Question

__Cu+__AgNO3–>__Ag+__Cu(NO3)2
Balance

Answer 1

To balance the chemical equation \( \text{Cu} + \text{AgNO}_3 \rightarrow \text{Ag} + \text{Cu(NO}_3\text{)}_2 \), we can follow these steps:

1. Write down the unbalanced equation:
\[
\text{Cu} + \text{AgNO}_3 \rightarrow \text{Ag} + \text{Cu(NO}_3\text{)}_2
\]

2. Count the number of atoms of each element on both sides of the equation:
- **Reactants**:
- Cu: 1
- Ag: 1
- N: 1
- O: 3
- **Products**:
- Cu: 1
- Ag: 1
- N: 2 (from \(\text{Cu(NO}_3\text{)}_2\))
- O: 6 (from \(\text{Cu(NO}_3\text{)}_2\))

3. To balance the nitrogens, note that there are 2 nitrogen atoms in the product. Therefore, we will need 2 silver nitrate molecules:
\[
\text{Cu} + 2\text{AgNO}_3 \rightarrow 2\text{Ag} + \text{Cu(NO}_3\text{)}_2
\]

4. Now, recount the number of atoms:
- **Reactants**:
- Cu: 1
- Ag: 2
- N: 2
- O: 6 (from \(2 \times 3\))
- **Products**:
- Cu: 1
- Ag: 2
- N: 2
- O: 6

Both sides are now equal, and the equation is balanced.

The balanced equation is:
\[
\text{Cu} + 2\text{AgNO}_3 \rightarrow 2\text{Ag} + \text{Cu(NO}_3\text{)}_2
\]