On passing one faraday of elecricity throuth the electrolytic cells containing `Ag^+ , Ni^(+3)` and `Cr^(+3)` ion solutions, the deposited Ag `(AT. Wt. = 108) Ni (At. Wt = 59 )` and `Cr (At wt. = 52)` is .

On passing 1 Faraday charge through the electrolytic cells containing Ag^(+),Ni^(2+),Cr^(3+) ions solution, the mass of deposited Ag is (At mass = 108 u ), Ni (At mass = 59u) and Cr (At mass = 52U):

One faraday of charge was passed through the electrolytic cells placed in series containing solution of Ag^(+), Ni^(2+) " and " Cr^(3+) respectively. The amount of Ag (At. mass 108), Ni (At. mass 50) and Cr(At. mass 52) deposited will be:

On passing 3 faraday of electricity through the three electrolytic cells connected in series containing Ag^+ , Ca^(2+) and Al^(3+) ions respectively. The molar ratio in which the three metal ions are liberated at the electron is

One Faraday charge was passed through the electrolytic cell placed in series containing solutions of Ag^(+), Ni^(2+) and Cr^(3+) . Then Ag, Ni and Cr deposited will be (Atomic masses , Ag= 108, Ni = 59 and Cr = 52)

On passing 3 faraday of electricity through the three electrolytic cells connected in series containing Ag^+,Ca^(2+) and AI^(3+) ions respectively. The molar ratio in which the three metal ions are liberated at the electrodes is :

0.1 Faraday of current was passed through the electrolytic cell placed in series containing solutions of Ag^(+), Ni^(2+) and Cr^(3+) respectively. The amount of Ag, Ni and Cr deposited will be (at. Mass, Ag=108, Ni=59, Cr=52 )

On passing C ampere of electricity through an electrolyte solution for l secodns, m gram metal deposits on cathode. The eq. wt. of metal is