Write the balanced equation for the combustion of dimethylsulfide, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~S},\) in an abundant supply of oxygen.

Combustion reactions are a type of chemical reaction where a substance combines with oxygen and releases energy in the form of light or heat. Commonly, the substance that combusts is organic, containing carbon and hydrogen, and the products are predominantly carbon dioxide (CO2) and water (H2O). In the specific example of dimethylsulfide combustion, we also see the production of sulfur dioxide (SO2) due to the sulfur content in the reactant.
In a complete combustion reaction, there is enough oxygen to allow the fuel to react completely and form a limited number of products, mainly CO2 and H2O, along with any other oxides formed from other elements present in the fuel. However, if there is insufficient oxygen, incomplete combustion occurs, resulting in a more complex mix of products, often including carbon monoxide (CO) and even soot or unburned carbon particles.

Stoichiometry is the aspect of chemistry that pertains to the quantitative relationships between reactants and products in a chemical reaction. With stoichiometry, we can determine the amount of reactants needed to produce a certain amount of product, or vice versa. It's like the recipe for a chemical reaction. In our current example of the combustion of dimethylsulfide, stoichiometry helps us understand the proportions of dimethylsulfide and oxygen that react to produce carbon dioxide, water, and sulfur dioxide.

To achieve a balanced stoichiometric equation, it is crucial to ensure that the number of atoms for each element is equal on both the reactant and product sides of the equation. This adheres to the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction. Thus, the mass of the reactants must equal the mass of the products.

Balancing chemical equations is a critical step in the study of chemistry. It ensures compliance with the Law of Conservation of Mass, indicating that atoms are neither created nor lost during a chemical reaction. The aim is to make the number of each type of atom equal on both sides of the equation. For this, we adjust the coefficients – the numbers placed before the molecules – in the reaction.

The balanced equation provides valuable insight into the stoichiometry of the reaction, allowing us to determine the relative quantities of reactants and products involved. In our exercise example, we meticulously balanced carbon, hydrogen, sulfur, and then oxygen, which required us to multiply the coefficients to get rid of any fractions and achieve whole number coefficients, which is the standard practice in representing balanced chemical equations.

The molecular composition refers to the identity and number of atoms that make up a molecule, which dictates the properties and the behavior of the molecule during chemical reactions. Understanding the molecular composition is integral in predicting product formation, explaining reactivity, and guiding the balancing of equations.
For instance, knowing that dimethylsulfide consists of two carbon (C), six hydrogen (H), and one sulfur (S) atom allows us to predict its combustion products and balance the chemical equation accordingly. As seen in our exercise, the molecular composition dictated that two molecules of carbon dioxide, three molecules of water, and one molecule of sulfur dioxide would be the products of the combustion of one molecule of dimethylsulfide in excess oxygen. This illustrates the tight link between molecular composition and stoichiometry in the systematic approach to solving chemical balance problems.