Chemical Equilibria

Flashcards covering key vocabulary and concepts related to chemical equilibria, Le Chatelier's principle, equilibrium constants, and industrial processes.

Reversible Reaction

A reaction where products can react to reform the original reactants, indicated by two opposing half arrows (=).

Dynamic Equilibrium

State where the rate of the forward reaction equals the rate of the backward reaction in a closed system, and the concentrations of reactants and products are constant.

Closed System

A system in which none of the reactants or products escape from the reaction mixture.

Open System

A system where matter and energy can be lost to the surroundings.

Position of Equilibrium

Refers to the relative amounts of products and reactants in an equilibrium mixture.

Le Chatelier's Principle

If a change is made to a system at dynamic equilibrium, the position of the equilibrium moves to minimize this change.

Equilibrium Expression

An expression that links the equilibrium constant, Kc, to the concentrations of reactants and products at equilibrium, taking stoichiometry into account.

Partial Pressure

The pressure that a gas would have if it was in the container all by itself in a mixture of gases.

Mole Fraction

The ratio of moles of a particular gas to the total number of moles of gas present in a mixture.

Equilibrium Constant (Kc)

Value that changes only if the temperature of the reaction changes. Solids are ignored.

Catalyst

A substance that increases the rate of a chemical reaction (speeds up both forward and reverse reactions equally) but has no effect on the position of equilibrium once it is reached.

Haber Process

Involves the synthesis of ammonia (N2(g) + 3H2(g) = 2NH3(g))

Contact Process

Synthesis of sulfuric acid (2SO2(g) + O2(g) = 2SO3(g))