Consider the reactions shown below :

Which of the follwoing statements is false?

Options

A. Silver chromate (VI) has the formula `Ag_(2)CrO_(4)`.
B. The minimum mass of zinc required to reduce 0.1 mole of `Cr^(3+)` to `Cr^(2+)` is 6.54g.
C. The conversion of `CrO_(4)^(2-)` into `Cr_(2)O_(7)^(2-)` is not a redox reaction.
D. The equation `Cr_(2)O_(7)^(2-) + 14H^(+)+6Fe^(2+)rarr2Cr^(3+)+7H_(2)O` correctly describes the reduction of `Cr_(2)O_(7)^(2-)` by acidified `FeSO_(4)`.

Answer

A, C, D

Explanation

(A) Formula of silver chromate (VI) will be `Ag_(2)CrO_(4)`
(B) Minimum mass of zinc required for reduction of 0.1 mole of `Cr^(3+)` to `Cr^(2+)=(0.1)/(2)` moles of Zn
(v.f. of Zn = 2 & v.f. of `Cr^(3+)=1`) `" " (6.54)/(2)g=3.27g`
(c) `CrO_(4)^(2-)hArrCr_(2)O_(7)^(2-)`
in both ions, chromium is in +6 oxidation state.
(D) Given reaction is correct.