Chapter 14 Learning Objectives

What is kinetics?

• Kinetics is the study of the change in the concentrations of reactants and products over a period of time; how fast a reaction occurs.

What happens to the amount of reactants as a reaction progresses? What happens to the amount of products as a reaction progresses?

• The amount of reactants decreases as the reaction progresses, while the amount of products increases until equilibrium is reached.

What is collision theory? What three conditions must be met in order for a reaction to occur?

• Collision theory is

• Reacting particles must collide

• Reactants must collide in the proper orientation (line up in a specific way)

• Reactants must have sufficient energy.

• Will result in effective collision.

What is the effect of increasing concentration of a reactant on reaction rate? Why and HOW does concentration have this effect on reaction rate? (Make sure you can connect concentration to rate via collision)

What is the effect of increasing the surface area of a solid reactant on reaction rate? Why and HOW does surface area have this effect on reaction rate? (Make sure you can connect surface area to rate via collision theory)

What is activation energy? How can you use an energy diagram to calculate it?

If the activation energy of a reaction is increased, how will the rate of the reaction be affected?If the activation energy of a reaction is decreased, how will the rate of the reaction be affected?

What is the effect of adding a catalyst on the rate of a reaction? How do catalysts cause this effect on the rate of a reaction?

What is reaction rate?

You should be able to describe how reaction rates change over time (do they increase or decrease?). You should also be able to use collision theory to explain why reaction rates change the way they do.

If I give you a balanced equation, you should be able to represent the rate in terms of either a reactant or a product. You should also be able to relate the rate of disappearance of a reactant to rate of appearance of a product (both symbolically and computationally). You should also be
able to relate the rate of reaction to the rate of disappearance of a reactant or to the rate of disappearance of a product.

• If I give you a balanced chemical equation and the rate at which, for example, a reactant disappears (or a way to calculate that rate), you should be able to calculate the rate at which another reactant or product in the same chemical equation changes.

• You should be able to calculate the rate of reaction from the rate at which a reactant disappears (or the rate at which a product appears).

What is a rate law?

You should be able to look at a rate law and determine the order with respect to each reactant, as well as the overall reaction order.

How is rate related to concentration for a zero order reaction? (In other words, if I double/triple/etc. the concentration of a zero order reaction, what will happen to the rate of that reaction?) For a first order reaction? For a second order reaction?

If I give you an initial rate and a rate law, you should be able to determine a final rate when the concentrations of reactants are changed.

If I give you a set of data with concentrations and initial rates for a series of experiments, you should be able to determine the rate law for the reaction. Make sure you know how to determine the rate law if one of the reactant concentrations is not constant from one experiment to another. You should also be able to calculate k for that reaction (with the correct units!).

How do the units of k relate to reaction order?

I will provide you with zero order, first order, and second order integrated rate laws on the test.

• You should be able to use the integrated rate laws to solve for any one of the variables (given the others or a way to find the others).

• You should be able to use percentages (either percentage of reactant remaining or percentage of reactant consumed / used) in integrated rate laws.

• You should be able to graphically determine the order of a reaction.

• You should be able to graphically determine k and [A]0 (this will be different for zero order, first order, and second order reactions...you should be able to determine this information from the integrated rate laws).

What is half-life?

I will provide you with the half-life equations for zero order, first order, and second order reactions.

• You should be able to use half-life equations to solve for a rate constant (and vice versa). [Note: that rate constant will often be plugged into or come from an integrated rate law!]

How does increasing temperature affect the value of a rate constant?

I will provide you with the Arrhenius equation. You should be able to solve it for any of the variables when given the others