How do the products and reactants of a chemical change compare?
The mass of the products is greater than the mass of the reactants because energy is absorbed by the reaction.
The mass of the products equals the mass of the reactants because energy is not absorbed or given off by the reaction. **
The mass of the products is less than the mass of the reactants because energy is given off by the reaction.
The mass of the products equals the mass of the reactants because the same atoms are present throughout the reaction.
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To determine the relationship between the products and reactants of a chemical change, we need to consider the law of conservation of mass. According to this law, the mass of a closed system remains constant before and after a chemical change. This means that no atoms are created or destroyed during a chemical reaction.
Based on this principle, the correct statement is:
"The mass of the products equals the mass of the reactants because the same atoms are present throughout the reaction."
This means that the total mass of the substances involved in the reaction is conserved. Although the arrangement of atoms may change, the total number of each type of atom remains the same.
To understand this concept, you can verify it by conducting a simple experiment. Take a balanced chemical equation, such as the reaction between hydrogen gas (H2) and oxygen gas (O2) to form water (H2O):
2H2 + O2 -> 2H2O
In this reaction, you'll notice that two molecules of hydrogen gas react with one molecule of oxygen gas to produce two molecules of water. By balancing the equation, it ensures that the total number of atoms on both sides of the equation remains the same.
If you measure the mass of the reactants (hydrogen gas, oxygen gas) before the reaction and the mass of the products (water) after the reaction, you'll find that the mass remains unchanged. This demonstrates the conservation of mass in a chemical reaction.