Chemistry Equilibrium and Reaction Kinetics

These flashcards cover key concepts related to chemical equilibrium, reaction kinetics, and the factors influencing chemical reactions.

Activation Energy

The minimum amount of energy required to initiate a chemical reaction.

Le Chatelier's Principle

When a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the change.

Equilibrium Constant (Keq)

A number that expresses the relationship between the concentrations of products and reactants at equilibrium in a reversible reaction.

Exothermic Reaction

A chemical reaction that releases energy in the form of heat.

Endothermic Reaction

A chemical reaction that absorbs energy in the form of heat.

Catalyst

A substance that increases the rate of a chemical reaction by lowering the activation energy.

Pressure Effect on Gases

Increasing pressure in a system with gaseous reactants or products favors the side of the reaction with fewer moles of gas.

Concentration Effect on Reaction Rates

Increasing concentration of reactants increases the rate of reaction due to more frequent collisions.

Temperature Effect on Reaction Rates

Increasing temperature generally increases reaction rates as it provides more energy for collisions.

Forward Reaction

The process in a reversible reaction where reactants are converted into products.

Reverse Reaction

The process in a reversible reaction where products are converted back into reactants.

Reversible Reaction

A reaction that can proceed in both the forward and reverse directions, reaching an equilibrium state.

KSP (Solubility Product Constant)

An equilibrium constant for a sparingly soluble compound, representing a saturated solution.

Decomposition Reaction

A chemical reaction where one compound breaks down into two or more simpler substances.

Collision Theory

A theory that states that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.

Equilibrium State

A condition in which the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products.