Same amount of current passed through two separate electrolytic cells containing `FeCl_(3)` and `NiSO_(4)` solutions respectively if `112g` of `Fe` deposited in first cell then amount of nickel deposited is (Molar mass of `Fe=56`, Molar mass of `Ni=59`)

If same quantity of electricity is passed through three electrolytic cells containing FeSO_(4),Fe_(2)(SO_(4))_(3) , and Fe(NO_(3))_(3) , then

If same quantity of electricity is passed through three electrolytic cells containing FeSO_(4),Fe_(2)(SO_(4))_(3) , and Fe(NO_(3))_(3) , then

The same amount of electricity was passed through molten cryolite containing Al_(2)O_(3) and NaCl. If 1.8 g of Al were liberated in one cell, the amount of Na liberated in the other cell is

A current of 12 A is passed through an electrolytic cell containing aqueous NiSO_4 solution. Both Ni and H_2 gas are formed at the cathode. The current efficiency is 60%. What is the mass of nickel deposited on the cathode per hour?

(a) A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO_(4) and ZnSO_(4) until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow ? Calculate the mass of Zn deposited at the cathode of cell Y (Molar mass : Fe= 56 g mol^(-1) Zn-65.3g mol^(-1) , 1F -96500 C mol^(-1) ) (b) In the plot of molar conductivity (wedge_(m)) vs Square root of concentration (c^(1//2)) , following curves are obtained for two electrolytes. A and B: Answer the following : (i) Predict the nature of electrolytes A and B. (ii) What happens on extrapolation of wedge_(m) to concentration approaching zero for electrolytes A and B ?

A current of 1.50 A was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The weight of silver deposited was 1.50g . How long did the current flow ? (Molar mass of Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1) ).

An electric current is passed through two voltameters connected in series and containing CuSO_4 and AgNO_3 solutions respectively. The masses of copper and silver deposited are 0.424 g and 1.44 g respectively. Find the equivalent mass of silver if that of copper is 31.75.

How long does it take to deposit 100 g of Al from an electrolytic cell containing Al_(2)O_(3) using a current of 125 ampere ?

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):

3 faraday electricity was passed through the three electrolytic cells connected in series containing Ag^(+)Ca^(2+) and Al^(+3) ions respectively. The molar ration in which the three metl ions are liberated at the electrodes is :