medium · MCAT chem-phys
A chemist observes that increasing the temperature of a reaction from 300 K to 310 K doubles the rate constant.
Which underlying principle best explains this observation?
- The reaction becomes significantly more exothermic at higher temperatures, driving the rate
- The activation energy required for the reaction gradually decreases as the temperature is increased
- A larger fraction of molecular collisions exceed the activation energy at higher temperatures.
- The increase in the frequency of molecular collisions alone fully accounts for the doubling of the rate
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