The rate constant of a chemical reaction increased from 0.100 s−1 to 3.10 s−1 upon raising the temperature from 25.0 ∘C to 55.0 ∘C .Part A: Calculate the value of (1/T2−1/T1) where T1 is the initial temperature and T2 is the final temperature.Part B: Calculate the value of ln(k1/k2) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.Part C: What is the activation energy of the reaction? Learning Goal:To use the Arrhenius equation to calculate theactivation energy.As temperature rises, the average kinetic energy ofmolecules increases. In a chemical reaction, thismeans that a higher percentage of the moleculespossess the required activation energy, and thereaction goes faster. This relationship is shown bythe Arrhenius equationk = Ae E./RTwhere k is the rate constant, A is the frequencyfactor, E is the activation energy, R = 8.3145J/(K mol) is the gas constant, and T is theKelvin temperature. The following rearrangedversion of the equation is also useful:k1InE.RT2where ki is the rate constant at temperature T1,and k2 is the rate constant at temperature T2.

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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...

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The rate constant of a chemical reaction increased from 0.100 s−1 to 3.10 s−1 upon raising the temperature from 25.0 ∘C to 55.0 ∘C .

Part A: Calculate the value of (1/T2−1/T1) where T1 is the initial temperature and T2 is the final temperature.

Part B: Calculate the value of ln(k1/k2) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.

Part C: What is the activation energy of the reaction?

Learning Goal:
To use the Arrhenius equation to calculate the
activation energy.
As temperature rises, the average kinetic energy of
molecules increases. In a chemical reaction, this
means that a higher percentage of the molecules
possess the required activation energy, and the
reaction goes faster. This relationship is shown by
the Arrhenius equation
k = Ae E./RT
where k is the rate constant, A is the frequency
factor, E is the activation energy, R = 8.3145
J/(K mol) is the gas constant, and T is the
Kelvin temperature. The following rearranged
version of the equation is also useful:
k1
In
E.
R
T2
where ki is the rate constant at temperature T1,
and k2 is the rate constant at temperature T2.

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