All Flashcards
What are the differences between a catalyst and an intermediate?
Catalyst: Speeds up the reaction, is not consumed. | Intermediate: Formed and consumed during the reaction.
What are the differences between elementary step and overall reaction?
Elementary Step: Individual step in a mechanism. | Overall Reaction: Net reaction after all elementary steps are combined.
What is the effect of a catalyst on the activation energy?
A catalyst lowers the activation energy of a reaction.
What happens if the rate-determining step includes an intermediate?
You'll need to use equilibrium concepts to substitute the intermediate out of the rate law.
What happens if you increase the concentration of a reactant in the rate-determining step?
The overall rate of the reaction will increase.
How do you determine the overall reaction from a mechanism?
Add all the elementary steps together and cancel out any species that appear on both sides of the equation (intermediates and catalysts).
How to determine the rate law from a reaction mechanism?
Identify the rate-determining step. The rate law for the overall reaction is the same as the rate law for the rate-determining step, based on its stoichiometry.
What is the first step to solve a mechanism problem?
Identify the rate-determining step.