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3 cards from this section. Quick, good the night before a test.
Define activation energy.
Think about the energy barrier that needs to be overcome.
What happens if the activation energy is high?
Consider how it relates to the energy needed for molecules to react.
What is activation energy?
Think of it as the energy barrier that needs to be crossed for a reaction to occur.
True or False: A lower activation energy leads to slower reaction rates.
Consider how the energy of molecules impacts movement and reaction rates.
If the activation energy for a particular reaction is 75 kJ/mol at 298 K, how would a temperature increase from 298 K to 308 K affect the rate constant, assuming it follows the Arrhenius equation? Use values where relevant.
Use R = 8.314 J/mol·K for calculations.
A reaction without a catalyst has an activation energy of 100 kJ/mol, while a catalyzed pathway requires only 50 kJ/mol. Compare the expected rates of these two reactions at 298 K.
Considering how much more accessible the catalyzed pathway makes the reaction is key!
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