CHEM101 Lecture Notes - Solubility Equilibrium, Phase Rule, Calcium Sulfate
Document Summary
A chemical system is said to be in equilibrium when the forward and reverse reaction rates are equal, and there is no overall change in the concentration of reactants or products over time. In other words, the reactant and product concentrations are constant and the system is in balance. There are different types of equilibrium, including: chemical equilibrium: this occurs when the forward and reverse reactions of a chemical reaction are balanced, resulting in a constant concentration of reactants and products. An example of a chemical equilibrium is the haber process, which produces ammonia from nitrogen and hydrogen. N2 + 3h2 2nh3: phase equilibrium: this occurs when two or more phases of a substance are present in a system and are in equilibrium with each other. An example of phase equilibrium is the equilibrium between ice and water at 0 c.
