Question

law of consevation of mass by means of chemical reaction​

Answer 1

Answer:

Law of conservation states that mass can neither be created nor be destroyed in a chemical reaction. Such as:

H2+ O2→H2O

This equation is not balanced. The correct one will be:

2H2+O2→2H2O

Here the equation clearly depicts that 2 mole of Hydrogen reacts completely with 1 mole of O2 to give 2 mole of H2O.

If you check, you will see that in both L.H.S and R.H.S the equation is having equal masses for each element.

Hope it helps you.

Answer 2

Answer:

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To prove:- Law of conservation of mass by means of chemical method.

Key points:-

• The law of conservation of mass states that mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations.
• According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.
• The law of conservation of mass is useful for a number of calculations and can be used to solve for unknown masses, such the amount of gas consumed or produced during a reaction.

Terms:-

• reactant:- Any of the participants present at the start of a chemical reaction. Also, a molecule before it undergoes a chemical change.
• law of conservation of mass:- A law that states that mass cannot be created or destroyed; it is merely rearranged.
• product:- A chemical substance formed as a result of a chemical reaction.

History of the Law of the Conservation of Mass:-

The ancient Greeks first proposed the idea that the total amount of matter in the universe is constant. However, Antoine Lavoisier described the law of conservation of mass (or the principle of mass/matter conservation) as a fundamental principle of physics in 1789.

This law states that, despite chemical reactions or physical transformations, mass is conserved — that is, it cannot be created or destroyed — within an isolated system. In other words, in a chemical reaction, the mass of the products will always be equal to the mass of the reactants.

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