# Law of conservation of mass who discovered

Lavoisier

## How did Antoine Lavoisier find the law of conservation of mass?

Lavoisier placed some mercury in a jar, sealed the jar, and recorded the total mass of the setup. … He found in all cases that the mass of the reactants is equal to the mass of the products. His conclusion, called the states that in a chemical reaction, atoms are neither created nor destroyed.

## Which best describes the Law of Conservation of Mass?

Which best describes the law of conservation of mass? The mass of the reactants and products is equal and is not dependent on the physical state of the substances. The equation below shows a general equation for a reaction, and the amounts of the substance are written underneath.

## How do you prove conservation of mass?

The law of conservation of mass states that matter cannot be created or destroyed in a chemical reaction. For example, when wood burns, the mass of the soot, ashes, and gases, equals the original mass of the charcoal and the oxygen when it first reacted. So the mass of the product equals the mass of the reactant.

## Why does a chemical equation need to be balanced?

Remember, chemical reactions follow the law of conservation of mass. Chemical equations show this conservation, or equality, in terms of atoms. The same number of atoms of each element must appear on both sides of a chemical equation.

## Why does a chemical equation need to be balanced quizlet?

Why must chemical equations be balanced? They must obey the Law of Conservation of Mass that states that matter cannot be created or destroyed, it is conserved. Atoms are never lost or gained in chemical reactions, they are rearranged. The mass of the reactants must equal the mass of the products.

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## Can neither be created nor destroyed?

The law of conservation of energy, also known as the first law of thermodynamics, states that the energy of a closed system must remain constantâ€”it can neither increase nor decrease without interference from outside. … The sum of these is called mechanical energy.

## Is the law of conservation of matter and mass the same?

Matter can change form through physical and chemical changes, but through any of these changes, matter is conserved. The same amount of matter exists before and after the changeâ€”none is created or destroyed. This concept is called the Law of Conservation of Mass.

## Can atoms be destroyed?

All matter is composed of extremely small particles called atoms. Atoms of a given element are identical in size, mass, and other properties. Atoms of different elements differ in size, mass, and other properties. Atoms cannot be subdivided, created, or destroyed.

## What is the law of conservation of mass easy definition?

The law of conservation of mass or principle of mass conservation states that for any system closed to all transfers of matter and energy, the mass of the system must remain constant over time, as the system’s mass cannot change, so quantity can neither be added nor be removed.

## What is the law of conservation of mass and energy?

The law of conservation of mass states that in a chemical reaction mass is neither created nor destroyed. Similarly, the law of conservation of energy states that the amount of energy is neither created nor destroyed. …

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## What type of reaction always releases energy?

exothermic reactions

## How can the law of conservation of mass be violated?

According to the law of conservation of mass, during any physical or chemical changes, the total mass of the products is equal to the total mass of the reactants. … Here conservation of mass is not obeyed as certain part of mass is converted into energy. So, law of conservation of mass is violated here.

## How do you use the law of conservation of mass?

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.