Given `E_(Ag^(+)//Ag)^(@)=+0.80 V, E_(Cu^(2+)//Cu)^(@)=+0.34 V, E_(Fe^(3+)//Fe^(2+))^(@)=+0.76 V, E_(Ce^(4+)//Ce^(3+))^(@)=+1.60 V`
Which of the following statements is not correct ?

Options

A. `Fe^(3+)` does not oxidise `Ce^(3+)`.
B. Cu reduces `Ag^(+) ` to Ag.
C. Ag will reduce `Cu^(2+)` to Cu.
D. `Fe^(3+)` reduces `Cu^(2+)` to Cu.

Explanation

To determine which statement is not correct regarding the given standard reduction potentials, we will analyze each ion's ability to oxidize another based on their reduction potentials.

### Given Data:
- \( E^\circ (Ag^+ // Ag) = +0.80 \, V \)
- \( E^\circ (Cu^{2+} // Cu) = +0.34 \, V \)
- \( E^\circ (Fe^{3+} // Fe^{2+}) = +0.76 \, V \)
- \( E^\circ (Ce^{4+} // Ce^{3+}) = +1.60 \, V \)

### Step 1: Identify the strongest oxidizing agent
The strongest oxidizing agent corresponds to the highest standard reduction potential. Here, \( Ce^{4+} \) has the highest potential of \( +1.60 \, V \).

### Step 2: Compare \( Fe^{3+} \) and \( Ce^{4+} \)
- \( E^\circ (Fe^{3+} // Fe^{2+}) = +0.76 \, V \)
- \( E^\circ (Ce^{4+} // Ce^{3+}) = +1.60 \, V \)

Since \( Ce^{4+} \) has a higher reduction potential than \( Fe^{3+} \), \( Fe^{3+} \) cannot oxidize \( Ce^{3+} \).

### Step 3: Compare \( Ag^+ \) and \( Cu^{2+} \)
- \( E^\circ (Ag^+ // Ag) = +0.80 \, V \)
- \( E^\circ (Cu^{2+} // Cu) = +0.34 \, V \)

Here, \( Ag^+ \) can oxidize \( Cu \) since \( Ag^+ \) has a higher reduction potential than \( Cu^{2+} \).

### Step 4: Compare \( Fe^{3+} \) and \( Cu^{2+} \)
- \( E^\circ (Fe^{3+} // Fe^{2+}) = +0.76 \, V \)
- \( E^\circ (Cu^{2+} // Cu) = +0.34 \, V \)

Since \( Fe^{3+} \) has a higher reduction potential than \( Cu^{2+} \), \( Fe^{3+} \) can oxidize \( Cu \).

### Conclusion:
Based on the analysis:
1. \( Fe^{3+} \) cannot oxidize \( Ce^{3+} \) (correct statement).
2. \( Ag^+ \) can oxidize \( Cu \) (correct statement).
3. \( Fe^{3+} \) can oxidize \( Cu \) (correct statement).

Thus, the statement that is not correct is that **\( Fe^{3+} \) cannot oxidize \( Ce^{3+} \)**.