The balanced equation for the combustion of dodecane (C₁₂H₂₆) in air is:

2 C₁₂H₂₆ + 37 O₂ → 24 CO₂ + 26 H₂O

Explanation:

* Dodecane (C₁₂H₂₆) is the fuel.

* Oxygen (O₂) is the oxidant, supplied by air.

* Carbon dioxide (CO₂) and water (H₂O) are the primary products of combustion.

Balancing the equation:

1. Carbon (C): There are 12 carbon atoms on the left side and 24 on the right. We need a coefficient of 2 in front of dodecane to balance the carbon.

2. Hydrogen (H): There are 26 hydrogen atoms on the left and 26 on the right.

3. Oxygen (O): There are 37 oxygen atoms on the left and 50 on the right. We need a coefficient of 37/2 in front of oxygen.

To avoid fractional coefficients, multiply the entire equation by 2, resulting in the balanced equation shown above.

Note: This equation represents complete combustion, where all the dodecane is completely oxidized. In reality, combustion may not be complete and some byproducts, such as carbon monoxide (CO) and soot, might be produced.