Amount of Substance - Chapter 2

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  • Created by: 12BurtD
  • Created on: 16-03-18 18:33
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  • Amount of Substance
    • Relative Atomic Mass
      • Ar
        • The average mass of an atom of an element (including isotopes) relative to 1/12 the Ar of Carbon-12
    • Relative Molecular Mass
      • Mr
        • The mass of a molecule compared to 1/12 the Ar of Carbon-12
      • Relative Formula Mass
        • Used for ions since they don't exist as Molecules
    • Avogadro Constant
      • The number of atoms in 12g of Carbon-12
      • The Mole
        • The amount of a substance that contains Avogadro number of particles
        • Equations
          • n = m / Mr
            • m - g         n - mol
          • n = cV
            • n = cV / 1000
              • c - mol dm^-3     V - cm^3
            • c - mol dm^-3    V - dm^3
          • PV = nRT
            • P - Pa             V - m^3           n - mol            R - 8.31     T - K
        • Gas Laws
          • Boyle's
            • PV = constant
          • Charles'
            • V/T = constant
          • Gay-Lussac's
            • P/T = constant
      • 6.022x10^23
    • Formulae
      • Empiricle
        • 1) Mass/%-age
          • 2) Relative Mass
            • 3) Moles
              • 4) Divide by smallest
                • 5) Make simplest ratio
      • Molecular
        • Ar of Molecule / RM of empirical formula of molecule
    • Atom Economy
      • (mass of desired products / total mass of reactants) x 100
    • Percentage Yield
      • (number of moles of specified product / theoretical max. moles of product) x 100
  • Ar
    • The average mass of an atom of an element (including isotopes) relative to 1/12 the Ar of Carbon-12

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