1.2 Amount Of Substance
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Define Relative Molecular Mass
Average mass of the naturally occurring isotopes of a compound, compared to 1/12 the mass of a carbon-12 atom
Define Relative Atomic Mass
Average mass of the naturally occurring isotopes of an atom, compared to 1/12 the mass of an atom of carbon-12
Define the Avagadro constant
Number of particles / atoms in one mole of a substance
Write the equation that links mass of 1 mol, mass of one atom and Avagradros constant
Mass of 1 mol = Mass of one atom x Avagradros constant
Define percentage yield
The % of a product produced by a reaction, compared to a theoretical reaction
How would you calculate percentage yield
Mass of useful product / expected mass of useful product
What can the percentage yield of a practical be used to investigate
Efficiency of practical techniques and whether reactions proceed as estimated
Define atom economy
% of products made into a certain (useful) product
How would you calculate atom economy?
Mr of atoms of useful product / Mr of atoms of reactants
What can the atom economy of a reaction be used to investigate?
Efficiency of using a specific reaction to produce a product
Write the ideal gas equation (in symbols and in words with units)
PV = nRT Pressure x volume = number of moles x gas constant x temperature Pressure in Pa, Volume in m3, gas constant R = 8.31, Temperature in K
What are the standard conditions
25*C / 298K 1 atm / 100k Pa
How do you convert between K and C temperatures
C to K = +273 K to C = -273
Define empirical formula
Simplest whole number ratio of atoms in a compound
What is the equation that links mols, concentration and volume?
Moles = concentration x volume
What is the equation that links moles, mass and Mr?
Moles = Mass / Mr