Select the correct statement if-
`E_(Mg^(2+)//Mg)^(@)=-2.4V, E_(Sn^(4+)//Sn^(2+))^(@)=0.1V, E_(MnO_(4)^(-),H^+//Mn^(2+))^(@)=1.5V, E_(I_(2)//I^(-))^(@)=0.5V`

Options

A. `MnO_(4)^(-)` is the strongest oxidizing agent and Mg is the strongest reducing agent.
B. `Sn^(4+)+2I^(-)toSn^(2+)+I_(2)` is a spontaneous reaction.
C. `Mg^(2+)+Sn^(2+)toMg+Sn^(4+)` is a spontaneous reaction.
D. Here, weakest oxidizing agent is `Sn^(4+)` and weakest reducing agent is `Mn^(2+)`

Explanation

To solve the question, we need to analyze the given standard reduction potentials and determine the validity of each statement based on those potentials.

### Step-by-Step Solution:

1. **Identify the Given Standard Reduction Potentials:**
- \( E^\circ (Mg^{2+}/Mg) = -2.4 \, V \)
- \( E^\circ (Sn^{4+}/Sn^{2+}) = 0.1 \, V \)
- \( E^\circ (MnO_4^-/Mn^{2+}) = 1.5 \, V \)
- \( E^\circ (I_2/I^-) = 0.5 \, V \)

2. **Determine the Strongest Oxidizing Agent:**
- The strongest oxidizing agent corresponds to the highest positive reduction potential.
- Among the given potentials, \( MnO_4^- \) has the highest reduction potential of \( 1.5 \, V \).
- Therefore, \( MnO_4^- \) is the strongest oxidizing agent.

3. **Determine the Strongest Reducing Agent:**
- The strongest reducing agent corresponds to the lowest (most negative) reduction potential.
- Here, \( Mg^{2+}/Mg \) has the lowest reduction potential of \( -2.4 \, V \).
- Therefore, \( Mg \) is the strongest reducing agent.

4. **Evaluate the First Statement:**
- The first statement claims that \( MnO_4^- \) is the strongest oxidizing agent and \( Mg \) is the strongest reducing agent.
- Based on our analysis, this statement is **correct**.

5. **Evaluate the Second Statement:**
- The second statement claims that the reaction \( Sn^{4+} + 2I^- \rightarrow Sn^{2+} + I_2 \) is spontaneous.
- To determine spontaneity, calculate the standard cell potential \( E^\circ_{cell} \):
- \( E^\circ_{cell} = E^\circ_{reduction} (Sn^{4+}/Sn^{2+}) + E^\circ_{oxidation} (I^-/I_2) \)
- \( E^\circ_{cell} = 0.1 \, V + (-0.5 \, V) = -0.4 \, V \)
- Since \( E^\circ_{cell} < 0 \), this reaction is **not spontaneous**. Thus, the second statement is **incorrect**.

6. **Evaluate the Third Statement:**
- The third statement claims that the reaction \( Mg^{2+} + Sn^{2+} \rightarrow Mg + Sn^{4+} \) is spontaneous.
- Calculate the standard cell potential:
- \( E^\circ_{cell} = E^\circ_{reduction} (Mg^{2+}/Mg) + E^\circ_{oxidation} (Sn^{2+}/Sn^{4+}) \)
- \( E^\circ_{cell} = (-2.4 \, V) + 0.1 \, V = -2.3 \, V \)
- Since \( E^\circ_{cell} < 0 \), this reaction is **not spontaneous**. Thus, the third statement is **incorrect**.

7. **Evaluate the Fourth Statement:**
- The fourth statement claims that \( Sn^{4+} \) is the weakest oxidizing agent and \( Mn^{2+} \) is the weakest reducing agent.
- The reduction potential for \( Sn^{4+}/Sn^{2+} \) is \( 0.1 \, V \) (which is positive, indicating it is an oxidizing agent).
- The reduction potential for \( Mn^{2+}/Mn \) is not given, but since \( Mn^{2+} \) is derived from \( MnO_4^- \) which has a positive potential, it is not the weakest reducing agent.
- Thus, the fourth statement is **incorrect**.

### Conclusion:
The only correct statement is the first one: **"MnO4- is the strongest oxidizing agent and Mg is the strongest reducing agent."**