What Is the Law of Indestructibility of Matter Definition Explanation and Examples
Scientists started looking at how and why chemicals react as they developed more exact theories about elements, compounds, and mixtures.
Law of Indestructibility of Matter
A. Lavoisier, a French chemist, provided the groundwork for the scientific study of matter when he stated that substances respond according to specific rules. The laws of chemical combination are what are known as these laws. Later, Dalton's Atomic Theory of Matter was built around these principles.
History of The Scientist
Name: Antoine-Laurent de Lavoisier
Born: 26 August 1743
Died: 8 May 1794
Field: Biologist, Chemist
Nationality: French
What is the Law of Conservation of Mass?
According to the rule of conservation of mass, no new mass will be formed during a chemical reaction in an entirely closed system. Furthermore, regardless of the kind of chemical reaction that takes place, the law of conservation of mass dictates that mass is preserved from reactants to products. The law of conservation of mass is simply defined as what goes in should come out.
Law of Conservation of Mass Examples
Chemical Reaction Taking Place
Following are some examples of conservation in a straightforward combination reaction involving the chemical combination of two substances: 200g A plus 100g B. The mass on the left side of the arrow will always equal the mass on the right side of the arrow in a closed system where none of the reactants is lost during the reaction.
In a double-replacement reaction, for instance, the components of the reactants have changed positions and are now AB + CD → AC + BD. In a wholly enclosed system, if 150g AB and 250g CD are chemically reacted, the combined masses of the products AC and BD will be 400g.
Limitations of Law of Indestructibility of Matter
According to the definition of the rule of conservation of mass, any physical or chemical change must result in an equal balance of reactant and product masses. However, some of the mass in a nuclear reaction is transformed into energy, leading to an imbalance in the mass of the reactants and products. The overall mass is not conserved as a result. This is the mass conservation principle's constraint.
According to Einstein's theory, the other restriction on mass conservation is that energy and mass can be converted into one another. As a result, both the system's mass and energy must be conserved for the law of conservation of mass to be true.
Applications of Law of Indestructibility of Matter
The ability to forecast a system's macroscopic behaviour without having to think about the microscopic specifics of how a physical process or chemical reaction would unfold is a key function of conservation laws.
Solved Examples
1. Why is the conservation of mass believed to be a part of the conservation of energy?
Ans: It has been found that in nuclear reactions, the mass of the reactants is greater than the mass of the products. The mass defect, also known as the difference in mass, is said to be transformed into energy via Einstein's equation. We should call it the law of conservation of mass and energy as a result.
2. Carbon dioxide and calcium oxide are both produced in equal amounts by 10 g of calcium carbonate. Explain this reaction using the mass conservation law.
Ans: Following the law of conservation of mass:
Reactant mass = Product mass.
10 g of Calcium carbonate = 6.2 g of Calcium oxide + 3.8 g of Carbon-dioxide.
10 g of reactant = 10 g of products
Thus, it is demonstrated that the above reaction adheres to the law of conservation of mass.
3. 36 grams of water are created when 4 grams of hydrogen and some oxygen combine. Determine the amount of oxygen that must have been consumed using the law of conservation of mass.
Ans: Mass given for each compound is as follows:
Hydrogen = 4g
Oxygen = x g
Water = 36 g
Following the Law of conservation of Mass:
Mass of reactants = Mass of products
4 g + x g = 36 g
x g = 36 g – 4 g
x = 32 g
Therefore, 32 g of oxygen was used.
Important Points to Remember
As long as there is no energy loss during a chemical reaction, the law of conservation of mass applies. As long as the frame of reference is inertial, the law of conservation of mass applies in terms of physics. This is because we are unable to characterize all energies in a non-inertial frame.
Conclusion
According to the rule of conservation, the mass of the products is dependent on the mass of the reactants. Based on the mass of the reactants utilized in the reaction, the law of conservation of mass is used to forecast the mass of the products that will be produced.
FAQs on Law of Indestructibility of Matter in Chemistry
1. What is the Law of Indestructibility of Matter?
The Law of Indestructibility of Matter states that matter cannot be created or destroyed in a chemical reaction, only transformed from one form to another. This law is also known as the Law of Conservation of Mass and was formulated by Antoine Lavoisier.
- The total mass of reactants equals the total mass of products.
- Atoms are rearranged during a chemical reaction but are not lost or gained.
- This principle applies to all ordinary chemical reactions.
2. Who discovered the Law of Indestructibility of Matter?
The Law of Indestructibility of Matter was formulated by Antoine Lavoisier in 1789. He performed careful experiments measuring masses before and after chemical reactions in sealed containers.
- He showed that the mass of reactants equals the mass of products.
- His work disproved earlier theories like the phlogiston theory.
- He is often called the "Father of Modern Chemistry."
3. How does the Law of Indestructibility of Matter apply to chemical reactions?
The Law of Indestructibility of Matter applies to chemical reactions by requiring that the total mass remains constant before and after the reaction. In every balanced equation:
- The number of atoms of each element is the same on both sides.
- No atoms are created or destroyed—only rearranged.
There are 4 hydrogen atoms and 2 oxygen atoms on both sides, so mass is conserved.
4. Can you give an example that proves the Law of Conservation of Mass?
An example that proves the Law of Conservation of Mass is the reaction between calcium carbonate and hydrochloric acid in a closed system. The balanced equation is:
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)
- If the reaction is done in a sealed container, the total mass remains constant.
- The mass of CaCO3 and HCl equals the mass of CaCl2, CO2, and H2O combined.
5. Why is it important to balance chemical equations according to the Law of Indestructibility of Matter?
Balancing chemical equations is necessary because the Law of Indestructibility of Matter requires the same number of each type of atom on both sides of the equation. A balanced equation:
- Ensures mass is conserved.
- Gives correct mole ratios for stoichiometric calculations.
- Represents the actual chemical process accurately.
6. What is the difference between the Law of Indestructibility of Matter and the Law of Conservation of Energy?
The Law of Indestructibility of Matter states that mass cannot be created or destroyed, while the Law of Conservation of Energy states that energy cannot be created or destroyed, only transformed. In chemistry:
- Mass conservation applies to atoms in chemical reactions.
- Energy conservation applies to heat absorbed or released (exothermic or endothermic reactions).
- Both laws operate simultaneously in chemical processes.
7. Does the Law of Indestructibility of Matter apply to nuclear reactions?
The Law of Indestructibility of Matter does not strictly apply to nuclear reactions because mass can be converted into energy. In nuclear processes:
- A small amount of mass is transformed into energy according to E = mc2.
- The combined mass–energy is conserved, not mass alone.
8. How do you verify the Law of Conservation of Mass experimentally?
You can verify the Law of Conservation of Mass by carrying out a chemical reaction in a closed system and measuring mass before and after the reaction. Steps:
- Place reactants in a sealed flask.
- Measure the total mass before reaction.
- Allow the reaction to occur without opening the system.
- Measure the total mass again.
9. What happens to atoms during a chemical reaction according to the Law of Indestructibility of Matter?
According to the Law of Indestructibility of Matter, atoms are rearranged during a chemical reaction but are neither created nor destroyed. Specifically:
- Old chemical bonds break.
- New chemical bonds form.
- The total number of each type of atom remains constant.
10. What are common mistakes students make about the Law of Indestructibility of Matter?
A common mistake is thinking that mass decreases if a gas escapes, but the Law of Indestructibility of Matter still applies in a closed system. Frequent errors include:
- Not considering gaseous products like CO2 in open reactions.
- Confusing physical changes with chemical reactions.
- Forgetting to balance chemical equations correctly.
