A solution of `Ni(NO_(3))_(2)` is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

A solution of CuSO_(4) is electrolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ?

An electrolytic cell contains a solution of Ag_(2)SO_(4) and platinum electrodes. Current is passed until 1.6 g. of O_(2) has been liberated at anode. The amonut of Ag deposited at cathode would be

Aqueous NaCl solution is electrolyzed using platinum electrodes. What is the product formed at cathode?

Three electrolytic cells A,B,C containing solutions of ZnSO_(4) , AgNO_(3) and CuSO_(4) , respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

When an aqueous solution of CuCl_(2) is electrolysed using Pt inert electrodes, the reaction at cathode and anode respectively are

A solution of copper sulphate is electrolysed using a current strength of 3 amp to deposite 60 grams of copper. What is the time taken for the electrolysis?

A current of 19296 C is passed through an aqueous solution of copper sulphate using copper electrodes . What is the mass (in g) of copper deposited at the cathode ? (molar mass of Cu = 63.5 g mol^(-1) )

One ampere of current is passed for 9650 sec. through molten AlCl_(3) . What is the weight is grams of Al deposited at cathode ?

A 0.200M KOH solutions is electrolysed for 1.5 h using a current of 8.00 A. How many moles O_2 were produced at the anode?

A current of 0.25 amp is passed through CuSO_(4) solution for 45 minutes. Calculate the mass of copper deposited on the cathode (At.wt of Cu = 63 .)