Topic 3 – Quantitative Chemistry Flashcards
Actual yield
The amount of product actually produced by a reaction.
Atom economy
The measure of the amount of starting materials that end up as useful
products.
Avogadro constant
The number of atoms, molecules or ions in a mole of a given
substance.
Avogadro’s law
Equal amounts in moles of gases occupy the same volume under the
same conditions of temperature and pressure.
Concentration
The amount of substance (e.g. the mass) in a certain volume of a solution.
Conservation of mass
The law of conservation of mass states that no atoms are lost or
made during a chemical reaction so the mass of the products equals the mass of the
reactants.
Limiting reactant
The reactant that is completely used up since it limits the amount of
products formed.
Mole
Chemical amounts are measured in moles. The mole is the unit for amount of
substance. The symbol for the unit mole is mol.
Percentage by mass
A value representing the concentration of an element in a compound
or a component in a mixture. It is calculated by the mass of a component divided by the total
mass of the mixture, multiplied by 100.
Percentage yield
The percentage ratio of the actual yield of product from a reaction
compared with the theoretical yield.
Relative formula mass
The sum of the relative atomic masses of the atoms in the numbers
shown in the formula. It is numerically equal to the mass of one mole of a substance in
grams.
Theoretical yield
The maximum amount of product that could be produced from the given
reactants, assuming a complete reaction takes place.
Thermal decomposition
The reaction that occurs when heat is applied to a compound
causing it to break down into its different chemical constituents.
Uncertainty
All measurements have a degree of uncertainty regardless of precision and
accuracy. Uncertainty can be due to the limitations of the measuring equipment or due to the
skill of the experimenter carrying out the measurements
