For the reductidon of silver ions with copper metal, the standard  cell potential was found to be + 0.46 V at 25⁰C. 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

If a salt bridge is removed from the two half cells, the voltage:

1. Drops to zero.

2. Does not change.

3. Increases gradually.

4. Increases rapidly.

Two electrolytic cells, one containing acidified ferrous chloride and another acidified ferric chloride are connected in series. The ratio of iron deposited at cathodes in the two cells when electricity is passed through the cells will be:

1. 3:1

2. 2:1

3. 1:1

4. 3:2

If the half-cell reaction A+e$\to$A^- has a large negative reduction potential, it follows that:

1. A is readily reduced

2. A is readily oxidized

3. A^- is readily reduced

4. A^- is readily oxidized

A certain current liberates 0.504 g of hydrogen in 2 hr. How many gram of copper can be liberated by the same current flowing for the same time in CuSO₄ solution?

1. 12.7

2. 16

3. 31.8

4. 63.5

Which one of the following pairs of substances on reaction will not evolve H₂ gas?

1. Iron and H₂SO₄ (aq)

2. iron and steam

3. Copper and HCl(aq)

4. Sodium and ethyl alcohol

4.5 g of aluminium (atomic mass 27u) is deposited at cathode from Al³⁺ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H⁺ ions in solution by the same quantity of electric charge will be

1. 44.8 L

2. 22.4 L

3. 11.2 L

4. 5.6 L

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 the electrode would be:

1. 0.059 V
2. 0.59 V
3. 00.118 V
4. 1.18 V

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

1. increase in ionic mobility of ions

2. 100% ionisation of electrolyte at normal dilution

3. increase in both, i.e. number of ions and ionic mobility of ions

4. increase in number of ions