The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,= 19.0 kJ/mol. If the rate constant of thisa8.- 1-1reaction is 2.5 × 10° Mat 343.0 °C, what will the rate constant be at 310.0 °C?'SRound your answer to 2 significant digits.- 1- 1kI| M•Sx10

Answered: Image /qna-images/answer/aef71b1b-a0f9-4206-8482-e41f53716cec.jpg

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 19.0 kJ/mol. If the rate constant of this reaction is 2.5 × 10° M's -1 at 343.0 °C, what will the rate constant be at 310.0 °C? Round your answer to 2 significant digits. -1 k = | M

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 19.0 kJ/mol. If the rate constant of this reaction is 2.5 × 10° M's -1 at 343.0 °C, what will the rate constant be at 310.0 °C? Round your answer to 2 significant digits. -1 k = | M

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=23.0 kJ/mol. If the rate constant of this reaction is 2.0 x 10° Ms at 173.0 °C, what will the rate constant be at 151.0 °C? Round your answer to 2 significant digits.
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 of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=11.0 kJ/mol. If the rate constant of this a 1 - 1 reaction is 3.2 × 10° M S. at 112.0 °C, what will the rate constant be at 149.0 °C? Round your answer to 2 significant digits. 1 - 1 k = ] M x10 •S ?
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 ?
A certain catalyzed reaction is known to have an activation energy E= 11.0 kJ/mol. Furthermore, the rate of this reaction is measured at 296. K and found to be 1.1 × 10 M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 10% from 296. K to 326. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 11.0 kJ/mol to 11.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5% V
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
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.
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