Final answer:
The question involves the chemical reaction known as combustion, where the hydrocarbon C7H14 reacts with oxygen to form carbon dioxide and water. The complete combustion process requires sufficient oxygen to ensure that only CO2 and H2O are the end products.
Step-by-step explanation:
The student's question focuses on the combustion of the hydrocarbon C7H14 to form carbon dioxide and water. Combustion is a chemical reaction where a hydrocarbon reacts with oxygen to produce carbon dioxide, water, and heat. This is an exothermic reaction, meaning it releases energy. The general formula for the complete combustion of a hydrocarbon is:
- Hydrocarbon + Oxygen → Carbon Dioxide + Water + Heat
For example, the combustion of methane, which is a simpler hydrocarbon, can be represented as:
- CH4 + 2O2 → CO2 + 2H2O + Heat
In the case of C7H14, a similar process occurs, requiring a sufficient amount of oxygen. Ensuring complete combustion, the products will only be carbon dioxide and water. In real-world scenarios, however, incomplete combustion might occur, especially if there is insufficient oxygen. This can lead to the formation of carbon monoxide and other compounds as by-products.
To write and balance the chemical equation for the combustion of C7H14, one would identify the number of carbon and hydrogen atoms in the fuel and balance them with the required number of oxygen molecules to form CO2 and H2O. The balanced equation would provide insight into the stoichiometry of the reaction, indicating how much oxygen is needed and how much carbon dioxide and water are produced.