To balance the chemical reaction for the tarnishing of silver, we need to ensure that the number of atoms of each element on the reactant side is equal to the number on the product side. The unbalanced chemical equation is:
[tex]\[ \square \, \text{Ag}(s) + \square \, \text{H}_2\text{S}(g) \rightarrow \square \, \text{Ag}_2\text{S}(s) + \square \, \text{H}_2(g) \][/tex]
We can follow these steps:
1. Identify each element involved: We have silver (Ag), hydrogen (H), and sulfur (S).
2. Balance the silver atoms:
- There are 2 silver atoms in the product (Agâ‚‚S), so we need 2 atoms of silver on the reactant side.
3. Balance the sulfur atoms:
- There is 1 sulfur atom in Hâ‚‚S and 1 sulfur atom in Agâ‚‚S, which are already balanced.
4. Balance the hydrogen atoms:
- There are 2 hydrogen atoms in Hâ‚‚S on the reactant side, and they form 1 molecule of Hâ‚‚ gas on the product side, which balances the hydrogen atoms.
So the balanced equation is:
[tex]\[ 2 \, \text{Ag}(s) + 1 \, \text{H}_2\text{S}(g) \rightarrow 1 \, \text{Ag}_2\text{S}(s) + 1 \, \text{H}_2(g) \][/tex]
Therefore, the coefficients that balance the tarnishing reaction equation are:
[tex]\[2, 1, 1, 1 \][/tex]
Hence, the balanced chemical equation is:
[tex]\[ 2 \, \text{Ag}(s) + 1 \, \text{H}_2\text{S}(g) \rightarrow 1 \, \text{Ag}_2\text{S}(s) + 1 \, \text{H}_2(g) \][/tex]
The coefficients are [tex]\( 2 \)[/tex] for Ag, [tex]\( 1 \)[/tex] for Hâ‚‚S, [tex]\( 1 \)[/tex] for Agâ‚‚S, and [tex]\( 1 \)[/tex] for Hâ‚‚.
