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About This Unit
In this unit, we will study chemical equilibrium, which occurs when a reversible reaction continues in both directions, but the forward and reverse reactions happen at the same rate. At equilibrium, the reaction has not stopped. Instead, the amounts of reactants and products stay constant because both processes are balanced.
We will learn how equilibrium systems respond when conditions change. Changes in concentration, temperature, pressure, or volume can disturb the balance between the forward and reverse reactions. Le Châtelier’s principle helps us predict how the system will shift to reduce the effect of the change.
A major focus of this unit is using equilibrium constants, K, and reaction quotients, Q, to describe and predict the composition of a mixture. You will learn how to decide whether a reaction will shift toward products or reactants, and how equilibrium ideas can be used to increase product yield.
We will also connect equilibrium to real-world examples, such as why pure oxygen can help treat carbon monoxide poisoning and what affects how much of a salt dissolves in water. Dissolving is also a reversible process, so solubility can be explained using equilibrium ideas.
On the AP Chemistry Exam students are expected to use data, calculations, graphs, and particle-level reasoning to support claims about equilibrium systems. Strong answers should connect the direction of a shift, the value of K or Q, and the particle-level changes happening in the system.
Essential Questions
- What does it mean for a chemical reaction to be at dynamic equilibrium?
- How are the rates of the forward and reverse reactions related at equilibrium?
- How can we predict whether a reversible reaction will shift toward reactants or products?
- How can the equilibrium constant, K, be used to describe the composition of a mixture at equilibrium?
- How can the reaction quotient, Q, be used to predict the direction a reaction will proceed?
- How can changes in concentration, temperature, pressure, or volume affect an equilibrium system?
- How can Le Châtelier’s principle help us manipulate a system to increase product yield?
- Why can pure oxygen help treat carbon monoxide poisoning?
- How can equilibrium ideas explain what factors affect how much of a salt dissolves?
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