pointless waste of time
Topic 1.2
AMOUNT OF SUBSTANCE
The mole
Reacting masses and atom economy
Solutions and titrations
The ideal gas equation
Empirical and molecular formulae
Ionic equations
Mill Hill County High School
THE MOLE
Since atoms are so small, any sensible laboratory quantity of substance must contain a huge number of atoms:
1 litre of water contains 3.3 x 1025 molecules.
1 gram of magnesium contains 2.5 x 1022 atoms.
100 cm3 of oxygen contains 2.5 x 1021molecules.
Such numbers are not convenient to work with, so it is necessary to find a unit of "amount" which corresponds better to the sort of quantities of substance normally being measured. The unit chosen for this purpose is the mole. The number is chosen so that 1 mole of a substance corresponds to its relative atomic/molecular/formula mass measured in grams. A mole is thus defined as follows:
A mole of a substance is the amount of that substance that contains the same number of elementary particles as there are carbon atoms in 12.00000 grams of carbon-12.
One mole of carbon-12 has a mass of 12.0g.
One mole of hydrogen atoms has a mass of 1.0g.
One mole of hydrogen molecules has a mass of 2.0g.
One mole of sodium chloride has a mass of 58.5g.
The number of particles in one mole of a substance is 6.02 x 1023. This is known as Avogadro's number, L.
Thus when we need to know the number of particles of a substance, we usually count the number of moles. It is much easier than counting the number of particles.
The number of particles can be calculated by multiplying the number of moles by Avogadro’s number. The number of moles can be calculated by dividing the number of particles by Avogadro’s number.
(Number of particles) = (number of moles) x L
The mass of one mole of a substance is known as its molar mass, and has units of gmol-1. It must be distinguished from relative atomic/molecular/formula mass, which is
AMOUNT OF SUBSTANCE
The mole
Reacting masses and atom economy
Solutions and titrations
The ideal gas equation
Empirical and molecular formulae
Ionic equations
Mill Hill County High School
THE MOLE
Since atoms are so small, any sensible laboratory quantity of substance must contain a huge number of atoms:
1 litre of water contains 3.3 x 1025 molecules.
1 gram of magnesium contains 2.5 x 1022 atoms.
100 cm3 of oxygen contains 2.5 x 1021molecules.
Such numbers are not convenient to work with, so it is necessary to find a unit of "amount" which corresponds better to the sort of quantities of substance normally being measured. The unit chosen for this purpose is the mole. The number is chosen so that 1 mole of a substance corresponds to its relative atomic/molecular/formula mass measured in grams. A mole is thus defined as follows:
A mole of a substance is the amount of that substance that contains the same number of elementary particles as there are carbon atoms in 12.00000 grams of carbon-12.
One mole of carbon-12 has a mass of 12.0g.
One mole of hydrogen atoms has a mass of 1.0g.
One mole of hydrogen molecules has a mass of 2.0g.
One mole of sodium chloride has a mass of 58.5g.
The number of particles in one mole of a substance is 6.02 x 1023. This is known as Avogadro's number, L.
Thus when we need to know the number of particles of a substance, we usually count the number of moles. It is much easier than counting the number of particles.
The number of particles can be calculated by multiplying the number of moles by Avogadro’s number. The number of moles can be calculated by dividing the number of particles by Avogadro’s number.
(Number of particles) = (number of moles) x L
The mass of one mole of a substance is known as its molar mass, and has units of gmol-1. It must be distinguished from relative atomic/molecular/formula mass, which is