The Mole

The quantity whose unit of the mole, used as a means of counting species such as atoms, ions and molecules

The amount of any substance containing as may elementary particles as there are carbon atoms in exactly 12 g of the carbon-12 isotope 6.02 x 10^23

The number of atoms per mole of the carbon-12 isotope

Moles= number of atoms/ avogadros constant

The mass per mole of a substance in units gmol^-1

Moles= mass in g/ molecular mass

The simplest whole number ratio of atoms of each element present in a compound

• Lay it out in a table and write masses or % mass • Find the moles of each element in the compound • Divide by the smallest moles • Then multiply or something to get all the numbers to be whole numbers

The chemical formula that gives the total number of atoms of each element in each molecule of a substance.

• Find empirical formula • Work out molecular mass of empirical formula • Compare to molecular mass given • See what multiple of it it is. Then multiply the numbers in the formula by this.

Contains no water molecules

A crystalline compound containing water molecules

Water molecules that are bonded into a crystalline structure of a compound

• Calculate moles of anhydrous solid left after heating • Calculate mass of water lost • Calculate moles of water lost • Divide moles of water by moles of anhydrous solid

Percentage error= total uncertainty/value measured * 100 If there are two measurements add the uncertaintities

The material which dissolves

The liquid it dissolves in

The resulting mixture formed from dissolving a solute in a solvent

The amount of solute, in moles, dissolved in 1 dm3 of solution

Moles= concentration (moldm-3) x volume (dm3)

• Do same equation as if you were calculating mol dm-3 2. But multiply the moles by the molecular mass and divide that by the volume.

Volume= moles x 24 at room temp and pressure

PV=nRT

Pressure- Pa Volume- m^3 Temperature- K Amount- Mole