Karteikarten
Amounts of Substances
Karten in diesem Stapel (21)
- 1Relative Atomic Mass (Ar)The average mass of an atom of an element, taking into account it's naturally occurring isotopes, relative to 1/12th the mass of carbon-12
- 2Relative Molecular Mass (Mr)The average mass of a molecule compared to 1/12th the mass of carbon-12
- 3Relative Formula Mass (Mr)The same as relative formula mass for ionic compounds as they do not exist as molecules
- 4Avogadro's Constant Na6.022 x 10^23
The number of atoms in 12g of carbon-12 - 5A Mole6.022 x 10^23 particles.
A substances formula mass weighed out in grams will contain one mole of that substance - 6Equation linking Moles, Mass and MrNo. Moles n = Mass m (g) / Mr of substance
- 7Equation linking Particles and MolesNo. Particles = Na x No. Moles n
- 8A SolutionA solvent with solute dissolved in it
- 9Equation linking Concentration, Moles, and VolumeConcentration C (moldm^-3) = No. moles n (mol) / Volume V (dm^3)
- 10The ideal gas equationPressure P (Pa) x Volume V (m^3) = no. moles n (mol) x gas const R (JK^-1mol^-1) x temperature T (K)
- 11Degrees Celcius to Kelvin+ 273
- 12KPa to pax 10^3
- 13cm^3 to dm^3x 10^-3
- 14dm^3 to m^3x 10^-3
- 15cm^3 to m^3x 10^-6
- 16m^3 to cm^3x 10^6
- 17m^3 to dm^3x 10^3
- 18dm^3 to cm^3x 10^3
- 19Empirical FormulaThe simplest ratio of atoms of each element in a compound
- 20Molecular FormulaThe actual ratio of atoms of each element in one molecule of the compound.
For ionic substances, actual ratio is the empirical formula. - 21State Symbols(s) - solid
(l) - liquid
(g) - gas
(aq) - aqueous
Informationen
- Beschreibung
- Definitions for Amounts of Substances module in AQA AS Chemistry
- Erstellt von
- Benjamin Rogers-Newsome
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- 17
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