The Mole and Gas Laws
The mole is chemistry's counting unit - like saying "a dozen" but for atoms and molecules. One mole always contains 6.02 × 10²³ particles (that's Avogadro's constant), whether you're counting atoms, ions, or molecules.
This massive number lets you convert between the microscopic world of atoms and the macroscopic world you can measure. The formula Number of particles = moles × Avogadro's constant is your key tool here.
For gases specifically, the ideal gas equation pV = nRT connects pressure, volume, temperature, and moles. Remember your units: pressure in Pa, volume in m³, temperature in Kelvin °C+273, and R = 8.31 J mol⁻¹ K⁻¹.
Concentration measures how much substance is dissolved per unit volume, typically in mol/dm³. This stays constant throughout a solution, making it perfect for calculations.
Memory Aid: Think of moles as chemistry's "packaging system" - it groups particles into manageable, countable units!