ELECTROLYSIS

In an electrolysis experiment, a cathode of mass 5g is found to weigh 5.01g after a current of 5A flows for 50s. What is the electrochemical equivalent of the deposited substance?

• 0.00004g/c

• 0.00002g/c

• 0.025000g/c

• 0.00001g/c

The electrochemical equivalent of a metal is 0.126x10^-6kg/c. The mass of the metal that a current of 5A will deposit from a suitable bath in 1hour is?

• 0.0378x10^-3kg

• 0.227x10-3kg

• 0.378x10^-3kg

• 2.268x10^-3kg

In the calibration of an ammeter using Faraday's laws of electrolysis, the ammeter reading is kept constant at 1.20A. If 0.990g of copper is deposited in 40minutes, the correction to be applied to the ammeter is?

(Electrochemical equivalent of copper = 3.3x10^-4g/c)

• 0.03A

• 0.04A

• 0.05A

• 0.06A

During electrolysis, 2.0g of a metal is deposited using a current of 0.5A in 3hours. The mass of the same metal which can be deposited using a current of 1.5A in 1hour is?

• 3.0g

• 2.0g

• 0.5g

• 1.0g

118.8cm² surface of the copper cathode of a voltmeter is to be coated with 10^-6m thick copper of density 9x10³kgm^-3. How long will the process run with 10A constant current? (Electrochemical equivalent of copper = 3.3x10^-7kg/c)

• 0.54minutes

• 5.4minutes

• 10.8minutes

• 15.0minutes

1.8g of a substance is liberated during electrolysis by the passage of a steady current of 2.0A for 2hours. How long will it take to liberate 5.4g of the same substance when the current is 3.0A?

• 2hours

• 3hours

• 4hours

• 5hours

In the electrolysis of copper sulphate solution 1.98g of copper in 100min by a steady current. If the electrochemical equivalent of copper is 0.0003g/c, the current is?

• 6A

• 3A

• 1.1A

• 0.5A

An electric current passes through two voltmeters in series, containing copper sulphate and silver nitrate respectively. What is the mass of silver deposited in a given time if the mass of copper deposited that time is 1g? (Atomic weight of copper is 63, Atomic weight of silver is 108, valency of copper is 2, valency of silver is 1)

• 2.8g

• 3.4g

• 3.9g

• 4.0g

A charge of one coulomb liberated 0.0033g of copper in an electrolysis process. How long will it take a current of 2A to liberated 1.98g of copper in such a process?

• 5min:29sec

• 30mins

• 50mins

• 60mins

If a current of 1A flowing for 5hrs deposits 6g of copper, calculate the mass of copper deposited by a current of 3A flowing for 7hrs

• 20.0g

• 25.2g

• 30.0g

• 30.5g