Balancing chemical equations is a fundamental aspect of chemistry, ensuring that matter is neither created nor destroyed in a reaction. An unbalanced equation means that the number of atoms for each element is not the same on both sides of the equation.
Given the equation:
[tex]$
AgBr(s) \rightarrow Ag(s) + Br_2(g)
$[/tex]
Let's analyze it step-by-step to determine why this equation might not correctly describe the reaction.
- Left Side (Reactants):
- Silver bromide (AgBr)
- Right Side (Products):
- Silver (Ag)
- Bromine gas (Br₂)
First, count the number of each type of atom on both sides of the equation:
- Left Side:
- Silver (Ag): 1 atom
- Bromine (Br): 1 atom
- Right Side:
- Silver (Ag): 1 atom
- Bromine (Br): 2 atoms (since Br₂)
By comparing the counts, it's clear that:
- The number of silver (Ag) atoms is balanced with 1 atom on each side.
- The number of bromine (Br) atoms is not balanced; we have 1 atom of bromine on the reactant side and 2 atoms in the form of Br₂ on the product side.
A balanced chemical equation must have the same number of each type of atom on both sides of the equation. Here, the discrepancy arises because each bromine atom on the right must be accounted for, reflecting that bromine molecules (Br₂) consist of two bromine atoms bonded together.
Based on these observations, the correct reason why the equation isn't balanced is related to the bromine atoms. Specifically, the problem lies in how the bromine is represented on the product side:
- Answer E: The bromine atoms on the right side of the equation are not bonded to another element.
Therefore, the correct answer is E.
