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.

Answer

A, B, C, D

Explanation

In `(overset(+1xx3)(Cu_(3))P^(-3))`,
`Cr^(1+)to3Cu^(2+)3e^(-)` ("oxidation")`
`underline(underset(x=-3)(P^(3-))toundersetunderset(x=5)(x+x-8=0)(H_(3)PO_(4)))`
`underline(4H_(2)O+Cu_(3)Pto3Cu^(2+)+H_(2)PO_(4)+11e^(-)+5H^(o+))`
Reduction:
`Cr_(2)O_(7)^(2-)+6e^(2-)+14H^(o+)to2Cr^(3+)+7H_(2)O` ..(ii)
Multiply equation (i) and 6 and equation (ii) by 11, net redox equation is:
(ii). Number of moles of `H_(2)SO_(4)` used `=62H_(2)SO_(4)`
`(=124H^(o+)=62SO_(4)^(2-))`
Number of moles of `CuSO_(4)` formed`=18CuSO_(4)(=18SO_(4)^(2-))` ltBrgt Number of moles of `Cr_(2)(SO_(4))_(3)` formed`=11Cr_(2)(SO_(4))_(3)` ltBrgt `(=33SO_(4)^(2-))`
Total number of `SO_(4)^(2-)` ion in reactant `=62`
Total number of `SO_(4)^(2-)` ion in product`=18+33=51`
Rest 11 " mol of "`SO_(4)^(2-)` ion in the reactant react with `(11)/(2mol)` of `K^(o+)` ion to give 11 " mol of "`K_(2)SO_(4)`.
Net redox reaction is:
`6Cu_(3)P+11K_(2)Cr_(2)O_(7)+62H_(2)SO_(4)to18CuSO_(4)`
`+6H_(3)PO_(4)+43H_(2)O+11Cr_(2)(SO_(4))_(3)+11K_(2)SO_(4)`