Final answer:
A balanced chemical equation conserves mass and specifies the stoichiometry of reactions, representing quantities of reactants and products in terms of moles.
Step-by-step explanation:
Understanding Balanced Chemical Equations
A balanced chemical equation is fundamental in chemistry as it represents the conservation of mass and the stoichiometry of reactions. For example, considering an equation like 2H₂ + O₂ → 2H₂O, it shows that two moles of hydrogen gas react with one mole of oxygen gas to produce two moles of water. This equality ensures that the number of atoms of each element is the same on both sides of the reaction equation, adhering to the Law of Conservation of Mass.
When it comes to mass-mass calculations as indicated by section 5.5: Mole-Mass and Mass-Mass Calculations, understanding the mole concept is essential. For instance, the molar mass of substances can be used to convert between the mass of a substance and the number of moles. Coefficients in a balanced equation can then be interpreted as representing the molar amounts of reactants and products, aiding in calculations regarding the amount of substances needed or produced in a reaction.
In any balanced equation, such as the Haber process, N₂ + 3H₂ → 2NH₃, the coefficients before the chemical formulas represent the molar ratio of reactants to products. This stoichiometric proportion is used to calculate the quantities of reactants needed and the amount of product that can be formed. Thus, a balanced chemical equation is not only a qualitative representation but also provides quantitative information for the reactants and products involved in a chemical reaction.