When heated to \(700-800^{\circ} \mathrm{C}\), diamonds, which are pure carbon, are oxidized by atmospheric oxygen. (They bum!) Write the balanced equation for this reaction.

In our everyday life, we observe many changes in substances around us, from the rusting of iron to the baking of bread. These changes result from chemical reactions, where substances, known as reactants, transform into new substances called products. A chemical reaction involves the breaking and forming of chemical bonds, which results in a change in the composition and properties of matter.

For instance, when diamonds, composed purely of carbon atoms, are heated at high temperatures in the presence of oxygen, they undergo a combustion reaction. Each carbon atom in the diamond binds with oxygen molecules from the air, resulting in the formation of carbon dioxide. The process is an example of an oxidation reaction—one particular type of chemical reaction where a substance combines with oxygen.

Oxidation is a process that involves the loss of electrons during a reaction by a molecule, atom, or ion. In terms of organic chemistry, it often refers to the process of a substance combining with oxygen. When carbon oxidizes, it reacts with oxygen to form carbon dioxide (CO2), which is what happens when diamonds are burnt.

The oxidation of carbon is a highly exothermic reaction, meaning it releases a significant amount of energy in the form of heat and light. This energy release is characteristic of combustion reactions, a type of oxidation, where carbon-based materials burn in an excess of oxygen.

Stoichiometry is the branch of chemistry that deals with the quantitative aspect of chemical reactions. It involves calculations to determine the amount of reactants required or the amount of products formed in a chemical reaction. Stoichiometry is grounded in the law of conservation of mass and uses the mole concept as its foundation to balance chemical equations.

In the balanced equation of the oxidation of carbon, stoichiometry tells us that one mole of carbon reacts with one mole of oxygen (O2) to form one mole of carbon dioxide (CO2). The molar ratios provide crucial insights into the reaction and are essential for ensuring that all atoms present in the reactants appear in the products.

The law of conservation of mass is a critical scientific principle that states that mass is neither created nor destroyed in a chemical reaction. Instead, the mass of the reactants is equal to the mass of the products. This law is fundamental in the balancing of chemical equations, as it ensures that the amount of each element is the same on both sides of the reaction.

In the given exercise, this law helps us to confirm that the equation C + O2 -> CO2 is balanced. It shows that one carbon atom is present on both sides, and the two oxygen atoms initially present in the reactant O2 are also accounted for in the product CO2. Thus, the mass is conserved, and the equation correctly represents the chemical reaction.