The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 80.0 kJ/mol. If the rate constant of this reaction is 0.013 M¹-s¹ at 150.0 °C, what will the rate constant be at 194.0 °C? Round your answer to 2 significant digits. -1 |* = M²³²-5²² S

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 80.0 kJ/mol. If the rate constant of this reaction is 0.013 M¹-s¹ at 150.0 °C, what will the rate constant be at 194.0 °C? Round your answer to 2 significant digits. -1 |* = M²³²-5²² S

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 rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E, = 8.0 kJ/mol. If the rate constant of this reaction is 1.1 x 10° M -1 -1 'S at 160.0 °C, what will the rate constant be at 108.0 °C? Round your answer to 2 significant digits.
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 314.0 °C 2.1 x 10¹1 384.0 °C 4.3 × 10¹1 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. kJ E = x10 a mol X Ś ?
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 59.0 °C 6.5 x 101 14 163.0 °C |4.2 × 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E x10 mol
-1 For a certain reaction, the frequency factor A is 7.5 × 10⁹ s1 and the activation energy is 21.4 What is the rate constant for the reaction at 95. °C? Round your answer to 2 significant digits. Note: Reference the Fundamental constants table for additional information. k = -1 S X kJ mol S
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=67.0 kJ/mol. If the rate constant of this -1 −1 reaction is 3.9 M •S at 99.0 °C, what will the rate constant be at 178.0 °C? Round your answer to 2 significant digits. - 1 -1 ☐ k = M • S ? x10 X Ś
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=69.0 kJ/mol. If the а - 1 rate constant of this reaction is 5.7 × 10² M - 1 S. at 304.0 °C, what will the rate constant be at 256.0 °C? Round your answer to 2 significant digits. - 1 - 1 k = || M •S x10 ?
When a reaction is performed at a temperature of 314. K, the rate constant is 1.9 x 10-6 s-1. When performed at 457. K, the rate constant is 8.5 x 104s-1. Calculate the activation energy_(Ea) of this reaction, in units of kJ/mol.
Calculate the rate constant, k, for a reaction at 73.0 °C that has an activation energy of 77.2 kJ/mol and a frequency factor of 2.61 x 10¹¹ s-¹. k = X10 TOOLS $1
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E, = 9.0 kJ/mol. If the rate constant of this reaction is 1.1 x 10 M 's -1 at 226.0 °C, what will the rate constant be at 146.0 °C? 10° Round your answer to 2 significant digits.
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 258.0 °C 3.9 x 1010 153.0 °C 1.5 × 1010 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ E х10 a mol
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=77.0 kJ/mol. If the rate constant of this reaction is 5.5 × 10 4 1 M S. at 55.0 °C, what will the rate constant be at 16.0 °C? -1 Round your answer to 2 significant digits. 1 1 k = ]Ms •S
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 407.0 °C 4.8 x 10¹0 268.0 °C 2.3 × 10 ¹0 a Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 a mol X 3 ?