One rule of thumb has been that a chemical reaction doubles in speed for every 10° increase in absolute temperature from room temperature (nominally 295 K). If this is strictly true, what is the activation energy of the chemical reaction?

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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One rule of thumb has been that a chemical reaction doubles in speed for every 10° increase in absolute
temperature from room temperature (nominally 295 K). If this is strictly true, what is the activation
energy of the chemical reaction?
Transcribed Image Text:One rule of thumb has been that a chemical reaction doubles in speed for every 10° increase in absolute temperature from room temperature (nominally 295 K). If this is strictly true, what is the activation energy of the chemical reaction?
Expert Solution
Step 1

The activation energy of a reaction can be determined by the Arrhenius equation. At two different temperatures, the Arrhenius equation can be written as:

lnk2k1=EaR×1T1-1T2          (1)

Here k1, and k2 are the rate constant at temperature T1, and T2 respectively. R is the ideal gas constant, and Ea is the activation energy of the reaction.

 

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