Question

Balance this
Ag2O+S —>

Answer 1

To balance the chemical equation for the reaction between silver oxide (Ag₂O) and sulfur (S), follow these steps:

1. Write down the unbalanced equation:
\[
\text{Ag}_2\text{O} + \text{S} \rightarrow
\]

2. Identify the products of the reaction. When silver oxide reacts with sulfur, it typically produces silver sulfide (Ag₂S) and oxygen (O₂). Thus, the products are:
\[
\text{Ag}_2\text{S} + \text{O}_2
\]

3. The unbalanced equation now looks like this:
\[
\text{Ag}_2\text{O} + \text{S} \rightarrow \text{Ag}_2\text{S} + \text{O}_2
\]

4. Now, balance the equation. Start with silver (Ag):
- We have 2 Ag on the left from Ag₂O, and we have 2 Ag in Ag₂S. So, Ag is balanced.

5. Next, balance sulfur (S):
- We have 1 S on the left and 1 S in Ag₂S, which is already balanced.

6. Finally, balance oxygen (O):
- We have 1 O in Ag₂O on the left and 2 O in O₂ on the right. To balance, we need 2 Ag₂O on the left to provide 2 O:
\[
2\text{Ag}_2\text{O} + \text{S} \rightarrow \text{Ag}_2\text{S} + \text{O}_2
\]

7. Update the S and balance:
\[
2\text{Ag}_2\text{O} + \text{2S} \rightarrow 2\text{Ag}_2\text{S} + \text{O}_2
\]

The balanced equation is:
\[
2\text{Ag}_2\text{O} + \text{2S} \rightarrow 2\text{Ag}_2\text{S} + \text{O}_2
\]

This equation is now balanced with respect to the number of atoms of each element on both sides.