Which of the following statements is/are correct about the reaction.
`H_(2)SO_(4)+Cu_(3)P+Cr_(2)O_(7)^(2-)toCuSO_(4)+H_(3)PO_(4)+2Cr^(3+)`

Options

A. The number of moles of `Cr_(2)O_(7)^(2-)` required to oxidise 6 " mol of "`Cu_(3)P` to `CuSO_(4)` and `H_(2)PO_(4)` is 11 mol.
B. The number of moles of `H_(2)SO_(4)` used in the reaction is
`62`.
C. The number of moles of `Cr_(2)(SO_(4))_(3)` formed in the reaction is 11.
D. The number of moles of `K_(2)SO_(4)` formed in the reaction is 11.

Explanation

To analyze the reaction \( H_2SO_4 + Cu_3P + Cr_2O_7^{2-} \rightarrow CuSO_4 + H_3PO_4 + 2Cr^{3+} \), we will break it down step by step to determine the correctness of the statements provided.

### Step 1: Identify the Oxidation and Reduction Processes
1. **Oxidation**: In the reaction, copper (Cu) in \( Cu_3P \) is oxidized. The oxidation state of Cu changes from 0 in \( Cu_3P \) to +2 in \( CuSO_4 \).
- Each \( Cu \) atom goes from 0 to +2, thus:
\[ Cu_3P \rightarrow 3Cu^{2+} + H_3PO_4 \]
- The total charge change for Cu is +6 (3 Cu atoms).

2. **Reduction**: The dichromate ion \( Cr_2O_7^{2-} \) is reduced to \( Cr^{3+} \). The oxidation state of Cr changes from +6 in \( Cr_2O_7^{2-} \) to +3 in \( Cr^{3+} \).
- The reaction can be represented as:
\[ Cr_2O_7^{2-} + 6e^- + 14H^+ \rightarrow 2Cr^{3+} + 7H_2O \]

### Step 2: Balancing the Reactions
- **Oxidation Half-Reaction**:
\[ Cu_3P + 8H^+ \rightarrow 3Cu^{2+} + H_3PO_4 + 4H_2O \]
(Total of 11 electrons transferred)

- **Reduction Half-Reaction**:
\[ Cr_2O_7^{2-} + 6e^- + 14H^+ \rightarrow 2Cr^{3+} + 7H_2O \]
(Total of 6 electrons transferred)

### Step 3: Combine the Half-Reactions
To balance the overall reaction, we need to ensure that the number of electrons lost in oxidation equals the number of electrons gained in reduction.

1. Multiply the oxidation half-reaction by 6 and the reduction half-reaction by 11 to balance the electrons:
\[ 6Cu_3P + 11Cr_2O_7^{2-} + 124H^+ \rightarrow 18Cu^{2+} + 6H_3PO_4 + 22Cr^{3+} + 53H_2O \]

### Step 4: Analyze the Statements
1. **Statement A**: The number of moles of \( Cr_2O_7^{2-} \) required to oxidize 6 moles of \( Cu_3P \) is 11 moles.
- **Correct**: From the balanced equation, 11 moles of \( Cr_2O_7^{2-} \) are indeed required.

2. **Statement B**: The number of moles of \( H_2SO_4 \) used in the reaction.
- **Correct**: Since \( H_2SO_4 \) provides \( H^+ \) ions, and we have 124 \( H^+ \) ions, we need 62 moles of \( H_2SO_4 \).

3. **Statement C**: The number of moles of \( Cr_2SO_4 \cdot 3 \) formed in the reaction.
- **Correct**: With 22 \( Cr^{3+} \) ions, \( \frac{22}{2} = 11 \) moles of \( Cr_2SO_4 \cdot 3 \) are formed.

4. **Statement D**: The number of moles of \( K_2SO_4 \) used in the reaction.
- **Correct**: The difference in sulfate ions is 11 moles, leading to the formation of 11 moles of \( K_2SO_4 \).

### Conclusion
All four statements A, B, C, and D are correct.