Effect of Temperature on Rate of Reaction and Chemical Equilibrium

These flashcards cover key concepts related to the effect of temperature on reaction rates, collision theory, chemical equilibrium, and related reactions and constants.

Rate of Reaction

The speed at which reactants are converted into products in a chemical reaction.

Collision Theory

A theory stating that for a reaction to occur, reactants must collide with sufficient energy and the correct orientation.

Energy of Activation (Ea)

The minimum energy required for a chemical reaction to occur.

Exothermic Reaction

A reaction that releases energy, usually in the form of heat.

Endothermic Reaction

A reaction that absorbs energy from its surroundings.

Arrhenius Equation

An equation that relates the rate constant of a reaction to temperature and activation energy.

Frequency Factor (A)

A constant that represents the frequency of collisions in a chemical reaction.

Chemical Equilibrium

A state in which the rates of the forward and reverse reactions are equal.

Law of Mass Action

The principle stating that at equilibrium, the ratio of the concentrations of products to reactants remains constant.

Reaction Quotient (Q)

A measure of the relative amounts of products and reactants present during a reaction at any point in time.

Le Chatelier's Principle

A principle stating that if a dynamic equilibrium is disturbed, the system will adjust to counteract the disturbance.

Catalyst

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

Inhibitor

A substance that decreases the rate of a chemical reaction by raising the activation energy.

Elementary Reaction

A single step reaction that occurs as part of a larger reaction mechanism.

Intermediate

A substance formed during the middle steps of a reaction but not present in the final products.

Rate-determining Step

The slowest step in a reaction mechanism that determines the overall rate of the reaction.

Equilibrium Constant (K)

A number that expresses the relationship between the concentrations of products and reactants at equilibrium.

Ionization Constant (K)

A measure of the extent of ionization of a weak acid or weak base in solution.

Electrolytes

Substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity.