E17D.4(b) The activation energy for the decomposition ofbenzene diazoniumchloride is 99.1 kJ mol". At what temperature is the rate constant 10 per centgreater than at 25 °C?16

The activation energy at 25˚C is 99.1 kJ/mol. Let k1 is the rate constant at 25˚C and k2 at T2. The…

Answered: E17D.4(b) The activation energy for the…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.63QE

See similar textbooks

Similar questions

The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
In aqueous solution buffered at a pH of 6.75 Penicillin G (molecular weight of 334.39 g/mole) undergoes hydrolysis via a pseudo first order reaction that has an activation energy of 77.3 kJ/mole and a pseudo first order rate constant of 1.58 x 10-7 s-1 at 30°C. What is the half life (in days) of Penicillin G under the conditions described?
The activation energy for the decomposit ion of benzene diazon ium chloride is 99.1 kJ mol-1. At what temperature w ill the rate be 10 per cent greater than its rate at 25 oC?
The rate of a 2nd order decomposition reaction was measured at 700 and 1000 K with the following rate constants 0.011 and 145 M-1 s-1. Calculate the activation energy and A.
The decomposition of [A] in solution at 75C proceeds via first order: A (aq) yields B (aq) What is the rate law for the reaction?
What is the activation energy of a reverse reaction at 679 K if the foward reaction has a rate constant of 50 M-1s-1, a pre-exponential factor of 30 M-1s-1, and a delta H of the reaction of 23 kJ/mol?
Given the following details about a reaction: activation energy = 2.3E4 J/mol Should the temperature be increased from the initial temperature of 473.15K to 523.15K, what factor will the rate constant will be increased to?
A chemical reaction is conducted at 2 different temperatures. When the reaction is conducted at 400 K, the reaction constant was measured as 2.10 M-1s-1. If the activation energy of the reaction is 3.30*105 J/mol, what would the reaction constant of the reaction be if it was conducted at 410 K? (Please provide your answer to 3 significant figures.)
For the gas-phase reaction A + A → A2, the experimental rate constant, kr, has been fitted to the Arrhenius equation with a frequency factor A = 4.07 × 105 dm3 mol−1 s−1 at 300 K and an activation energy of 65.4 kJ mol−1. Calculate Δ‡S, Δ‡H, Δ‡U, and Δ‡G for the reaction.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

E17D.4(b) The activation energy for the decomposition ofbenzene diazonium chloride is 99.1 kJ mol". At what temperature is the rate constant 10 per cent greater than at 25 °C? 16