#1.43
Calculate relative formula mass given relative atomic masses
#1.44
Calculate the formulae of simple compounds from reacting masses or percentage composition and understand that these are empirical formulae
#1.45
Deduce:
a) the empirical formula of a compound from the formula of its molecule
b) the molecular formula of a compound from its empirical formula and its relative molecular mass
#1.46
Describe an experiment to determine the empirical formula of a simple compound such as magnesium oxide
#1.47
Explain the law of conservation of mass applied to:
a) a closed system including a precipitation reaction in a closed flask
b) a non-enclosed system including a reaction in an open flask that takes in or gives out a gas
#1.48
Calculate masses of reactants and products from balanced equations, given the mass of one substance
#1.49
Calculate the concentration of solutions in g dm-3
#1.50
Recall that one mole of particles of a substance is defined as:
a) the Avogadro constant number of particles (6.02 × 1023 atoms, molecules, formulae or ions) of that substance
b) a mass of 'relative particle mass' g
#1.51
Calculate the number of:
a) moles of particles of a substance in a given mass of that substance and vice versa
b) particles of a substance in a given number of moles of that substance and vice versa
c) particles of a substance in a given mass of that substance and vice versa
#1.52
Explain why, in a reaction, the mass of product formed is controlled by the mass of the reactant which is not in excess
#1.53
Deduce the stoichiometry of a reaction from the masses of the reactants and products