All Flashcards
What are the key differences between catalysts and intermediates?
Catalysts: Speed up the reaction but are not consumed; not part of the overall reaction. Intermediates: Formed and consumed during the reaction; not present in the overall reaction.
Difference between rate law derived from RDS and overall balanced equation?
Rate Law from RDS: Determined by the reactants in the rate-determining step; must be verified experimentally. Overall Balanced Equation: Represents the stoichiometry of the reaction; does not directly indicate the rate.
What is the effect of the rate-determining step on the overall reaction rate?
The rate-determining step limits the overall reaction rate; the reaction cannot proceed faster than its slowest step.
What is the effect of a catalyst on the activation energy of a reaction?
A catalyst lowers the activation energy of a reaction, thereby increasing the reaction rate.
What happens if the derived rate law from a mechanism does not match the experimental rate law?
The proposed mechanism is not valid and must be revised or discarded.
What is a reaction mechanism?
A detailed, step-by-step sequence of elementary reactions that collectively describe how a chemical reaction occurs.
What is an elementary step?
A single step in a reaction mechanism that represents one molecular event.
What is a catalyst?
A substance that speeds up a reaction without being consumed in the process.
What is an intermediate?
A species that is formed and consumed during the reaction but does not appear in the overall balanced equation.
What is the rate-determining step (RDS)?
The slowest step in a reaction mechanism that determines the overall rate of the reaction.
Define rate law.
An equation that expresses the rate of a reaction in terms of the concentrations of reactants.