AP Chemistry Unit 7: Equilibrium

TLDR

• Equilibrium means forward and reverse reactions occur at equal rates.

• Use equilibrium constants (K, Kc, Kp) to determine product vs reactant favorability.

• Compare Q vs K to predict reaction direction.

• Apply ICE tables to calculate equilibrium concentrations.

• Use Le Chatelier’s Principle to explain how systems respond to stress.

Why This Unit Matters

Equilibrium is one of the most heavily tested and conceptually important units in AP Chemistry. It shows up everywhere — from gases and solubility to acids, bases, and thermodynamics.

The AP exam does not reward memorizing rules like “shift left” or “shift right.” It rewards students who can explain why a system shifts, using equilibrium logic, Q vs K comparisons, and particle-level reasoning.

If you master this unit, Units 8 and 9 become significantly easier.

1. What Chemical Equilibrium Really Means

A system is at equilibrium when the rate of the forward reaction equals the rate of the reverse reaction.

Key points:

• Concentrations remain constant, but reactions continue.

• Equilibrium does not mean equal amounts of reactants and products.

• Equilibrium can only occur in a closed system.

Dynamic equilibrium is a favorite AP concept question.

2. Equilibrium Constants (K)

For a general reaction:
aA + bB ⇌ cC + dD

The equilibrium constant is written as:
K = ([C]ᶜ[D]ᵈ) / ([A]ᵃ[B]ᵇ)

Rules to remember:

• Include only gases and aqueous species.

• Exclude solids and pure liquids.

• Exponents come from coefficients in the balanced equation.

Types of equilibrium constants:

• Kc: based on molar concentrations.

• Kp: based on partial pressures of gases.

3. Relationship Between Kc and Kp

For gaseous reactions:
Kp = Kc(RT)^(Δn)

Where:

• Δn = moles of gaseous products − moles of gaseous reactants

• R = 0.0821 L·atm·mol⁻¹·K⁻¹

• T must be in Kelvin

This relationship is commonly tested in calculation-based questions.

4. Reaction Quotient (Q)

Q has the same form as K but uses current concentrations instead of equilibrium values.

How to interpret:

• Q < K → reaction shifts forward

• Q > K → reaction shifts backward

• Q = K → system is already at equilibrium

Mnemonic: Q chases K.

This comparison often appears before ICE-table calculations.

5. Magnitude of K

The size of K tells you about reaction favorability.

• K ≫ 1 → product-favored

• K ≈ 1 → significant amounts of both

• K ≪ 1 → reactant-favored

Important clarification:
A large K does not mean the reaction is fast. Rate is a kinetics concept, not equilibrium.

6. ICE Tables

ICE tables are used to calculate equilibrium concentrations.

Steps:

• I: write initial concentrations

• C: express change using x

• E: write equilibrium concentrations

Plug equilibrium values into the K expression and solve for x.

AP shortcut:
If K is very large or very small, x is often negligible. Always justify this assumption if used.

7. Le Chatelier’s Principle

When a system at equilibrium is disturbed, it shifts to counteract the disturbance.

Concentration Changes

• Adding reactant shifts equilibrium toward products.

• Adding product shifts equilibrium toward reactants.

Pressure and Volume (Gases)

• Decreasing volume (increasing pressure) shifts toward fewer gas moles.

• Increasing volume shifts toward more gas moles.

Temperature

Treat heat as a reactant or product.

• Exothermic reaction: heat is a product.

• Endothermic reaction: heat is a reactant.

Changing temperature is the only stress that changes the value of K.

Catalysts

• Do not shift equilibrium.

• Only speed up the time needed to reach equilibrium.

8. Manipulating Equilibrium Expressions

Equilibrium constants change predictably when reactions are modified.

• Reverse reaction → K becomes 1/K

• Multiply coefficients by n → Kⁿ

• Add reactions → multiply K values

These relationships are commonly tested in multi-step problems.

9. Equilibrium and Thermodynamics

Equilibrium connects directly to free energy.

Key relationship:
ΔG° = −RT ln K

Interpretation:

• Large K → negative ΔG° → spontaneous forward reaction

• Small K → positive ΔG° → nonspontaneous forward reaction

At equilibrium, ΔG = 0.

Common Pitfalls

• Including solids or liquids in K expressions.

• Confusing reaction speed with K magnitude.

• Forgetting to adjust K when equations are reversed or scaled.

• Applying Le Chatelier without considering gas mole count.

• Treating catalysts as equilibrium shifters.

Tutor Tip

On AP free-response questions, never say “it shifts left” without explanation.

Strong answer example:
“Adding reactant increases Q, making Q < K, so the system shifts forward to restore equilibrium.”

That reasoning language is exactly what AP graders look for.

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