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4 cards from this section. Quick, good the night before a test.
Define activation energy.
Think about the energy barrier that reactants must overcome.
What is the Arrhenius equation used for?
This equation helps in understanding how temperature affects reaction rates.
What does the activation energy determine?
Think about the energy needed for reactants to interact successfully.
True or False: A catalyst is consumed in the reaction.
Consider how catalysts are used in reactions.
A chemical reaction had a measured rate constant of k at 298 K. If the temperature is increased to 308 K and the rate constant doubles, what can be inferred about the activation energy?
Consider how the Arrhenius equation illustrates the relationship between k and T.
If a certain catalyst reduces the activation energy from 100 kJ/mol to 60 kJ/mol, how would this impact the reaction rate at a fixed temperature?
Remember what a catalyst does to activation energy and how it influences molecular collisions.
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