AP Chem unit 7

Dynamic Equilibrium

Condition where the rate of the forward reaction equals that of the backward reaction.

Equilibrium Constant (K)

A value that expresses the relationship between concentrations/partial pressures of reactants and products at equilibrium.

Dynamic Equilibrium

Condition where the rate of the forward reaction equals that of the backward reaction.

Equilibrium Constant (K)

A value that expresses the relationship between concentrations/partial pressures of reactants and products at equilibrium.

Q

Indicates the extent to which a reaction has proceeded; compares reaction quotient with K to determine the direction shift.

Q > K

Indicates there are too many products, causing the reaction to shift to the left (towards reactants).

Q < K

Indicates there are too many reactants, causing the reaction to shift to the right (towards products).

Le Châtelier’s Principle

Explains how a system at equilibrium responds to changes in concentration, temperature, volume/pressure, or dilution.

Ksp

The equilibrium constant for the dissolution of an ionic solid.

Qsp > Ksp

Indicates that a precipitate will form.

Qsp < Ksp

Indicates that no precipitate is formed.

Temperature Increase Effect on Equilibrium

Shifts the reaction towards the endothermic direction.

Temperature Decrease Effect on Equilibrium

Shifts the reaction towards the exothermic direction.

Reciprocal Relationship of K

When reversing a reaction, K becomes the reciprocal of the original K.

Coefficient Multiplication Effect on K

If coefficients of a reaction are multiplied, K is raised to that power.