For the gas phase isomerization of cis-cyanostyrene, cis-C6H3CH=CHCNtrans-CGH5CH=CHCN the rate constant has been determined at several temperatures. When In k in s-l is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.32×104 K and a y-intercept of 26.7. The activation energy for the gas phase isomerization of cis-cyanostyrene is kJ/mol.

For the gas phase isomerization of cis-cyanostyrene, cis-C6H3CH=CHCNtrans-CGH5CH=CHCN the rate constant has been determined at several temperatures. When In k in s-l is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.32×104 K and a y-intercept of 26.7. The activation energy for the gas phase isomerization of cis-cyanostyrene is kJ/mol.

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...

See similar textbooks

Similar questions

The following data are for the gas phase decomposition of sulfuryl chloride at 600 K.SO2Cl2(g) SO2(g) + Cl2(g) [ SO2Cl2 ], M 3.73×10-3 1.87×10-3 9.35×10-4 4.68×10-4 time, min 0 203 406 609 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is ________ min .(2) Based on these data, the rate constant for this _______(zero, first, or second) order reaction is __________min-1.
Knowledge about the speed of chemical reactions is extremely important for industrial production, especially when optimizing a process. In this sense, strategies can be developed based on changes in the surface area, concentration of reactants, system temperature, and the use of catalysts. Considering this information, analyze the following statements: I. The frequency and orientation of collisions between the reacting species, as well as the amount of energy in the system, are determining factors for the formation of the activated complex. II. The use of catalysts provides an alternative pathway for the formation of the activated complex with lower activation energy, consequently increasing the reaction rate. III. Exothermic transformations are more advantageous because they release energy during product formation, thereby eliminating the need to supply energy to the reactants. Is it correct to assert that:
The activation energy for a reaction is determined to be 389.9 kJ. The rate constant at 20.5ºC is equal to 4.06 x 10-6 s-1. What is the rate constant at 34.9ºC for the reaction? Report your answer to the tenths place and using scientific notation (e.g. 1.27 x 103 or -1.27 x 10-3) and do not include units
I don’t know how to do this question about activation energy.
For the gas phase decomposition of bromoethane, CH;CH,Br >C,H4 + HBr -1 the rate constant in s has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of-2.63x104 K and a y-intercept of 29.6. The value of the rate constant for the gas phase decomposition of bromoethane at 703 K is -1 (Enter your answer to one significant figure.)
For the gas phase decomposition of t-butyl acetate, CH3COOC(CH,))3– 3/3 (CH,)2C=CH, + CH,COOH 3/2 the rate constant has been determined at several temperatures. When In k in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.04×104 K and a y-intercept of 30.7. The activation energy for the gas phase decomposition of t-butyl acetate is kJ/mol.
Gaseous SO2Cl2 undergoes the following decomposition: SO2Cl2 (g) --> SO2(g) +Cl2(g) The above reaction has a second-order kinetic dependence on the SO2Cl2 concentration with a rate constant of (0.00400 M-1* s-1). If one starts with 0.0641 molar SO2Cl2 at time zero, what is the calculated molar concentration of SO2Cl2 remaining after 40.23 minutes of decomposition of the initial SO2Cl2
Please don't provide handwritten solution ....
13. The following data give the temperature dependence of the rate constant for the reaction N₂O4 →→ 2NO21/202. Plot the data and calculate the activation energy of the reaction. T(K) 273 298 308 318 328 338 k (sec-¹) 7.87 x 10-7 3.46 x 10-5 1.35 x 104 4.98 x 104 1.50 x 10-³ 4.87 x 10-3
The following data are for the gas phase decomposition of sulfuryl chloride at 600 K. sO,C2(g)- - SO2(g) + Cl2(g) [ SO;Clz ], M 2.89x103 1.45x103 7.25x104 3.63x104 time, min 168 336 504 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is | min. (2) Based on these data, the rate constant for this order reaction is min
The half-lives for the forward and reverse reactions that are first order in both directions are 82ms and132ms respectively. Calculate the corresponding relaxation time for return to equilibrium after a temperature jump