Ch4 Amount of substances- mols in solids and gases Flashcards
Relative atomic mass
Weighted mean mass of an atom of an element compared with 1/12 the mass of an atom of Carbon-12
Relative isotopic mass
Mass of an atom of an isotope of the element compared with 1/12 the mass of an atom of carbon-12
Relative molecular mass
Weighted mean mass of a molecule compared with 1/12 the mass of an atom of carbon-12
Relative formula mass
weighted mean mass of a formula unit of the compound compared with 1/12 the mass of an atom of carbon-12
One mole
amount of substance that contains as many elementary particles as there are atoms in 12g of carbon-12
Avogadro constant
6.02 x 10^23
Number of particles present in 1 mol of any substance
Molar mass
mass of one mol of a substance
Mole formula
n = m/Mr
Empirical formula
Simplest whole number ratio of atoms of the elements in a compound
Water crystillisation
water present in hydrated salts
Hydrated compound
contains water as part of its structure
Anhydrous compound
hydrated compound after its lost its water of crystillisation
Avogadro’s law
equal volumes of gases measured at the same temperature and pressure will contain the same number of molecules
Molar volume
At room temperature and pressure, 1 mol pf gas occupies 24dm^3
Ideal gas equation
PV = nRT
P- in pascals
V- in m^3
T- kelvin
