Chemical Reaction Kinetics Concepts

Jeremy Krug reviews AP Chemistry Unit 5, focusing on Chemical Kinetics. The video covers factors affecting reaction rates, rate laws, reaction orders, and graphical methods for determining reaction order. It also explains integrated rate laws, half-life, multistep reactions, collision theory, activation energy, energy profiles, and the Arrhenius equation. The role of catalysts in reaction mechanisms is discussed, concluding with a preview of Unit 6 on Thermodynamics.

Which of the following factors does NOT affect the rate of a chemical reaction?

• Concentration of reactants

• Presence of a catalyst

• Temperature

• Color of reactants

In the reaction 2 NO + O2 → 2 NO2, how does the rate of disappearance of O2 compare to that of NO?

• It is twice as fast

• It is half as fast

• It is three times as fast

• It is the same

What is the overall order of a reaction with a rate law: Rate = k[ClO2]^2[OH-]^1?

• First order

• Second order

• Third order

• Fourth order

Which graph indicates a first-order reaction when plotting concentration data?

• Natural log of concentration vs. time

• Rate vs. concentration

• Concentration vs. time

• Reciprocal of concentration vs. time

For a first-order reaction, how is the half-life related to the rate constant?

• Half-life is equal to the rate constant

• Half-life is inversely proportional to the rate constant

• Half-life is independent of the rate constant

• Half-life is directly proportional to the rate constant

In a multistep reaction, what is the role of the slowest step?

• It is the last step

• It does not affect the reaction rate

• It is the fastest step

• It determines the overall reaction rate

What is a reaction intermediate?

• A molecule that speeds up the reaction

• A molecule that is consumed in the reaction

• A molecule that appears in the final products

• A temporary molecule formed during the reaction

How does a catalyst affect a chemical reaction?

• It decreases the activation energy

• It slows down the reaction

• It changes the reaction products

• It increases the activation energy

What is the role of a surface catalyst?

• It reacts with the products

• It forms a bond with the reactants

• It increases the temperature

• It changes the color of the reactants

In an energy profile of a multistep reaction, what does the highest peak represent?

• The fastest step

• The slowest step

• The final product

• The initial reactant