In the electrochemical cell:

Zn|ZnSO₄(0.01 M) || CuSO₄(1.0M),Cu, the emf of this Daniel cell is E₁. When the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ is changed to 0.01 M, the emf changes to E₂. The relationship between E₁ and E₂ is : 
( Given, $\frac{RT}{\mathrm{F }}$= 0.059)

1. E₁ = E₂

2. E₁ < E₂

3. E₁ > E₂

4. E₂ = 0 $\ne$E₁

The weight of silver (atomic weight = 108) displaced by a quantity of electricity which displaces 5600 mL of O₂ at STP will be : 

1. 5.4 g

2. 10.8 g

3. 54.0 g

4. 108.0 g

The equilibrium constant of the reaction:

Cu (s) + 2Ag⁺ (aq) $\to$Cu²⁺ (aq) + 2Ag(s) ;

E^o = 0.46 V at 298 K is:

During electrolysis of conc. H₂SO₄, perdisulphuric acid (H₂S₂O₈), and O₂ form in equimolar amount. The amount of H₂ that will form simultaneously will be : 

1. Thrice that of O₂ in moles.

2. Twice that of O₂ in moles.

3. Equal to that of O₂ in moles.

4. Half of that of O₂ in moles.

When aqueous NaCl solution is electrolysed using inert electrodes then pH of the solution-

1. Increases.

2. Decreases.

3. Remains same.

4. First increases then decreases.

The quantity of electricity required to reduce 12.3 g of nitrobenzene to aniline with 50 % current efficiency is:

1. 1 F

2. 0.6 F

3. 0.5 F

4. 1.2 F

The maximum work which can be obtained from a Daniel cell \(Zn_{(s)}\ |\ Zn^{+2}_{(aq)}\ || Cu^{+2}_{(aq)}\ |\ Cu_{(s)}\) is:

1. 106.15 kJ

2. -212.3 kJ

3. 424.6 kJ

4. +212.3 kJ

At 298 K the Emf of the following cell is:-

\(\small{Pt|H_{2}(1 \ atm)|H^{+}(0.02 \ M) \ || \ H^{+}(0.01 \ M)|H_{2}(1 \ atm)|Pt}\)

1. - 0.017 V

2. 0.0295 V

3. 0.1 V

4. 0.059 V

By how much will the potential of half cell Cu²⁺| Cu change if the solution is diluted to 100 times at 298 K. It will -

During discharge of a lead storage cell, the density of sulphuric acid in the cell-

1. Increases.                                     

2. Decreases.

3. Remains unchanged.                      

4. Initially increases but decreases subsequently.