Part A The activation energy of a certain reaction is 38.9 kJ/mol . At 20 ∘C , the rate constant is 0.0130 s−1 . At what temperature would this reaction go twice as fast?
Part A The activation energy of a certain reaction is 38.9 kJ/mol . At 20 ∘C , the rate constant is 0.0130 s−1 . At what temperature would this reaction go twice as fast?
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 108CP: The decomposition of NO2(g) occurs by the following bimolecular elementary reaction:...
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Question
The Arrhenius Equation is typically written as
k=Ae−Ea/RT
However, the following more practical form of this equation also exists:
lnk2k1=EaR(1T1−1T2)
where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures ( T1 and T2 ).
Part A
The activation energy of a certain reaction is 38.9 kJ/mol . At 20 ∘C , the rate constant is 0.0130 s−1 . At what temperature would this reaction go twice as fast?
Express your answer numerically in degrees Celsius
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