Question

\[AgN{{O}_{3}}+NaCl\to AgCl+\text{ }NaN{{O}_{3}}\]
In this reaction, the mass of $AgN{{O}_{3}}$ and $NaCl$ is equal to the mass of $AgCl$ and $NaN{{O}_{3}}$. Then, this reaction satisfies
(A) Law of constant composition
(B) Law of conservation of mass
(C) Gay Lussac’s Law
(D) Law of multiple proportions

Answer 1

Hint: The state, composition and proportion of the reactants and products formed must be seen, as it will help to determine the law followed during the reaction. Also, check if the given reaction is balanced before proceeding further.

Complete step by step solution:
In the given reaction, solid silver nitrate is dissolved in sodium chloride solution. In which due to the exchange of cations and anions, the double displacement reaction takes place. It forms a solid white precipitate of silver chloride in sodium nitrate solution. This is an example of precipitation reaction as well.
As during the silver nitrate and sodium chloride reaction, the mass of products formed is the same as the mass of reactants as given. Thus, it conserves the mass during the reaction.
Thus, in a reaction, involving chemical and physical changes, the total mass of the substances remains unchanged in an isolated system known as the Law of conservation of mass.
This chemical reaction simply shows the rearrangement of the atoms and the bonds, with the number of atoms remaining unchanged, that is, the number of atoms reactant is equal to the product side.

Therefore, the reaction satisfies the option (B)- Law of conservation of mass.

Additional information:
When the reactants are present in a gaseous state, the Gay Lussac’s law becomes applicable.

Note: This chemical reaction simply shows the rearrangement of the atoms and the bonds, with the number of atoms unchanged, that is, the number of atoms on the reactant side is equal to the product side. This is made use of during the balancing of the equation, where the number of moles is the same on both the sides of any element.