The electricity required in coulombs for the oxidation of 1 mole of FeO to is:
1. | 964.87 C | 2. | 96487 C |
3. | 96.487 C | 4. | 9.6487 C |
The amount of charge required for the reduction of 1 mol of to is -
The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:
(Charge on electron = 1.60 × 10–19 C)
1.
2.
3.
4.
When 0.1 mol MnO42– is oxidized, the quantity of electricity required to completely oxidise MnO42– to MnO4– is:
1. 96500 C
2. 2 × 96500 C
3. 9650 C
4. 96.50 C
The number of Faradays required to produce 20.0 g of Ca from molten CaCl2 is-
1. 2F
2. 1F
3. 4F
4. 3F
A steady current of 1.5 A flows through a copper voltmeter for 10 min. If the electrochemical equivalent of copper is 30 × 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
For the cell, Ti/Ti+(0.001M)||Cu2+(0.1M)|Cu, at
25 C is 0.83 V. Ecell can be increased :
1. By increasing [Cu2+]
2. By increasing [Ti+]
3. By decreasing [Cu2+]
4. None of the above.
The number of electrons involved in the deposition of 63.5 g of Cu from a solution of is:
1
2
3
4
A 100.0 mL dilute solution of Ag+ is electrolyzed for 15.0 minutes with a current of 1.25 mA and the silver is removed completely. The initial [Ag+] is :-
1. 2.32 x 10 M
2. 2.32 x 10 M
3. 2.32 x 10 M
4. 1.17 x 10 M
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, ΔGo will be:
(F = 96500 C mol-1)
1. -89.0 kJ
2. -89.0 J
3. -44.5 kJ
4. -98.0 kJ