Two electrolytic cells are connected in series containing `CuSO_(4)` solution and molten `AlCl_(3)`. If in electrolysis 0.4 moles of 'Cu' are deposited on cathode of first cell. The number of moles of 'Al' deposited on cathode of the second cell is

A constant electric current flows for 4 hours through two electrolytic cells connectedin series. Onecontain AgNO_3 ssolutionandsecondcontains CuCl_2 solution. During this time, 4 grams of Ag are deposited in the first cell: How many grams of Cu are deposited in the second cell?

If 36g of Al is deposited at the cathode the number of moles of electrons used is.

If 36 g. of Al is deposited at the cathode, the number of moles of electrons used is

Two electrolytic cells containing CuSO_(4) and AgNO_(3) respectively are connected in series and a current is passed through them until 1 mg of copper is deposited in the first cell. The amount of silver deposited in the second cell during this time is approximately [Atomic weights of copper and silver are respectively 63.57 and 107.88 ]

The same quantity of electricity is passed through two cells one containing AlCl3 solution and the other containing ZnCl2 solution. If 0.04 mole of Al is produced in the first cell, the number of moles of Zn produced in the second cell will be

Exactly 0.4 faraday of charge is passed through three electrolytic cells connected in series, first containing AgNO_(3) , second CuSO_(4) while third containing FeCl_(3) solution. How many grams of each metal will be deposited assuming only cathodic reaction in each cell ?