12_Unit_3_Equilibrium_ppt_2

Reversible Reactions

Reactions that do not go to completion, resulting in a mixture of reactants and products at equilibrium.

Equilibrium

A state where the forward and reverse reactions occur at the same rate.

Endergonic Reaction

A non-spontaneous reaction that absorbs energy.

Exergonic Reaction

A spontaneous reaction that releases free energy.

Entropy

A measure of the disorder of a system; higher disorder increases the chance of a reaction.

Enthalpy

The total energy stored in a substance, represented by the symbol H.

Activation Energy

The minimum energy required for colliding particles to react.

Catalyst

A substance that increases the rate of a chemical reaction without being consumed.

LeChatelier’s Principle

If a stress is applied to a system at equilibrium, the system will adjust to relieve the stress.

Collision Theory

Atoms, ions, and molecules form chemical bonds when they collide with sufficient kinetic energy.

Law of Disorder

Matter tends to move towards maximum disorder.

Equilibrium Position

The state of a reaction at equilibrium affected by concentration, temperature, and pressure.

Heterogenous Equilibrium

Equilibrium involving reactants and products in different phases.

Chemical Equilibrium

A dynamic state where the concentrations of the reactants and products remain constant.

Equilibrium Constant (K)

A dimensionless quantity that indicates the position of equilibrium for a reaction.

Reaction Quotient (Q)

A ratio that compares the concentrations of products and reactants at any point in time.

Pressure Effects on Equilibrium

Increasing or decreasing pressure shifts the equilibrium toward the side with fewer or more molecules, respectively.

Temperature Effects on Equilibrium

Increasing temperature shifts equilibrium in the endothermic direction, while decreasing it shifts towards the exothermic direction.

Changes in Concentration Effect

Adding reactants shifts equilibrium toward products, while adding products shifts it toward reactants.

Adding or Removing a Catalyst

A catalyst does not shift equilibrium or change K, but it allows the system to reach equilibrium more quickly.

Calculating Equilibrium Constant Expression

K is calculated using the concentrations of products over reactants, omitting solids and pure liquids.