pl answer Q 11 12.
13.
14.
Questions
ELECTROCHEMISTRY
Electrolysis is used in refining extraction
metals upon discharge pore„tilas
e as as the Ofthe electrodes used in some cases.
The products Of electrolysis Of an aqueous solution Of using inert be
and S02 at anode
C) Sodium at cathode and oxygen at anode
D) Hydrogen at cathode and oxygen at anode
The quantity of electricity required to reduce 12.3 g Of nitrobenzene to aniline assuming 500/0
C) 231600 coulombs
B) 57900 coulombs
II. From the above question if the potential drop across the cell is energy consumed
B) 38600 J
C) 347400 J
b) 231600 J
Electrolysis is the process energy is converted to chemical energy. In electrolytic
cell, oxidation takes place ai anode and reduction at cathode. Electrode process depends on the
electrode taken for electrolysis. Amount of substance liberated at an electrode is directly
proportional to the amount of charge passed through it. The mass of substance liberated at
electrode is calculated using the following reaction:
ltE
96500
Here, E represents the equivalent mass and 96500 C is called the Faraday constant. Faraday
(96500 C) is' the Charge of 1 mol electron, i.e., 6.023 x 1023 electrons; it is used to liberate one
gram equivalent of the substance.
On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode
will be:
A) Hydrogen
B) Oxygen
C) Hydrogen sulphite D) Sulphur oxide
How many faradays are required to reduce I mol BrOÄ to Br-?
Calculate the volume of gas liberated at the anode at S.T.P. during the electrolysis of a CuS04
solution by a current of I A passed for 16 min and 5 sec.
D) 448 mL
C) 112 mL
B) 56 mL
A) 224 mL
