A current of 1.50A was passed through an electrolytic cell containing `AgNO_3` solution with inert electrodes. The mass of silver deposited to cathode was 1.50g. How long did the current flow? (atomic mass of Ag = 108u, 1F = 96500C).

Three electrolytic cells A, B and C containing electrolytes ZnSO_4 , AgNO_3 and CuSO_4 respectively were connected in series. A steady current of 1.5A was passed through them. 1.45g Ag were deposited at the cathode of cell B. How long did the current flow?(Atomic mass of Cu = 63.5u, Zn = 65.3u, Ag = 108u.)

A current of 0.50 ampere is passed for 30 minutes through a voltameter containing copper sulphate solution. Calculate the mass of Cu deposited at the cathode. Given that atomic mass of Cu is 63.0amu.

Two electrolytic cell containing AgNO_3 solution and dilute H_2SO_4 solution were connected in series. A steady current of 2.5 ampre was passed through them till 1.078g of silver was deposited. (Ag = 108 u, IF = 96500 C). How much electricity was consumed?

Two electrolytic cell containing AgNO_3 solution and dilute H_2SO_4 solution were connected in series. A steady current of 2.5 ampere was passed through them till 1.078g of silver was deposited. (Ag = 108 u, IF = 96500 C). What was the weight of oxygen gas liberated?

Three electolytic 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 throught 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?

A solution of CuSO_4 is electolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode?

Three electrolytic cells A, B and C containing electrolytes ZnSO_4 , AgNO_3 and CuSO_4 respectively were connected in series. A steady current of 1.5A was passed through them. 1.45g Ag were deposited at the cathode of cell B.What mass of copper and zinc were deposited? (Atomic mass of Cu = 63.5u, Zn = 65.3u, Ag = 108u.)

How many moles of mercury will be produced by electrolysing 1.0M Hg(NO_3)_2 . Solution with a current of 2.00A for 3 hours? (molar mass of Hg(NO_3)_2=200.6gmol^(-1) .

Silver crystallises in fcc lattice. If edge length of the cell is 4.07xx10^-8 cm and density is 1.05 g cm^-3 . Calculate the atomic mass of silver.