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?

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 ?

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 .)

A current of 0.5 ampere when passed through AgNO_(3) solution for 193 seconds deposited 0.108 g. of silver. The equivalent weight of Ag is

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

3 ampere current was passed through an aqueous solution of an unknown salt of Pd for 1 hr 2.977 g of Pd^(n+) was deposited at cathode. Find the value of n. (atomic weight of Pd is 106.4)

When same quantity of electricity is passed through aqueous AgNO_(3) and H_(2)SO_(4) solutions connected in series, 5.04 xx 10^(-2) g of H_(2) is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen =1.008, silver =108)

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) )

An electric current is passed through two solutions (a) AgNO_3 and (b) a solution of 10g of blue vitriol in 500 ml water, using Pt separately After 30 min , it was found 1.307 g Ag was deposited. What was the concentration of Cu^(2+) after electrolysis?

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolyte cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent the equivalent mass and 96500 C is called the faraday constant. Faraday (96500 C) is the charge of 1 mole electron i.e., 6.023 xx 10^(23) electrons, it is used to liberate on gram equivalent of the substance. The platinum electrodes were immersed in a solution of cupric sulphate (CuSO_4) and electric current is passed through the solution. After sometimes, it was observed that the colour of copper sulphate disappeared with evolution of a gas at the electrode. The colourless solution contains.

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolyte cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent the equivalent mass and 96500 C is called the faraday constant. Faraday (96500 C) is the charge of 1 mole electron i.e., 6.023 xx 10^(23) electrons, it is used to liberate on gram equivalent of the substance. The passage of current liberates H_2 at cathode and Cl_2 at anode. The solution is