What's an unbalanced equation?

An unbalanced chemical equation has unequal no of atoms in the reactants and products.

Take it as an example : Mg + O2 ⇒ MgO

Law of conservation of mass governs the balancing of a chemical equation. According to this law matter can neither be created nor destroyed in a chemical reaction

Explanation:

so for your question your answer will be:

There is more mass represented on the right side of the equation than on the left side.

According to the law of conservation of mass, the balanced reaction is a reaction in which the mass of the reactant side must be equal to the mass of product side.

AgBr (s) - > Ag (s) + Br2 (g) (This is an unbalanced reaction)

Mass of reactant, AgBr = 108 + 80 = 188 g

Mass of product, Ag+Br_2 = 108 + 2 (80) = 268 g

This reaction is not balanced reaction because there is more mass represented on the right side of the equation than on the left side.

2AgBr (s) - > 2Ag (s) + Br (g) (Now this is a Balanced reaction)

Mass of reactant, 2 AgBr = 2 (108 + 80) = 376 g

Mass of product, 2Ag + Br2 = 2 (108) + 2 (80) = 376 g

In the balanced reaction, the mass of reactant is equal to the mass of product.

So your answer will be There will be more mass represented on the right side of the equation than on the left side.

The correct option is, (D)

Explanation : Balanced chemical reaction : According to the law of conservation of mass, the balanced reaction is a reaction in which the mass of the reactant side must be equal to the mass of product side.

(unbalanced reaction)

Mass of reactant, AgBr = 108 + 80 = 188 g

Mass of product, = 108 + 2 (80) = 268 g

This reaction is not balanced reaction because there is more mass represented on the right side of the equation than on the left side.

(Balanced reaction)

Mass of reactant, 2 AgBr = 2 (108 + 80) = 376 g

Mass of product, = 2 (108) + 2 (80) = 376 g

In the balanced reaction, the mass of reactant is equal to the mass of product.

So, from the given option, the option D is correct.