Final answer:
The key difference between balanced and unbalanced chemical equations is that a balanced equation shows equal number and types of atoms on both sides, conserving mass, while an unbalanced one does not. Balancing chemical equations is crucial for correct stoichiometric calculations, as it indicates the precise mole ratios of reactants and products involved in a chemical reaction.
Step-by-step explanation:
The difference between balanced and unbalanced chemical equations lies in the equality of the number and types of atoms on both sides of the equation. A balanced chemical equation reflects the law of conservation of mass, meaning the atoms and molecules' count must be the same for the reactants and the products. For instance, the balanced equation for the production of ammonia from hydrogen and nitrogen has coefficients that show the precise stoichiometric factors for the reaction.
Conversely, an unbalanced chemical equation does not represent the same number of each type of atom on both sides of the equation, and thus does not reflect the actual proportions of reactants and products involved in the reaction.
When we balance an equation, we add coefficients to ensure that there's an equal number of atoms for each element in the reactants and products. Balancing by inspection is a common method used to achieve this. Balancing is critical for correctly understanding and computing reaction stoichiometry, as it allows for accurate quantitative assessments and calculations in mol, not in units of mass or volume.