Assertion: In the redox reaction `8H^(+)(aq)+4NO_(3)^(-)+6Cl^(-)+Sn(s) rarr SnCl_(6)^(2-)+4NO_(2)+4H_(2)O`. the reducing agent is `Sn(s)`.
Reason In balacing half-reaction, `S_(2)O_(3)^(2-) rarr S(s)`, the number of electrons added on the left is `4`.

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
B. Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-1
C. Statement-1 is True, Statement-2 is False.
D. Statement-1 is False, Statement-2 is True.

Explanation

To solve the question, we need to analyze the assertion and reason provided in the context of the redox reaction:

**Assertion:** In the redox reaction \(8H^+(aq) + 4NO_3^{-} + 6Cl^{-} + Sn(s) \rightarrow SnCl_6^{2-} + 4NO_2 + 4H_2O\), the reducing agent is \(Sn(s)\).

**Reason:** In balancing the half-reaction, \(S_2O_3^{2-} \rightarrow S(s)\), the number of electrons added on the left is 4.

### Step-by-Step Solution:

1. **Identify the Oxidation States:**
- In the reaction, we need to determine the oxidation states of the elements involved.
- For \(Sn(s)\), the oxidation state is 0.
- In \(SnCl_6^{2-}\), the oxidation state of \(Sn\) can be calculated as follows:
- Each \(Cl\) has an oxidation state of -1, so for 6 \(Cl\), the total is -6.
- Therefore, \(Sn\) must have an oxidation state of +4 to balance the -6 from \(Cl\) to give a total charge of -2.

2. **Determine the Role of \(Sn\):**
- Since \(Sn\) goes from an oxidation state of 0 to +4, it is losing electrons and is therefore oxidized.
- The species that gets oxidized is the reducing agent. Hence, \(Sn(s)\) is indeed the reducing agent in this reaction.

3. **Analyze the Reason:**
- The reason discusses the half-reaction involving \(S_2O_3^{2-}\) and its reduction to \(S(s)\).
- In this half-reaction, \(S\) in \(S_2O_3^{2-}\) has an oxidation state of +2. To reduce it to elemental sulfur (0 oxidation state), 2 electrons are required for each sulfur atom.
- Since there are 2 sulfur atoms in \(S_2O_3^{2-}\), a total of 4 electrons are needed for the complete reduction.

4. **Conclusion:**
- The assertion is correct because \(Sn(s)\) is the reducing agent.
- The reason is also correct in stating that 4 electrons are needed, but it does not explain why \(Sn(s)\) is the reducing agent in the given reaction.

### Final Answer:
- **Assertion is correct.**
- **Reason is correct but does not explain the assertion.**