Combustion methods
Complete Combustion: to produce water and carbon dioxide, happens in a plentiful supply of oxygen
Combustion equations for alkanes:
1) Ethane:
C2H6(g) + 3.5 O2(g) --> 2CO2(g) + 3H2O(g) = because there is a 3.5 which is theoretically impossible because you cannot split a oxygen molecule in 3.5 so you have to double the whole equation so that it can be balanced!
2C2H6(g) + 7O2(g) --> 4CO2(g) + 6H2O(g)
2)Propane:
Ethane:
C3H8(g) + 5O2(g) -->3CO2(g) + 4H2O(g)
- Test: co2 turns limewater cloudy
- h20 turns anhydrous copper sulphate white to blue.
Combustion equations for alkanes:
1) Ethane:
C2H6(g) + 3.5 O2(g) --> 2CO2(g) + 3H2O(g) = because there is a 3.5 which is theoretically impossible because you cannot split a oxygen molecule in 3.5 so you have to double the whole equation so that it can be balanced!
2C2H6(g) + 7O2(g) --> 4CO2(g) + 6H2O(g)
2)Propane:
Ethane:
C3H8(g) + 5O2(g) -->3CO2(g) + 4H2O(g)
Combustion equations for alkenes:
1) Ethene:
C2H4(g) + 3O2(g) --> 2CO2(g) + 2H2O(g)
2)Propene:
C3H6(g) + 4.5O2(g) -->3CO2(g) + 3H2O(g)
C6H6(g) + 9O2(g) -->6CO2(g) + 6H2O(g)
1) Ethene:
C2H4(g) + 3O2(g) --> 2CO2(g) + 2H2O(g)
2)Propene:
C3H6(g) + 4.5O2(g) -->3CO2(g) + 3H2O(g)
C6H6(g) + 9O2(g) -->6CO2(g) + 6H2O(g)