The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. Therefore, the total mass of the reactants must equal the total mass of the products.
A balanced chemical equation demonstrates this law in the following ways:
-
Same Number of Atoms: In a balanced equation, the number of atoms of each element is the same on both the reactant side and the product side. This means that no atoms are lost or gained during the reaction.
-
Stoichiometry: By ensuring that the coefficients (the numbers in front of the chemical formulas) are balanced, the equation reflects the proportions of reactants and products, showcasing that the mass (and thus the number of atoms) remains constant. For example, if you have a balanced equation like \(2H_2 + O_2 \rightarrow 2H_2O\), you can see that there are four hydrogen atoms and two oxygen atoms on each side.
-
Total Mass Calculation: If you were to take the molar masses of the reactants and products in a balanced equation, they would equal each other. This numerical balance further confirms that the total mass before and after the reaction remains the same.
Overall, a balanced chemical equation is a clear representation of how chemical reactions adhere to the law of conservation of mass, demonstrating the equality of mass on both sides of the reaction.