Previous Next