L25 - Equilibrium

FThe concept of reaction equilibrium The equilibrium constant Equilibrium constant for liquids, solid and gases

Equilibrium

The study of how chemical reactions lead to a balance between reactants and products.

Reaction to Completion

The reactants are converted into products.

Dynamic Equilibrium

A dynamic condition where the rate of the forward reaction equals the rate of the reverse reaction.

Forward Reaction (NO2 to N2O4 Example)

The reaction that converts NO2 into N2O4.

Reverse Reaction (NO2 to N2O4 Example)

The reaction that converts N2O4 into NO2.

Equilibrium State

A state where there is no further change in concentrations of reactants and products.

Equilibrium Constant (K)

At a given temperature, a chemical system reaches a state in which a particular ratio of reactants and product concentrations has a constant value.

Ratio of Concentrations

Product concentrations all multiplied together, divided by the reactant concentrations all multiplied together.

Equilibrium Constant Greater Than One

If the reaction favors the products, then the equilibrium constant will be bigger than one.

Equilibrium Constant Less Than One

If there are more reactants than products at equilibrium, then the equilibrium constant will be less than one.

Doubled Coefficients Effect

If you double the coefficients, you square the equilibrium constant.

Swapped Equation Order Effect

If you swap the way you write the equation, it just means that the value for that equilibrium constant is one over.

Equilibrium Constant for Stepwise Reactions

The equilibrium constant for the overall reaction is just the product of the equilibrium constants for the stepwise reactions.