Chem Final Equations

Avogradro’s Number (Constants)

NA​=6.022×1023 mol−1

Gas constant (Constants)

R = 0.08206 L atm / mol K R = 8.314 J / mol K

Faraday Constant (Constants)

F = 96,485 C /mol e

Temperature conversion (Constants)

0°C = 273.15 K

Pressure conversion (Constants)

Pressure conversion (Constants)

1 atm = 760 Torr = 760 mmH

Heat (phase change) calendar (Heat/Energy)

• q=nΔHfus​

• q=mΔHfus

• q=nΔHvap

• q=mΔHvap

Heat (temperature change) (Heat/Energy)

q = mCΔT

Molarity (Solutions & Concentration)

M = mol solute/L solution

Molality (Solutions & Concentration)

M = mol solute/kg solvent

Mole fraction (Solutions & Concentration)

Xa = mol A / total moles

Mass percent (Solutions & Concentration)

% mass = Mass solute (or solvent)/ Total mass x 100

Freezing point depression (Boiling & Freezing Point Changes)

ΔTf=imKf

Boiling Point Elevation (Boiling & Freezing Point Changes)

ΔTb=imKb

New freezing temp (Boiling & Freezing Point Changes)

Tf=Tf∘−ΔTf

Osmotic Pressure

Π=iMRT

General rate expression (Reaction Rates)

Rate Law (Reaction Rates)

Comparing rate experiments (Reaction Rates)

Zero Order (Integrated Rate Laws)

First order (Integrated Rate Laws)

Second Order (Integrated Rate Laws)

Arrhenius Equation

Log Rules

Equilibrium constant (Equilibrium)

Gas equilibrium (Equilibrium)

Relationship (Equilibrium)

Water equilibrium

Acid Constant (Acid–Base Equations)

Base Constant (Acid–Base Equations)

pKa / pKb (Acid–Base Equations)

• pKa=−log⁡Ka

• pKb=−log⁡Kb

pH / pOH (Acid–Base Equations)

Relationships (Acid–Base Equations)

Henderson–Hasselbalch

Weak acid/base shortcut

When x is small

Free energy (Thermodynamics)

ΔG=ΔH−TΔS

Standard free energy (Thermodynamics)

Nonstandard (Thermodynamics)

Phase equilibrium temp (Thermodynamics)

T=ΔH/ΔS

Cell Potential (Electrochemistry)

Free energy relationship (Electrochemistry)

Nernst Equation (Electrochemistry)

Equilibrium relationship (Electrochemistry)

Alternate equilibrium form (Electrochemistry)