CHEM 1C Lecture Notes - Lecture 2: Equilibrium Constant, Partial Pressure

• School: UC-Irvine
• Department: Chemistry
• Course: CHEM 1C

Document Summary

Irreversible: 100 reactant/0 product " 0 reactant/100 product. The equilibrium constant (k): defined as a ratio (at equilibrium) where the concentration of products is raised to the concentration of reactants. If you see an equilibrium constant of 1 then the ratio between reactants and products is 50/50. If you see an equilibrium constant less than 1 then the ration between reactants and products is that reactants are greater than products. If you see an equilibrium constant of greater than 1 then the ratio between reactants and products is that products are greater than reactants. K describes the equilibrium composition of the rxn mixture. At a given temperature, k is constant. Homogeneous equilibria: where the reactants and products are all of the same phase. Heterogeneous equilibria: involves pure solids pure liquids or solvents as reactants or products, the pure solid, liquid, or solvent is not included in the equilibrium expression. We can only include gaseous and aqueous solutions.