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−Ea/RT where k is the rate constant, A is the frequency factor, Ea 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: ln(k2k1)=(EaR)(1T1−1T2) where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2. The rate constant of a chemical reaction increased from 0.200 s−1 to 2.80 s−1 upon raising the temperature from 26.0 ∘C to 52.0 ∘C . Calculate the value of (1T1−1T2) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.
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−Ea/RT where k is the rate constant, A is the frequency factor, Ea 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: ln(k2k1)=(EaR)(1T1−1T2) where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2. The rate constant of a chemical reaction increased from 0.200 s−1 to 2.80 s−1 upon raising the temperature from 26.0 ∘C to 52.0 ∘C . Calculate the value of (1T1−1T2) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 49QRT
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To use the Arrhenius equation to calculate the activation energy.
As temperature rises, the average kinetic energy of molecules increases. In a
k=Ae−Ea/RT
where k is the rate constant, A is the frequency factor, Ea 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:
ln(k2k1)=(EaR)(1T1−1T2)
where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2.
The rate constant of a chemical reaction increased from 0.200 s−1 to 2.80 s−1 upon raising the temperature from 26.0 ∘C to 52.0 ∘C .
Calculate the value of (1T1−1T2) where T1 is the initial temperature and T2 is the final temperature.
Express your answer numerically.
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