Conservation of Mass

Definition

Conservation of mass is a fundamental principle in science stating that mass cannot be created or destroyed in a closed system during a chemical reaction. This concept connects deeply with the development of atomic models, as it laid the groundwork for understanding how atoms interact and combine to form new substances while retaining their total mass.

5 Must Know Facts For Your Next Test

1. The conservation of mass was first formulated by Antoine Lavoisier in the late 18th century, who is often referred to as the father of modern chemistry.
2. Lavoisier conducted experiments that showed that during chemical reactions, the mass of the reactants is always equal to the mass of the products, establishing a key principle in chemistry.
3. This principle paved the way for later atomic theories by confirming that atoms are indivisible particles that maintain their mass through reactions.
4. The conservation of mass is fundamental to balancing chemical equations, as it ensures that all atoms are accounted for before and after a reaction.
5. Understanding conservation of mass has implications beyond chemistry; it also plays a role in physics, biology, and environmental science, influencing how scientists view interactions in different systems.

Review Questions

• How did Antoine Lavoisier's experiments contribute to the development of atomic models?
  • Antoine Lavoisier's experiments demonstrated that mass is conserved in chemical reactions, leading to the conclusion that atoms must exist as the fundamental units of matter. His work laid the groundwork for later atomic models by providing evidence that matter is not lost or gained during reactions but merely transformed. This understanding was crucial for scientists to develop more sophisticated models of atomic structure and behavior.
• In what ways does the conservation of mass apply when balancing chemical equations?
  • When balancing chemical equations, the conservation of mass requires that the number of atoms of each element be the same on both sides of the equation. This ensures that all reactants are accounted for as they transform into products. By following this principle, chemists can accurately represent the amounts of substances involved in a reaction and predict how different chemicals will interact while maintaining the same total mass.
• Evaluate how the concept of conservation of mass has influenced modern scientific thinking across various fields.
  • The concept of conservation of mass has significantly influenced modern scientific thinking by establishing a foundational principle that applies across multiple disciplines, including chemistry, physics, and biology. It shapes our understanding of chemical reactions and physical processes, promoting a view of matter as stable yet transformable. Furthermore, this principle informs environmental science by guiding how we assess material cycles in ecosystems and the impact of human activities on natural resources, emphasizing sustainability and resource management.

Related terms

Atomic Theory: The scientific theory that matter is composed of discrete units called atoms, which can combine and rearrange in chemical reactions without changing their individual mass.

Chemical Reaction: A process that leads to the transformation of one set of chemical substances into another, where the total mass of reactants equals the total mass of products.

Dalton's Law: A principle formulated by John Dalton, stating that in a chemical reaction, atoms are neither created nor destroyed, reinforcing the conservation of mass concept.