Ideal Gas Law
Where:
= Pressure = Volume = Number of moles = Ideal gas constant = Temperature in Kelvin
Stoichiometry and Molecular Relationships
Conservation of Mass
Molar Mass
= Molar mass (g/mol) = Mass (g) = Number of moles
Molar Concentration (Molarity)
= Molarity (mol/L) = Number of moles = Volume of solution (L)
Mass Percentage
Chemical Equilibrium
Equilibrium Constant (
Where
Law of Mass Action (for gases):
= Equilibrium constant in terms of pressure = Change in the number of moles of gas
Thermochemistry
First Law of Thermodynamics
= Change in internal energy = Heat = Work done on or by the system
Reaction Enthalpy (
Gibbs Free Energy (
= Gibbs free energy = Change in enthalpy = Temperature = Change in entropy
Electrochemistry
Faraday’s Law
= Total charge (in coulombs) = Number of moles of electrons = Faraday’s constant (96485 C/mol)
Standard Cell Potential
Nernst Equation
= Cell potential = Gas constant = Temperature = Number of electrons transferred = Reaction quotient
Acids and Bases
Acid Dissociation Constant (
Ionic Product of Water
Relationship between pH and Proton Concentration
Relationship between pOH and Hydroxide Concentration
pH-pOH Relationship
Chemical Kinetics
Reaction Rate
For the equation
= Reaction rate = Rate constant , = Concentrations of reactants n$ = Partial orders of reaction with respect to each reactant
Arrhenius Equation
= Rate constant = Frequency factor = Activation energy = Gas constant = Temperature in Kelvin
Nuclear Chemistry Formulas
Radioactive Decay Law
= Number of nuclei that have not decayed at time = Initial number of nuclei = Decay constant