Consider the following standard reduction potentials:-
`{:(Fe^(2+)+2e^(-)hArrFe,,,E^(@) =- 0.41V),(Ag^(+)+e^(-)hArrAg,,,E^(+)=0.80V),(O_(2)+2H_(2)O+4e^(-)hArr4OH^(-),,,E^(@)=0.40V):}`
What would happens if a block of silver metal is connected to a buried iron pipe via a wire:-

Options

A. The silver metal would corrode, a current would be produced in the wire, and `O_(2)` would be reduced on the surface of the iron pipe.
B. The silver metal would corrode, a current would be produced in the wire, and `Fe^(2+)` would be reduced on the surface of the iron pipe.
C. The iron pipe would corrode, a current would be produced in the wire, and `Ag^(+)` would be reduced on the surface of the silver metal.
D. The iron pipe would corrode, no current would be produced in the wire, and `O_(2)` would be reduced on the surface of the iron pipe.

Answer

To solve the problem, we need to analyze the standard reduction potentials given and determine what happens when a block of silver metal is connected to a buried iron pipe.

### Step-by-Step Solution:

1. **Identify the Standard Reduction Potentials:**
- For Iron: \( \text{Fe}^{2+} + 2e^- \leftrightarrow \text{Fe}, \quad E^\circ = -0.41 \, \text{V} \)
- For Silver: \( \text{Ag}^+ + e^- \leftrightarrow \text{Ag}, \quad E^\circ = +0.80 \, \text{V} \)
- For Oxygen: \( \text{O}_2 + 2\text{H}_2\text{O} + 4e^- \leftrightarrow 4\text{OH}^-, \quad E^\circ = +0.40 \, \text{V} \)

2. **Determine the Tendency to Get Oxidized or Reduced:**
- The more positive the standard reduction potential, the greater the tendency for that species to be reduced.
- Silver has the highest reduction potential (+0.80 V), indicating it has a strong tendency to be reduced.
- Iron has a lower reduction potential (-0.41 V), indicating it has a greater tendency to be oxidized.

3. **Analyze the Reaction:**
- When silver is connected to iron, the silver will attract electrons and get reduced, while iron will lose electrons and thus get oxidized.
- The reaction for iron can be represented as:
\[ \text{Fe} \rightarrow \text{Fe}^{2+} + 2e^- \]
- This means that iron will corrode, losing electrons to the silver.

4. **Conclusion:**
- Since iron has a lower reduction potential, it will corrode when connected to silver. The silver will not corrode because it is being reduced instead.
- Therefore, the correct conclusion is that the iron pipe will corrode, and a current will be produced in the wire as electrons flow from iron to silver.

### Final Answer:
The iron pipe would corrode, and a current would be produced in the wire as Ag⁺ gets reduced on the surface of the silver metal.

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