A common rule-of-thumb for many chemical reactions states that, at normal conditions, the reaction rate doubles for each increase of 10°C. Assuming a "normal" temperature of 20°C, estimate the activation energy of a "typical" chemical reaction. If we select 20°C as the reference temperature, what is a "typical" dimensionless activation energy?
A common rule-of-thumb for many chemical reactions states that, at normal conditions, the reaction rate doubles for each increase of 10°C. Assuming a "normal" temperature of 20°C, estimate the activation energy of a "typical" chemical reaction. If we select 20°C as the reference temperature, what is a "typical" dimensionless activation energy?
Chapter8: Sampling, Standardization, And Calibration
Section: Chapter Questions
Problem 8.19QAP
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