In the chemical reaction,
`Ag_(2)O+H_(2)O+2e^(-) to 2Ag+2OH^(-)`

Options

A. water is oxidised
B. Silver is oxidised
C. Silver is reduced
D. Hydrogen is reduced

Answer

To solve the question regarding the chemical reaction \( \text{Ag}_2\text{O} + \text{H}_2\text{O} + 2e^- \rightarrow 2\text{Ag} + 2\text{OH}^- \), we need to analyze the oxidation states of the elements involved and determine which species is oxidized and which is reduced.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- Reactants: \( \text{Ag}_2\text{O} \), \( \text{H}_2\text{O} \), and \( 2e^- \)
- Products: \( 2\text{Ag} \) and \( 2\text{OH}^- \)

2. **Determine the Oxidation States**:
- In \( \text{Ag}_2\text{O} \):
- Let the oxidation state of silver (Ag) be \( x \).
- The oxidation state of oxygen (O) is \(-2\).
- The compound is neutral, so:
\[ 2x - 2 = 0 \implies 2x = 2 \implies x = +1 \]
- Therefore, in \( \text{Ag}_2\text{O} \), silver is in the +1 oxidation state.

- In the product \( 2\text{Ag} \):
- The oxidation state of silver in its elemental form is \( 0 \).

3. **Analyze Changes in Oxidation States**:
- Silver changes from +1 in \( \text{Ag}_2\text{O} \) to 0 in \( 2\text{Ag} \).
- This indicates that silver is gaining electrons (2 electrons are added), which means it is being reduced.

4. **Determine the Role of Other Species**:
- Water (\( \text{H}_2\text{O} \)) does not change its oxidation state; it remains as \( H^+ \) and \( OH^- \).
- The hydroxide ion (\( \text{OH}^- \)) is formed, but does not indicate oxidation or reduction in this context.

5. **Conclusion**:
- Since silver is reduced (gaining electrons), the correct answer is that silver is reduced.

### Final Answer:
The correct option is **Option 3: Silver is reduced**.