Faradays Law Of Electrolysis

A steady current of 1.5 A flows through a copper voltmeter for 10 min. If the electrochemical equivalent of copper is 30 \times 10^-5 g C^-1, the mass of copper deposited on the electrode will be:

1. 0.40 g

2. 0.50 g

3. 0.67 g

4. 0.27 g

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.0 x 10⁴ A of current is passed through molten Al₂O₃ for 6 hours, the mass of aluminum produced is:
(Assume 100 % current efficiency, the atomic mass of Al = 27 g mol^-1)

1.	9.0 x 103 g	2.	8.1 x 104 g
3.	2.4 x 105 g	4.	1.3 x 104 g

For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25 °C. The value of standard Gibbs energy, ΔG^o will be:

(F = 96500 C mol^-1)

1. -89.0 kJ

2. -89.0 J

3. -44.5 kJ

4. -98.0 kJ

In producing chlorine by electrolysis, 100 kW power at 125 V is being consumed.
How much chlorine per minute is liberated:
(Given -ECE of chlorine is 0.367 X 10-6 kgC^-1)

1.$\mathrm{<mspace\; width="1em"></mspace>1}.76\backslash times{10}^{-3}$ $kg$

2. $9.67\backslash times{10}^{-3}$ $kg$

3. $17.61\backslash times{10}^{-3}$ $kg$

4. $3.67\backslash times{10}^{-3}$ $kg$

During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is:

1. 55 minutes

2. 110 minutes

3. 220 minutes

4. 330 minutes

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:

(Given: Charge on electron = 1.60 \times 10^–19 C)

1. $6\backslash times{10}^{23}$

2. $6\backslash times{10}^{20}$

3. $3.75\backslash times{10}^{20}$

4. $7.48\backslash times{10}^{20}$

Match the redox conversions in List-I with the corresponding number of Faradays required in List-II.

List-I (Redox Conversion)		List-II (Number of Faraday required)
A.	1 mol of H2O to O2	I.	3F
B.	1 mol of to	II.	2F
C.	1.5 mol of from molten	III.	1F
D.	1 mol of FeO to Fe2O3	IV.	5F

Choose the correct answer from the options given below:

1.	A - III, B - IV, C - I, D - II	2.	A - II, B - III, C - I, D - IV
3.	A - III, B - IV, C - II, D - I	4.	A - II, B - IV, C - I, D - III

Mass in grams of copper deposited by passing 9.6487 A current through a voltmeter containing copper sulphate for 100 seconds is(Given : Molar mass of Cu: F = 96487 C)

1.	0.315 g	2.	31.5 g
3.	0.0315 g	4.	3.15 g