Q. No.Faraday’s laws of electrolysis are associated with:
1. The atomic number of the reactants.2. The atomic number of the anion.
3. The equivalent weight of the electrolyte.
4. The speed of the cation
| Column I | Column II | ||
| (A) | Electrochemical equivalent | (i) | Potential difference \(\times\) Quantity of charge |
| (B) | Faraday | (ii) | Mass of substance deposited by one coulomb of charge |
| (C) | Ampere | (iii) | Charge carried by one mole of electrons |
| (D) | Electrical energy | (iv) | One coulomb of electric charge passed through one second |
2. (A) →(ii), (B)→(iii), (C) →(iv), (D)→ (i)
3. (A) →(iii), (B)→(iv), (C) →(i), (D)→ (ii)
4. (A) →(iv), (B)→(i), (C) →(ii), (D)→ (iii)
coloumb charge liberated 1 gm silver (Ag). If the charge is doubled then the amount of liberated Ag will be:
| 1. | 1 gm | 2. | 2 gm |
| 3. | 3 gm | 4. | 4 gm |
The number of electrons passing per second through a cross-section of Cu wire carrying 10 ampere is :
1.
2.
3.
4.
The amount of electricity required to deposit 1.0 mole of aluminium from a solution of AICl3 will be:
1. 1 faraday
2. 3 faraday
3. 0.33 faraday
4. 1.33 faraday
1. 3
2. 6
3. 4
4. 7
During an electrolysis experiment, if a 100 mA current is passed through a solution of AgNO3 for 30 minutes, how many coulombs of electricity will be consumed?
1. 108 C
2. 18000 C
3. 180 C
4. 3000 C
The number of electrons delivered at the cathode during electrolysis by a current of 1A in
60 seconds is:
(charge of electron = 1.6 x 10C)
1. \(6.22 \times 10^{23}\)
2. \(6.022 \times 10^{20}\)
3. \(3.75 \times 10^{20}\)
4. \(7.48 \times 10^{23}\)
A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is trivalent. The atomic mass of the metal is
1. 30
2. 150
3. 90
4. 289.5
1. 2.4 × 104 s
2. 1.5 × 103 s
3. 7.6 × 102 s
4. 3.8 × 102 s
© 2026 GoodEd Technologies Pvt. Ltd.