3.2 Stoichiometry

The average mass of the isotopes of an element compared to 1/12 the mass of an atom of carbon - 12

The sum of the relative atomic masses in a molecule Mr

The sum of relative atomic masses in ionic compounds

6.02x10^23 NA

The greater the amount of solute in a given volume(solvent) the greater the concentration

c=n/v g/dm3 (G/dm3=mol/dm3 x MR

One mole of any gas occupies a volume of 24 dm3

A substance formed by the union of two or more elements.

No atoms are lost or made in a chemical reaction, the atoms join together in different ways to form products

Actual yield/theoretical yield x 100

The simplest whole number ratio of the different atoms or ions in a compound

Actual number for each type of atom in a compound Number and type of different atoms in one molecule

(Atomic mass x number of mols of particular element in a compound)/molar mass of a compound x 100

Amount of solute dissolved in a solvent to make 1 dm3 of solution, the greater the amount of solute in a given volume, the greater the concentration.

Mol/dm3

Divide by 1000

1 atm

V=n x 24

m=n x M

g/mol

Calculate the molar mass of the empirical formula Relative molecular mass is divided by your answer Multiply each elemnt in the empirical formula to get the answer

Change % into grams Find number of mols Divide each of the mols by the smallest number of mols Times by the same whole numbers if you dont end up with whole numbers

When the product is produced in excess

Limits amount of product formed