Equilibrium Concepts

Vocabulary

equilibrium

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

equilibrium constant (Kc)

for a chemical system at equilibrium at a certain temperature, the product concentrations multiplied together divided by the reactant concentrations multiplied together, with each term raised to the power of its coefficient in the balanced equation

Haber-Bosch process

process that breaks down the nitrogen-nitrogen bonds in N2 and converts nitrogen into ammonia (NH3)

law of mass action

chemical law that states when a reaction reaches equilibrium, the product concentrations multiplied together divided by the reactant concentrations multiplied together, with each term raised to the power of its coefficient in the balanced equation, is a constant

Le Chatelier's principle

principle that states that a change in the temperature, pressure, or concentration of a component will cause the equilibrium condition of a chemical system to change in a way that reduces the change

reaction quotient (Q)

ratio that can be used to predict how a system not in equilibrium will change to reach equilibrium

reversible reaction

reaction in which the products of the reaction can also react to produce the reactants at a nonnegligible rate