A current of 10 A is passed for 80 min and 27 seconds through a cell containing dilute sulfuric acid.
(1) How many moles of oxygen gas will be liberated at the anode ?
(2) Calculate the amount of zinc deposited at the cathode when another cell containing `ZnSO_(4)` solution is connected in series.

A current of 12 A is passed through an electrolytic cell containing aqueous NiSO_4 solution. Both Ni and H_2 gas are formed at the cathode. The current efficiency is 60%. What is the mass of nickel deposited on the cathode per hour?

An electrolytic cell contains a solution of Ag_(2)SO_(4) and have platinum electrodes. A current is passed until 1.6gm of O_(2) has been liberated at anode. The amount of silver deposited at cathode would be

A current was passed for two hour through a solution of an acid that liberated 11.2 litre of oxygen at NTP at anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same time?

(a) A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO_(4) and ZnSO_(4) until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow ? Calculate the mass of Zn deposited at the cathode of cell Y (Molar mass : Fe= 56 g mol^(-1) Zn-65.3g mol^(-1) , 1F -96500 C mol^(-1) ) (b) In the plot of molar conductivity (wedge_(m)) vs Square root of concentration (c^(1//2)) , following curves are obtained for two electrolytes. A and B: Answer the following : (i) Predict the nature of electrolytes A and B. (ii) What happens on extrapolation of wedge_(m) to concentration approaching zero for electrolytes A and B ?

A current of 1 A is possed through a dilute solution of sulphuric acid for some time to liberate 1 g of oxygen. How much hydrogen is liberated during this period? How long was the current passed? Faraday constant = 96500 C mol^(-1) .

The same amount of electricity was passed through molten cryolite containing Al_(2)O_(3) and NaCl. If 1.8 g of Al were liberated in one cell, the amount of Na liberated in the other cell is

How many moles of Pt may be deposited on the cathode when 0.80F of electricity is passed through 1.0M solution of Pt^(4+) ?

In an electrolysis experiment, current was passed for 5h through two cells connected in series. The first cell contains a solution of gold and second contains copper sulphate solution. In the first cell, 9.85g of gold was deposited. If the oxidation number of gold is +3 , find the amount of copper deposited at the cathode of the second cell. Also calculate the magnitude of the current in ampere, ( Atomic weight of Au is 1197 and atomic weight of Cu is 63.5) .

The electrolytic cell, one containing acidified ferrous chlo- ride and another with acidified ferric chloride are connected in series. The ratio of iron deposited at cathodes in the two cells when electricity is passed through the cells will be:

A current of 2A was passed for 1.5 hours through a solution of CuSO_(4) when 1.6g of copper was deposited. Calculate percentage current efficiency.