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