Question

Write an equation for the combustion of butane.

Short answer

The balanced chemical equation for the combustion of butane is $2C4H10+13O2\to 8CO2+10H2O$.

Step-by-step solution

Write the chemical formula for butane

Butane is an organic molecule with the formula C4H10. It consists of four carbon (C) atoms and ten hydrogen (H) atoms.

Write the reactants for the combustion

Combustion is a chemical reaction that involves a fuel and an oxidant, typically oxygen (O2). For the combustion of butane, the reactants are butane (C4H10) and oxygen (O2).

Write the products of the combustion

The products of the complete combustion of a hydrocarbon are carbon dioxide (CO2) and water (H2O).

Balance the equation

The balanced chemical equation must have the same number of each type of atom on both sides of the equation. For the combustion of butane, the balanced equation is:$$2C4H10+13O2\to 8CO2+10H2O$$

Key concepts

Chemical Reactions

At the heart of chemistry lies the study of chemical reactions, which are the processes that involve the transformation of one set of chemical substances into another. A chemical reaction is symbolized by a chemical equation wherein the reactants are listed on the left side, and the products are listed on the right. When butane combusts, it reacts with oxygen in a chemical reaction that releases energy in the form of heat and light.

Understanding the combustion of butane involves recognizing that it is a type of chemical reaction known as a combustion reaction. In this process, butane (a hydrocarbon) reacts with oxygen (the oxidant) to produce carbon dioxide and water. However, to fully understand and depict this transformation, we need a balanced chemical equation, ensuring that the law of conservation of mass is respected.

Balancing Chemical Equations

Balancing chemical equations is a crucial step in the study of chemical reactions, ensuring the same number of atoms for each element are present on both sides of the equation to obey the conservation of mass. With the chemical equation of butane's combustion, we must ensure that the carbon, hydrogen, and oxygen atoms are balanced.

To achieve this, start with the most complex molecule, typically the one with the most elements or atoms. In the case of the combustion of butane, we balance carbon (C) and hydrogen (H) atoms first by adjusting the coefficients, which are numbers placed in front of the compounds. Finally, balance the oxygen (O) atoms, which may require some trial and error. The balanced equation for the combustion of butane, $$2C4H10+13O2\to 8CO2+10H2O$$, illustrates that we have the same number of each type of atom on both sides of the reaction. This balanced equation serves as a blueprint to understanding the quantitative aspects of the chemical reaction.

Hydrocarbon Combustion

Hydrocarbon combustion is a specific type of chemical reaction where a hydrocarbon, like butane, reacts with oxygen to form carbon dioxide and water, typically releasing heat and sometimes light—a classic example of an exothermic reaction.

In our daily lives, the combustion of hydrocarbons provides the energy needed to power vehicles, heat homes, and cook food. From an educational standpoint, understanding hydrocarbon combustion is essential for grasping broader concepts like stoichiometry, energy transfer, and reaction thermodynamics. In the equation for butane's combustion, we see the transformation of a hydrocarbon into simpler, oxide-based molecules. This reaction is clean and efficient when an adequate supply of oxygen is available, resulting in complete combustion. Incomplete combustion, on the other hand, can produce carbon monoxide and soot due to insufficient oxygen, underlining the importance of proper air-to-fuel ratios in practical applications.