Unless under pressure, carbonic acid \(\left(\mathrm{H}_{2} \mathrm{CO}_{3}\right)\) in aqueous solution breaks down into carbon dioxide and water, and carbon dioxide is evolved as bubbles of gas. Write an equation for the conversion of carbonic acid to carbon dioxide and water.

Understanding the breakdown of carbonic acid (\texttt{H\(_{2}\)CO\(_{3}\)}) in an aqueous solution is a fascinating and relevant application of chemical principles. When not under pressure, carbonic acid naturally decomposes into carbon dioxide (\texttt{CO\(_{2}\)}) and water (\texttt{H\(_{2}\)O}). This process is characterized by the release of CO\(_{2}\) as bubbles of gas, which is an observable phenomenon many are familiar with when opening a bottle of a carbonated drink.
The balanced chemical equation representing this reaction is simple yet significant, \texttt{H\(_{2}\)CO\(_{3}\) \(\rightarrow\) CO\(_{2}\) + H\(_{2}\)O}. The equation needs to be balanced to comply with the law of conservation of mass, which states that the number of atoms of each element must be the same on both sides of the equation. For carbonic acid decomposition, the equation is already in its balanced form, showing that one molecule of carbonic acid gives rise to one molecule of carbon dioxide and one molecule of water.

In chemistry, stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It is a foundational concept that enables chemists to predict the amounts of substances consumed and produced in a given reaction.
When balancing the chemical equation for the decomposition of carbonic acid, stoichiometry ensures that the principle of the conservation of mass is respected. By looking at the balanced equation \texttt{H\(_{2}\)CO\(_{3}\) \(\rightarrow\) CO\(_{2}\) + H\(_{2}\)O}, we can determine that one mole of carbonic acid yields one mole of carbon dioxide and one mole of water under standard conditions.
Stoichiometry is not only about balancing equations but also about understanding mole ratios, calculating mass relationships, and interpreting volume relations in gases, which are all vital when it comes to actual laboratory work or industrial applications.

A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. The carbonic acid decomposition is a classic example of a chemical reaction, where reactants (carbonic acid) are converted into products (carbon dioxide and water).
This particular reaction is classified as a decomposition reaction, which is a type of chemical reaction where one compound breaks down into two or more simpler substances. These reactions can be influenced by various factors such as temperature, concentration, and pressure. Understanding the nature of chemical reactions is essential for predicting reaction behavior, synthesizing new compounds, and even in fields like environmental science where the impact of gases like CO\(_{2}\) on atmospheric chemistry is studied.