A : `2 F^(-) + Cl_(2) to 2 Cl^(-) + F_(2)` is a reaction having `Delta G^0 = -ve` .
R : `Cl_(2)` is better oxidizing agent than `F_(2)` .

Options

A. If both Assertion & Reason are true and the reason is the correct explanation of the assertion , then mark (1)
B. If both Assertion & Reason are true but the reason is not the correct explanation of the assertion , then mark (2)
C. If Assertion is true statement but Reason is false , then mark (3)
D. If both Assertion and Reason are false statements , then mark (4)

Answer

To solve the assertion and reason question, we will analyze both the assertion (A) and the reason (R) step by step.

### Step 1: Analyze the Assertion (A)
The assertion states that the reaction:
\[ 2 F^{-} + Cl_{2} \rightarrow 2 Cl^{-} + F_{2} \]
has a standard Gibbs free energy change (\( \Delta G^0 \)) that is negative.

1. **Identify the oxidation and reduction**:
- In this reaction, \( Cl_{2} \) is being reduced to \( Cl^{-} \) (going from oxidation state 0 to -1).
- \( F^{-} \) is being oxidized to \( F_{2} \) (going from oxidation state -1 to 0).

2. **Determine the Gibbs free energy change**:
- The Gibbs free energy change (\( \Delta G^0 \)) is related to the cell potential (\( E^0 \)) by the equation:
\[ \Delta G^0 = -nFE^0 \]
- Here, \( n \) is the number of moles of electrons transferred, and \( F \) is Faraday's constant.

3. **Calculate the standard cell potential (\( E^0 \))**:
- The standard reduction potential for \( Cl_{2} + 2e^{-} \rightarrow 2Cl^{-} \) is approximately \( +1.36 \, V \).
- The standard reduction potential for \( F_{2} + 2e^{-} \rightarrow 2F^{-} \) is approximately \( +2.87 \, V \).
- Since \( F^{-} \) is oxidized, we take the oxidation potential as negative:
\[ E^0 = E^0_{\text{cathode}} (Cl_{2}) + E^0_{\text{anode}} (F_{2}) \]
\[ E^0 = 1.36 \, V + (-2.87 \, V) = -1.51 \, V \]

4. **Evaluate \( \Delta G^0 \)**:
- Since \( E^0 \) is negative, \( \Delta G^0 \) will be positive, which contradicts the assertion that \( \Delta G^0 \) is negative.

**Conclusion for Assertion**: The assertion is **false**.

### Step 2: Analyze the Reason (R)
The reason states that \( Cl_{2} \) is a better oxidizing agent than \( F_{2} \).

1. **Definition of an oxidizing agent**:
- An oxidizing agent is a substance that gains electrons (is reduced) and causes another substance to be oxidized. The strength of an oxidizing agent is determined by its standard reduction potential.

2. **Compare the reduction potentials**:
- The reduction potential for \( Cl_{2} \) is \( +1.36 \, V \).
- The reduction potential for \( F_{2} \) is \( +2.87 \, V \).
- Since \( F_{2} \) has a higher reduction potential than \( Cl_{2} \), \( F_{2} \) is a stronger oxidizing agent than \( Cl_{2} \).

**Conclusion for Reason**: The reason is **false**.

### Final Conclusion
Both the assertion and the reason are false.