Mole concept

• Mole


  The amount of a substance which contains as many elementary entities as there are atoms in 12.0 grams of carbon-12

  
• Avogadro's number


  6.02 x 10^23 atoms, ions, molecules, electrons, protons, etc.
• Mole in terms of formula

  Moles = Mass / Relative Molecular Mass

  
• Mole in terms of formula

  • 10g of sodium hydroxide (NaOH)
  • 1g of hydrogen gas (H2)
  • 0.2 mole of calcium trioxonitrate (V) Ca(NO3)2

  
• Mole in terms of Relative Atomic Mass (RAM) or Relative Molecular Mass (RMM)


  1 mole of any substance = RAM or RMM of the substance

  
• Mole in terms of RAM/RMM

  • 27g of Aluminium (Al)
  • 0.1 mole of sodium trioxocarbonate (IV) (Na2CO3)
  • 10.35g of Lead (Pb)
• Mole in terms of Avogadro's number

  1 mole = 6.02 x 10^23 atoms, ions, molecules, electrons, protons, etc.

  
• Mole in terms of Avogadro's number

  • 2 moles of potassium ion (K+)
  • 4.4g of Carbon (IV) oxide (CO2)
  • 12.04 x 10^23 atoms of Nitrogen (N2)

  
• Molar volume


  The volume occupied by 1 mole of any gas at standard temperature and pressure (STP), which is 22.4 dm^3 or 22,400 cm^3
• Mole in terms of molar volume

  • 2 moles of carbon (IV) oxide (CO2) at STP
  • 5,600 cm^3 of chlorine gas (Cl2) at STP