The same amount of electricity was passed through two cells containing molten Al₂O₃ and molten NaCl. If 1.8g of Al were liberated in one cell, the amount of Na liberated in the other cell is:

(1) 4.6 g

(2) 2.3 g

(3) 6.4 g

(4) 3.2 g

Standard Reduction electrode potential of three metals X, Y and Z are -1.2V, + 0.5V and -3V respectively. The reducing power of these metals will be 

(1) Y>X>Z

(2) Z>X>Y

(3) X>Y>Z

(4) Y>Z>X

How many columbs of electricity are consumed when 100 mA current is passed through a solution of AgNO₃ for 30 minute during an electrolysis experiment?

(1) 108

(2) 18000

(3) 180

(4) 3000

Standard reduction potentials at 25$°$C of Li⁺/Li, Ba²⁺/Ba, Na⁺/Na and Mg²⁺/Mg are -3.05, -2.90, -2.71 and -2.37 V respectively. Which one of the following is the strongest oxidising agent ?

(1) Mg²⁺

(2) Ba²⁺

(3) Na⁺

(4) Li⁺

For the cell, Ti/Ti⁺(0.001M)||Cu²⁺(0.1M)|Cu, ${\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}$ $$at

25 $°$C is 0.83 V. E_cell can be increased :

1. By increasing [Cu²⁺]

2. By increasing [Ti⁺]

3. By decreasing [Cu²⁺]

4. None of the above.

A hydrogen gas electrode is made by dipping platinum wire in a solution of HCI of pH = 10 and by passing hydrogen gas around the platinum wire at 1 atm pressure. The oxidation potential of electrode would be

1. 0.059 V

2. 0.59 V

3. 00.118 V

4. 1.18 V

The atomic mass of Al is 27. When a current of 5 faraday is passed through a solution of Al³⁺ ions, the mass of Al deposited is:

(1) 27g

(2) 36g

(3) 45g

(4) 9g

On the basis of the information available from the reaction.

$\frac{4}{3}\mathrm{Al} + {\mathrm{O}}_2 \stackrel{ }{\to }\frac{2}{3}{\mathrm{Al}}_2{\mathrm{O}}_3, ∆G =-827\mathrm{kJ} {\mathrm{mol}}^{-1}$ 

of O₂, the minimum EMF required to carry out the electrolysis of Al₂O₃ is :(F=96500 C mol^-1) 

(1) 2.14 V

(2) 4.28 V

(3) 6.42 V

(4) 8.56 V

For the reduction of silver ions with copper metal, the standard cell potential was found to be + 0.46 V at 25ºC. The value of standard Gibbs energy, $\Delta$G⁰ will be:
(F = 96500 Cmol^-1)

1. -89.0 KJ

2. 89.0 J

3. -44.5 KJ

4. -98.0 KJ

A solution of sodium sulphate in water is electrolysed using inert electrodes. The products at the cathode and anode are respectively:

(1) H₂, O₂

(2) O₂, H₂

(3) O₂, Na

(4) O₂, SO₂