Chemistry chapter 7: Mole concept and stoichiometry
mole
number of moles of gas
no. of particles
mass
calculated by taking the volume of gas in dm3 and dividing by 24dm3
calculated by taking the number of moles and multiplying 6.02x10^23, which is also known as Avogadro's constant
calculated by taking the number of moles and multiplying that number by the MOLAR MASS of the substance
relative atomic mass
average mass of one atom of that element relative to 1/12 the mass of an atom of carbon-12
relative molar mass
average mass of one MOLECULE of that substance relative to 1/12 the mass of an atom of carbon-12
relative formula mass
the relative formula mass of an IONIC compound is the average mass of ONE UNIT OF THAT COMPOUND relative to 1/12 the mass of an atom of carbon-12
percentage mass
can be calculated by taking the number of atoms of the element in the formula and multiplying the atomic mass of the element over the molar mass of the compound and multiply the whole thing by 100%
molar mass
one mol of a substance has a mass equal to its relative atomic mass, relative molecular or formula mass in grams, which is the molar mass of the substance
concentration of a solution
amount of solute dissolved in a unit volume of the solvent
concentration in mol/dm3
concentration in g/dm3
calculated by taking the mass of the solute in g and dividing it by the volume of the solvent in dm3
calculated by dividing the number of moles of solute and dividing it by the volume of solvent in dm3
the 2 types of concentrations are related by a formula
concentration in g/dm3 divided by molar mass of solute in g/mol is equal to the concentration of the same substance in mol/dm3