`1` mol each of `AG AgBO_3, CuSO_4` and `AICI_3` is electrolysed. The number of faradays rewuired is in the ration of:

1 mol each of AgNO_3, CuSO_4 and AICI_3 is electrolyzed. The number of faradays required is in the ration of:

If 1 mol electron is passed through each of AgNO_(3) , CuSO_(4) and AiCl^(3) , solutions , calculate the ratio of number of moles of Ag , Cu and Al formed at cathode .

Assertion: One faraday can deposit one mol each of Ag, Cu and Al. Reason: Number of electrons in one coulomb of current is not a constant.

An electric charge of 5 Faradays is passed through three electrolytes AgNO_3, CuSO_4 and FeCl_3 solution. The grams of each metal liberted at cathode will be

An electric charge of 5 Faradays is passed through three electrolytes AgNO_3, CuSO_4 and FeCl_3 solution. The grams of each metal liberted at cathode will be

An electric charge of 5 Faradays is passed through three electrolytes AgNO_3, CuSO_4 and FeCl_3 solution. The grams of each metal liberted at cathode will be

If 3F of electrictiy is passed through the solutions of AgNO_3, CuSO_4 and Auc=CL_3 , the molar ration of the cations deposited at the cathode is .

If 3F of electricity is passed through the solutions of AgNO_3, CuSO_4 and AuCL_3 , the molar ration of the cations deposited at the cathode is .

During electrolysis of 1 litre of aq. CuSO_4 , the P^(H) of the solution is changed from 5.0 to 4.3 . Then the number of faradays consumed in the process is (x xx 10^(-4)) , here , (x + y) = ?