When heated, cyclopropane is converted to propene. Rate constants for this reaction at 470. °C and 510. °C are k = %3D 1.10 x 104 s and k = 1.02 x 103 s1, respectively. Determine the activation energy, Ea, from these data. S S Ea= kJ/mol %3D

When heated, cyclopropane is converted to propene. Rate constants for this reaction at 470. °C and 510. °C are k = %3D 1.10 x 104 s and k = 1.02 x 103 s1, respectively. Determine the activation energy, Ea, from these data. S S Ea= kJ/mol %3D

Name: When heated, cyclopropane is converted to propene. Rate constants for
Uploaded: 2022-11-30T19:17:17.000Z
Channel: Bartleby
Description: When heated, cyclopropane is converted to propene. Rate constants for this reaction at 470. °C and 510. °C are k =%3D1.10 x 104 s and k = 1.02 x 103 s1, respectively. Determine the activation energy, Ea, from these data.SSEa=kJ/mol%3D

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 101QRT

See similar textbooks

Similar questions

For the reaction of iodine atoms with hydrogen molecules in the gas phase, these rate constants were obtained experimentally. 2I(g) + H2(g) 2HI(g) (a) Calculate the activation energy and frequency factor for this reaction. (b) Estimate the rate constant of the reaction at 400.0 K.
Would the slope of a ln(k) versus 1/T plot (with temperature in kelvin) for a catalyzed reaction be more or less negative than the slope of the ln(k) versus 1/T plot for the uncatalyzed reaction? Explain. Assume both rate laws are first-order overall.
At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.
The rate constant for the decomposition of acetaldehyde, CH3CHO, t0 methane, CH4, and carbon monoxide, CO, in the gas phase is 1.1102 L/mol/s at 703 K and 4.95 L/moI/s at 865 K. Determine the activation energy for this decomposition.
Sucrose, a sugar, decomposes in acid solution to give glucose and fructose. The reaction is first-order in sucrose, and the rate constant at 25 C is k = 0.21 h1. If the initial concentration of sucrose is 0.010 mol/L, what is its concentration after 5.0 h?
The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the gas-phase reaction NO(g)+O3(g)NO2(g)+O2(g) which is important in the chemistry of stratospheric ozone depletion. (a) Calculate the rate constant for this reaction at 370. K. (b) Assuming that this is an elementary reaction, calculate the rate of the reaction at 370. K if [NO] = 0.0010 M and [O3] = 0.00050 M.
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2NO2(g)2NO(g)+O2(g) The rate constant at 273 K is 2.3 1012 L/mol s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.5 atm to 1.5 atm at 500. K? Assume ideal gas behavior.
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 a reaction involving the decomposition of a hypothetical substance Y, these data are obtained: Determine the order of the reaction. Write the rate law for the decomposition of Y. Calculate k for the experiment above.
The table below presents measured rate constants for the reaction of NO with ozone at three temperatures. From these data, determine the activation energy’ of the reaction in kj/mol. (Assume the temperatures all have at least two significant figures.) k (L mol-1 s’1) Temperature (K) 1.3 X 106 200 4.4 X 106 250 9.9 X 106 300