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What are the steps of the Half-reaction method for Balancing redox Reactions?

Chemistry - Combustion Reaction?

  • When the hydrocarbon, C8H16, undergoes complete combustion, which is an oxidation-reduction reaction, a specific set of products are formed. What is the sum of the coefficients in the balanced equation? The products of a combustion reaction are CO2 and H2O, correct? And I know the steps for balancing redox reactions, I just can't seem to get the correct answer. Thank you for your help!

  • Answer:

    Since it is a combustion reaction the reactants are C8H16 and O2. The products are CO2 and H2O. C8H16 + O2 --> CO2 + H2O First balance C. C8H16 + O2 --> 8 CO2 + H2O Next balance H. C8H16 + O2 --> 8 CO2 + 8 H2O Finally balance O. C8H16 + 12 O2 --> 8 CO2 + 8 H2O The sum of the coefficients are (1+12+8+8) = 29

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Since it is a combustion reaction the reactants are C8H16 and O2. The products are CO2 and H2O. C8H16 + O2 --> CO2 + H2O First balance C. C8H16 + O2 --> 8 CO2 + H2O Next balance H. C8H16 + O2 --> 8 CO2 + 8 H2O Finally balance O. C8H16 + 12 O2 --> 8 CO2 + 8 H2O The sum of the coefficients are (1+12+8+8) = 29

Pushpa Padmanabhan

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