Which of the following statements is`//`are correct?
In the reaction `xCu_(3)P+yCr_(2)O_(7)^(2-)rarrCu^(2+)+H_(3)PO_(4)+Cr^(3+)`

Options

A. `Cu` in `Cu_(3)P` is oxidised to `Cu^(2+)` whereas `P` in `Cu_(3)P` is also oxidised to `PO_(4)^(3-)`.
B. `Cu` in `Cu_(3)P` is oxidised to `Cu^(2+)` whereas `P` in `Cu_(3)P` is reduced to `H_(3)PO_(4)`.
C. In the conversion of `Cu_(3)P` to `Cu^(2+)` and `H_(3)PO_(4),11 "electrons" are involved.
D. The value of `x` is `6`

Explanation

To solve the question regarding the redox reaction \( xCu_3P + yCr_2O_7^{2-} \rightarrow Cu^{2+} + H_3PO_4 + Cr^{3+} \), we will analyze the oxidation states, identify oxidation and reduction processes, and balance the reaction.

### Step 1: Determine the oxidation states
1. **Copper in \( Cu_3P \)**:
- In \( Cu_3P \), copper (Cu) has an oxidation state of +1.
- Phosphorus (P) has an oxidation state of -3.

2. **Dichromate ion \( Cr_2O_7^{2-} \)**:
- Chromium (Cr) has an oxidation state of +6.
- Oxygen (O) has an oxidation state of -2.

3. **Products**:
- In \( Cu^{2+} \), copper has an oxidation state of +2.
- In \( H_3PO_4 \), phosphorus has an oxidation state of +5.
- In \( Cr^{3+} \), chromium has an oxidation state of +3.

### Step 2: Identify oxidation and reduction
- **Oxidation**:
- Copper is oxidized from +1 in \( Cu_3P \) to +2 in \( Cu^{2+} \).
- Phosphorus is oxidized from -3 in \( Cu_3P \) to +5 in \( H_3PO_4 \).

- **Reduction**:
- Chromium is reduced from +6 in \( Cr_2O_7^{2-} \) to +3 in \( Cr^{3+} \).

### Step 3: Analyze the statements
1. **Statement 1**: "Copper in \( Cu_3P \) is oxidized to \( Cu^{2+} \) whereas phosphorus in \( Cu_3P \) is also oxidized to \( PO_4^{3-} \)."
- **Correct**: Both copper and phosphorus undergo oxidation.

2. **Statement 2**: "Copper in \( Cu_3P \) is oxidized to \( Cu^{2+} \) whereas phosphorus in \( Cu_3P \) is reduced to \( H_3PO_4 \)."
- **Incorrect**: Phosphorus is oxidized, not reduced.

3. **Statement 3**: "In the conversion of \( Cu_3P \) to \( Cu^{2+} \) and \( H_3PO_4 \), 11 electrons are involved."
- **Correct**: This can be verified by balancing the half-reaction.

4. **Statement 4**: "The value of \( x \) in the balanced equation is 6."
- **Correct**: After balancing the complete reaction, we find \( x = 6 \).

### Step 4: Conclusion
- The correct statements are 1, 3, and 4.

### Final Answer
The correct statements are:
1. Copper in \( Cu_3P \) is oxidized to \( Cu^{2+} \) whereas phosphorus in \( Cu_3P \) is also oxidized to \( PO_4^{3-} \).
3. In the conversion of \( Cu_3P \) to \( Cu^{2+} \) and \( H_3PO_4 \), 11 electrons are involved.
4. The value of \( x \) in the balanced equation is 6.