Question

This chemical equation is not balanced:

AgBr(s) → Ag(s) + Br2(g).

Why isn’t it possible for the reaction to occur as indicated by the unbalanced equation?

A. There are more substances on the right side of the equation than on the left side.
B. There is a gas on the right side of the equation but not on the left side.
C. The bromine atoms must go through a liquid state before becoming a gas.
D. There is more mass represented on the right side of the equation than on the left side.
E. The bromine atoms on the right side of the equation are not bonded to another element.

Answer 1

D

Step-by-step explanation:

Answer 2

Answer : 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.

`AgBr(s)\rightarrow Ag(s)+Br_2(g)` (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)\rightarrow 2Ag(s)+Br(g)` (Balanced reaction)

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

Mass of product,
`2Ag+Br_2` = 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.