How a Balanced Chemical Equation Proves the Law of Conservation of Mass
A balanced chemical equation demonstrates the Law of Conservation of Mass by showing that the number of atoms for each element present in the reactants is equal to the number of atoms for those elements in the products. This equality ensures that mass is conserved throughout the chemical reaction. For example, if a reaction begins with certain reactants, a balanced equation will account for all the atoms involved and confirm that the same total mass of matter exists on both sides of the equation.
Quick Check and Test Help
The principle of conservation of mass can be illustrated with an example involving masses:
- Mass of Reactants = Mass of Products: If a chemical reaction has 50 grams of reactants, the total mass of the products formed must also be 50 grams.
- Multiple Products: If the reaction produces multiple products, the combined mass of these products will still equal the initial mass of the reactants, asserting that no mass is lost or created during the reaction.
Lesson 10: Law of Conservation of Matter
Objective of the Lesson
The objective of this lesson is to understand the principles of the Law of Conservation of Matter and how it relates to chemical reactions and balanced equations.
Law of Conservation of Matter
The Law of Conservation of Matter states that matter cannot be created or destroyed in an isolated system. This means that the quantity of matter remains constant, and any change in the form of matter does not result in a loss or gain of mass.
Difference Between the Law of Conservation of Mass and the Law of Conservation of Matter
The Law of Conservation of Mass and the Law of Conservation of Matter describe the same fundamental principle – that the total mass remains constant in any closed system during a chemical reaction. However, the terms can sometimes have slightly different implications depending on the context. In most cases, they are used interchangeably in chemistry.
Atom Quantity in Reactions
If you begin a reaction with 3 atoms, you will have 3 atoms present at the end of the reaction. Regardless of the types of bonds formed or break, the total count of individual atoms remains unchanged, in accordance with the Law of Conservation of Matter.