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Formulate the (balanced) combustion reaction of an octane (C8H18)
Solution: Burning I mean, a reaction with O2, after possibility to be created carbon dioxide and water:
C8H18 +12.5·O2 ⇄ 8·CO2 + 9·H2O
How can this be solved at all? It is assumed that C8H18 is a particle. Thus are 8 C-atoms on the left page the reaction equation present. However, this also requires 8 C atoms on the Since the C – atoms only go into the carbon dioxide must be total 8 CO2 present.
Similar to the hydrogen atoms, on the left side, there are 18 H atoms coming from the octane. which requires 2 H atoms per molecule. Thus a maximum of 9 water molecules can be formed.
So all the coefficients are on the right. However, this also results in the total number of the O – atoms, namely 8·2 + 9·1 = 25 O – atoms. They're finally coming from O2 on the left. In total, 12.5·O2 molecules can be formed.
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