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Law of Conservation of Mass Experiments

Law of conservation of mass is proposed by John Dalton. In his theory of the atom that atoms can neither be created nor destroyed, but change from one form to another. Hence matter too which is made up of atoms can be neither created nor destroyed.

Lavoisier formulated the law on the basis of experimental evidence. He heated tin with air in a closed vessel and found that the total mass of tin and air before the chemical change remained unaltered even after the chemical change producing tin oxide provided the temperature remained constant. Hence before and after the experiment the mass remained the same.

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State the Law of Conservation of Mass

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Law of conservation of mass states that "In any chemical reaction the total mass of the reacting substances is equal to the total mass of the products of the reaction provided masses are measured under similar conditions".

The mass balance upon the "law of conservation of mass". The law of conservation of mass states that mass can be neither created nor destroyed. Thus the mass of a closed system must be constant or conserved. Mass can change form but the total mass must not be changed. From the "law of conservation of mass". 

Mass In = Mass Out + Mass Accumulation

Many solutions in the industrial and chemical processes today are derived from the use of these laws. 

When calcium carbonate is heated a chemical reaction takes place to form calcium oxide and carbon dioxide. It has been found by experiments that if 100 grams of calcium carbonate are decomposed completely then 56 grams of calcium oxide and 4 grams f carbon dioxide are formed. This can be written as 

Calcium carbonate $\xrightarrow[Chemical\ reaction]{Heat}$ Calcium oxide + Carbon dioxide

In this example, calcium carbonate is the reactant and it has a mass of 100g. Calcium oxide and carbon dioxide are the products and they have a total mass of 56g + 44g = 100g. Now since the total mass od products is equal to the total mass of reactant there is no change of mass during this chemical reaction.

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