If equal volume of 1M `KMnO_(4)` and 1M`K_(2)Cr_(2)O_(7)` solution are used to react with `Fe^(2+)` oxidized will be :

If equal volumes of 1 M KMnO_(4) and 1M K_(2)Cr_(2)O_(7) solutions are allowed to oxidise Fe(II) to Fe(III) in acidic medium, then Fe(II) oxidised will be

If equal volumes of 1 M KMnO_(4) and 1M K_(2)Cr_(2)O_(7) solutions are allowed to oxidise Fe(II) to Fe(III) in acidic medium, then Fe(II) oxidised will be

If equal volumes of 0.1 M KMnO_(4) and 0.1 M K_(2)Cr_(2)O_(7) solutions are allowed to oxidise Fe^(2+) to Fe^(3+) in acidic medium, then Fe^(2+) oxidised will be:

If equal volumes of 0.1 M KMnO_(4) and 0.1 M K_(2)Cr_(2)O_(7) solutions are allowed to oxidise Fe^(2+) to Fe^(3+) in acidic medium, then Fe^(2+) oxidised will be:

Ratio of moles of Fe (II) oxidised by equal volumes of equimolar KMnO_(4) and K_(2)Cr_(2)O_(7) solutions in acidic medium will be:

Ratio of moles of Fe (II) oxidised by equal volumes of equimolar KMnO_(4) and K_(2)Cr_(2)O_(7) solutions in acidic medium will be:

State three uses of KMnO_(4) and K_(2)Cr_(2)O_(7) each.

Equal volumes of 1M KMnO_4 and 1M K_2Cr_2O_7 solution are allowed to oxidise Fe^(2+) ions to Fe^(3+) ions in acidic medium. The number of moles of Fe^(2+) ions oxidised in the two cases are in the ratio: