Question

The amount $4.88$g of $KCI{O_3}$when heated produces $1.92$ g of oxygen and $2.96$g of $KCl$. Which of the following statements regarding the experiment is correct?
(a) The result illustrates the law of conservation of mass
(b) The result illustrates the law of conservation of multiple proportions
(c) The result illustrates the law of conservation of constant proportion
(d) None of the above laws is followed

Answer 1

The law of conservation of mass states that, the mass of the reactants involved in the chemical reaction is equal to the mass of the products formed. Law of constant proportions states that the ratio of atoms in a particular compound is the same or fixed.

Complete answer:
Given that $KCI{O_3}$ has a mass of $4.88$g is heated. Potassium chlorate is the chemical name of $KCI{O_3}$. It has potassium, chlorine and oxygen atoms. It is a white crystalline substance.
When potassium chlorate $\left( {KCI{O_3}} \right)$ is heated, it produces oxygen and potassium chloride.
The chemical reaction involved is $2KCl{O_3} \to 2KCl + 3{O_2}$
Thus, the products of oxygen and potassium chloride form, when potassium chlorate is heated.
The mass of oxygen produced is $1.92$ gm. The mass of potassium chloride formed is $2.96$gm.
The sum of the mass of oxygen and mass of potassium chloride is $4.88$gm.
Since, the mass of $KCI{O_3}$ heated is $4.88$gm.

Thus, the mass of the reactants and products are equal, which proves the law of conservation of mass.

Note:
The law of conservation of mass states that the mass of the reactants and products should be equal. The mass of all the reactants should be calculated clearly. The product's mass can also be added if one or more reactants is present, and it should be equal to the mass of the reactants.