How does a balanced chemical equation demonstrate the Law of Conservation of Mass?
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A balanced chemical equation demonstrates the Law of Conservation of Mass by showing that the total mass of the reactants is equal to the total mass of the products. This means that in a chemical reaction, mass is neither created nor destroyed. To understand how a balanced chemical equation demonstrates this law, let me explain how to balance an equation.
To balance a chemical equation, you need to ensure that the number of atoms of each element is the same on both sides of the equation. Here's the explanation of the steps to balance an equation:
1. Write down the unbalanced equation: Start by writing down the chemical equation with the reactants on the left side and the products on the right side, separated by an arrow.
2. Count the number of atoms: Count the number of atoms of each element on both sides of the equation. This includes all elements involved, such as carbon, hydrogen, oxygen, etc.
3. Use coefficients: Add coefficients (whole numbers in front of the formulas) to balance the equation. You can balance the equation by adjusting these coefficients to ensure that the number of atoms of each element is the same on both sides.
4. Check for balance: After adjusting the coefficients, go back and count the number of atoms again to make sure they're equal on both sides.
Once the equation is balanced, it shows that the total mass of the reactants is equal to the total mass of the products. This illustrates the Law of Conservation of Mass, which states that mass cannot be created or destroyed in a chemical reaction. The number of atoms before and after the reaction remains the same, but their arrangement and combinations change, resulting in different substances.
In summary, a balanced chemical equation demonstrates the Law of Conservation of Mass because it shows that the total mass of the reactants equals the total mass of the products. Balancing the equation ensures that every atom is accounted for and no mass is lost or gained during the reaction.