What is the formula for the complete combustion of C7H16?

Prepare for the Integrated Science and Technology (ISAT) Exam with our quiz. Use our flashcards and multiple choice questions to study effectively. Each question includes hints and detailed explanations. Get ready to ace your exam!

The complete combustion of heptane (C7H16) is represented by the balanced chemical equation where all the carbon in the hydrocarbon is converted to carbon dioxide (CO2) and all the hydrogen is converted to water (H2O).

The correct equation is C7H16 + 11O2 → 7CO2 + 8H2O. In this reaction, heptane reacts with oxygen (O2) to produce seven molecules of carbon dioxide and eight molecules of water.

To balance the equation, we first note that C7H16 contains seven carbon atoms and sixteen hydrogen atoms. For complete combustion, each carbon atom should yield one CO2 molecule, resulting in 7 CO2 from 7 carbons. Each pair of hydrogen atoms produced yields one water molecule, so we have 8 water molecules for the 16 hydrogens in heptane (16 H / 2 = 8 H2O).

On the reactant side, the oxygen requirement needs to be calculated based on the products. Each CO2 molecule requires two O2 molecules for its formation, which accounts for the carbon. For the 7 CO2, this results in a total of 14 oxygen atoms (

Subscribe

Get the latest from Examzify

You can unsubscribe at any time. Read our privacy policy