`A 500mL` sample of a `0.1M Cr^(3+)` is electrolyzed with a current of `96.5A`. If the remaining `[Cr^(3+)]` is `0.04M` then the duration of process is:-

A 250.0 mL sample of a 0.20M Cr^(3+) is electrolysed with a current of 96.5 A. If the remaining [Cr^(3+)] is 0.1 M, the duration of process is:

A 250.0 mL sample of a 0.20M Cr^(3+) is electrolysed with a current of 96.5 A. If the remaining [Cr^(3+)] is 0.1 M, the duration of process is:

A 250.0 mL sample of a 0.20M Cr^(3+) is electrolysed with a current of 96.5 A. If the remaining [Cr^(3+)] is 0.1 M, the duration of process is:

A 250 mL sample of 0.20MCr^(3+) is electrolysed with a current of 96.5 A. If the remaining concentration of Cr^(3+) ions is 0.1 M, the duration of electrolysis is (Atomic mass of Cr=52)

The number of moles of the solute present in 500 ml of 0.04 M solution is:

Volume of 0.1 M K_2Cr_2O_7 required to oxidize 35 ml of 0.5 M FeSO_4 solution is