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Electrolysis is the process in which ele...

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.
Calculate the volume of gas liberated at the anode at STP during the electrolysis of a `CuSO_4` solution by a current of 1 A passed for 16 minutes and 5 seconds.

A

`224 mL `

B

`56 mL `

C

`112 mL `

D

` 448 mL `

Text Solution

Verified by Experts

The correct Answer is:
B
`96500 CaCl to (1)/(4) " mole of " O_2`
` 1 xx 16 xx 60 CaCl to NO_2 = ?`
` n_(O_2) = (1 xx 16 xx 60 xx (1)/(4))/(96500) , V_(O_2) + n_(O_2) xx 22400 = 55. 709 = ~= 56 ml`
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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

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