Electrolysis

Electro Lysis
1. To split things
2. Electrisity
3. To use Electrisity to break things down into different things
Electrolysis of Brine (Salt Water)
1. Sodium Chloride dissolved in Water
  1. NaCl +H2O
  2. Na+, Cl-, H+, OH-
2. Products
  1. Hydrogen
    1. Hydrogenation
      1. Making Margerine
  2. Chlorine
    1. Killing Bacteria
      1. Pools and Tap Water
  3. Sodium Hydroxide
    1. Making Soap
      1. Detergent
3. 2H+ + 2e– → H2
  1. Half equation for the formation of Hydrogen
4. 2Cl- → Cl2 + 2e-
  1. Half equation for the formation of Chlorine
5. The Reactions
  1. Chlorine is less reactive than the Hydroxide ions
    1. Thus it has to go to an Atom, not a stable Ion
  2. Hydrogen is less reactive than the Sodium Ions
    1. Thus the Hydrogen has to turn into an Atom again
  3. The remaining Hydroxide and Sodium Ions are bonded into Sodium Hydroxide
Electrolysis of Aluminium
1. Cyralite is added to the Bourxite to lower melting point
  1. Goes from 2000°C to 900°C
    1. Saves Energy
      1. Makes it cheaper
2. Al3+ + 3e- → Al
  1. Half equation for Aluminium
3. 2O2- → O2 + 4e-
  1. Half equation for Oxygen
4. Due to the tempretures, some of the Oxygen Ions bond with the carbon Anode
  1. Causing it to wear away
    1. Need to be replaced often
5. Aluminium is needed as it is very useful
  1. Very Stong
  2. Very Light
6. Bourxite is a fancy word for Aluminium Ore
7. Bourxite is made up of Aluminium 3+ and Oxygen 2-

Resource summary

	Created by Alex Maraio over 10 years ago