How many grams of silver could be plated out on a shield by electrolysis of a solution containing `Ag^(+)` ions for a period of 4 hours at a current strength of 8.5 amperes? [Molar mass of `Ag`=107.8g]

How many grams of silver could be plated out on a serving tray by electrolysis of a solution containing silver in +1 oxidation state for a period of 8.0 h at a current of 8.46 A ? What is the area of the tray if the thickness of the silver plating is 0.00254 cm? Density of silver is 10.5 g// cm^(3) .

State and explain Faraday 's laws of electrolysis. How many grams of silver will be deposited by the electrolysis of silver nitrate solution with a current of 5 amperes for 10 minutes.

How many mole of HCl are required to prepare one litre of buffer solution (conataining NaCN+HCl) of ph 8.5 using 0.01 g formula weight of NaCN(K_(HCN)=4.1xx10^(-10)?

Three electrolytic cells A,B and C containing solutions of zinc sulphate, silver nitrate and copper sulphate, respectively are connected in series. A steady current of 1.5 A was passed through them until 1.45g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited in the concerned cells? ( Atomic mass of Ag= 108, Zn = 65.4, Cu = 63.5)

Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid were connected in a series. A steady current of 2.5 A was passed through them till 1.078 g of silver was deposited ( Ag = 107.8 g //" mol" ) (a) How much electricity was consumed? (b) What is the weight of oxygen gas liberated during the reaction?

How much time is required for 1.5 g Ag to deposit when 1.50 A current is passed through an electrolytic cell containing AgNO_(3) solution with inert electrodes?

A current of 0.5 amperes was passed through a solution of silver nitrate for six min. Find the mass of silver deposited. (Atomic mass of Ag = 108 )

Electric current is passed through two cells A and B in series. Cell A contains aqueous solution of Ag_(2) SO_(4) and platinum electrodes. Cell B contains aqueous solution of CuSO_(4) and copper electrodes. The current is passed till 1.6g of oxygen is liberated at the anode in cell A. Calculate the quantities of copper and silver deposited at the cathode of the two cells. [ Atomic mass, O = 16, Cu 63.5, Ag = 108]

State and explain Faraday 's laws of electrolysis. A current of 6 amperes is passed through a solution of Ag NO_3 for 20 minutes. 8 gm of silver is deposited. Find out the electrochemical equivalent of silver.

State and explain Faraday 's laws of electrolysis. When a current of 6 ampere strength is passed through AgNO_3 solution for 10 minutes, 4 gms of silver is deposited. Find out the electrochemical equivalent of silver.