For a particular first order reaction at 25 °C, the concentration of reactants reduced to one halfof its initial value after 5000 s. At 35 °C, the concentration is halved after 1000 s. Calculate(i)the rate constant of the reaction at 25 °C;(ii)the time required for the concentration to be reduced to one quarter of its initial valueat 35 °C; and(iii)the activation energy of the reaction.

Answered: Image /qna-images/answer/28965787-0cd6-4395-92c2-3ebf9521c034.jpg

Answered: For a particular first order reaction…

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

A substance decomposes according to first order kinetics. The rate constants at various temperatures are as follows: T(°C) 600 650 700 750 k (S^(-1)) 1.87x10-3 0.0113 0.569 0.244 Calculate the activation energy required
A certain 2nd order reaction is known to proceed by a two-step process such that k1<<k2. The forward reaction has an activation energy of 48 kJ/mole and the reverse reaction has an activation energy of 62 kJ/mole. Sketch the energy diagram for the reaction.
The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 x 10-15 s-1 at 298 K and a rate constant of 8.66 x 10-7 s-1 at 425 K. Determine the activation energy for this reaction in kJ/mol.
(b) The half-life for the decomposition of dinitrogen pentoxide at 70 °C is 101.6 s. At the beginning of the decomposition reaction, 0.025 moles of dinitrogen pentoxide were dissolved in 2 x10³ cm³ of water. Assuming that the reaction follows the first order reaction, predict the duration (in minutes) for the dinitrogen pentoxide to decompose to 0.01 mol.
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 rate constant for a reaction varies between 0.590 L·mol-1·s-1 at 325°C and 2.10 L·mol-1·s-1 at 400°C. Determine the activation energy for this reaction to the nearest whole number in units of kilojoules per mole. Include only the numerical answer (no units).
The kinetics of a gas phase reaction of the form A → Products results in a rate constant of 1.308 M-1 s-¹. For this reaction, the initial concentration of A is 0.483 M. At what time would the concentration of A reach 0.042 M?
Our body obtains energy from the combustion of glucose. During this process, glucose is transformed first into fructose. This reaction has an activation energy close to 55 kJ inside our body, where the process is catalyzed by enzimes. Without these catalysts, the activation enerrgy is close to 97 kJ. How many times does the catalyst increase the rate of this reaction in our body at a normal temperature close to 98.6 F (37 °C)? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b с d 1.8 times 1.2 x 107 times 2.3 x 104 times 780 times X Your answer
Given the same reactant concentrations, the reaction CO(g) + Cl2(g) → COCl2(g) at 249°C is 48.4 times as fast as the same reaction at 169°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
For the first-order reaction N2O5( g) 2 NO2 g) + → t1/2= 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 105 s', determine the value of k at 50°C.
The rate constant for a first-order reaction is 2.66 × 10‒2 s‒1 at 298 K. What is the rate constant at 350. K if the activation energy for the reaction is 52.9 kJ/mol?
6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO2 (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS