Write a balanced equation, including all of the appropriate notations, for each of the following reactions. $$ \begin{array}{l}{\text { a. Steam reacts with solid carbon to form }} \\\ {\text { the gases carbon monoxide and hydrogen. }} \\ {\text { b. Heating ammonium nitrate in aqueous }} \\ {\text { solution forms dinitrogen monoxide gas }} \\ {\text { and liquid water. }} \\ {\text { c. Nitrogen dioxide gas forms from the }} \\ {\text { reaction of nitrogen monoxide gas and }} \\\ {\text { oxygen gas. }}\end{array} $$

Stoichiometry is foundational in understanding chemical reactions. It deals with the quantitative relationships between the reactants and products in a chemical reaction. Essentially, it tells us how much of each substance is needed to react with another, and what amount of product will be formed as a result.

When approaching stoichiometry, think of it like a recipe: if you need to bake a cake, the recipe provides the exact amount of each ingredient. Similarly, a balanced chemical equation provides the exact proportions of reactants that react to form the products.

Furthermore, stoichiometry can involve calculations such as determining the molar ratios, mass of reactants or products, and the amount of energy involved in a reaction. It plays a crucial role in many practical applications, including pharmaceuticals, engineering, and environmental science.

Chemical reactions are processes where substances, known as reactants, transform into entirely new substances called products. These transformations occur through the breaking and forming of chemical bonds. Reactions are represented by chemical equations which contain the chemical notations of the reactants and products along with their respective physical states.

Chemical reactions can be classified into different types, such as synthesis, decomposition, single replacement, double replacement, and combustion. Each type involves different patterns of reactant and product formation. For instance, combustion reactions typically involve oxygen as a reactant and produce carbon dioxide and water. Understanding the types of chemical reactions helps in predicting the products that might form.

Chemical notations represent the shorthand way of describing chemical compounds and the reactions they undergo. These notations include chemical symbols for elements, numbers representing the number of atoms (subscripts), and coefficients representing the number of molecules or moles. Additionally, the physical states of substances are denoted as (s) for solids, (l) for liquids, (g) for gases, and (aq) for aqueous solutions.

Correctly writing chemical formulas and equations is crucial in conveying accurate information about the reaction. For example, the notation '2H₂O' tells us there are two molecules of water, each containing two hydrogen atoms and one oxygen atom. Learning to interpret these symbols and notations is essential for mastering stoichiometry and reaction balancing.

Reaction balancing is the process of ensuring that the number of atoms of each element is the same on both sides of the chemical equation. This is in accordance with the Law of Conservation of Mass, which states that matter cannot be created or destroyed in a chemical reaction. Therefore, the mass and charge must be balanced in the equation.

The steps to balance a chemical reaction typically involve: writing an unbalanced equation with correct formulas, determining the stoichiometry of the reactants and products, and adjusting coefficients to balance the atoms. The coefficients represent the smallest whole number ratios of molecules that are involved in the reaction. Through this process, one confirms that the atoms that enter a reaction are equal to those that come out in the form of products.

For instance, in the reaction of nitrogen monoxide and oxygen forming nitrogen dioxide: 2NO(g) + O₂(g) → 2NO₂(g), the coefficients show that two molecules of nitrogen monoxide react with one molecule of oxygen to form two molecules of nitrogen dioxide.