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.

The equilibrium constant of the reaction:

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

E^o = 0.46 V at 298 K is:

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

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

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.

The specific conductivity of a solution depends upon :

1. Number of ions as well as mobility of ions.          

2. Number of ions per cc or (cm³) of solution.

3. Number of ions per cc or (cm³) as well as mobilities of ions.

4. Mobilities of ions.

The  number of electrons involved in the deposition of 63.5 g of Cu from a solution of $CuS{O}_4$ is:

1 $6.022$ $\times$ ${10}^{23}$ $$

2 $3.011$ $\times$ ${10}^{23}$ $$

3 $12.044$ $\times$ ${10}^{23}$ $$

4 $$ $6.022$ $\times$ ${10}^{22}$

Value of ${{\wedge }_m}^0$ for $$ $SrC{l}_2$ (strong electrolyte) in water at $\mathrm{25 }°C$ from the data below is:

1. 270 Ω^-1 cm² mol^-1                                                     

2. 260 Ω^-1 cm² mol^-1 

3. 250 Ω^-1 cm² mol^-1                                                    

4. 255 Ω^-1 cm² mol^-1 

Given cell: 

Pt(s)|H₂(g)(P = 1 atm)| CH₃COOH(0.1 M), HCl(0.1 M) || KCl(aq)|Hg₂Cl₂(s)|Hg

EMF of the cell is found to be 0.045 V at 298 K and the temperature coefficient is 3.4×10^-4 V K^-1. The cell entropy change of the following cell is : 

[Given K_a CH₃COOH = 10^-5  M]

1. 70.8 J K⁻¹ mol⁻¹                      

2. 65.2 J K⁻¹ mol⁻¹

3. 79.2 J K⁻¹ mol⁻¹                  

4. 83.5 J K⁻¹ mol⁻¹

The $k=$ $4.95$ $\times$ ${10}^{-5}S$ $c{m}^{-1}$ for a 0.00099 M solution. The reciprocal of the degree of dissociation of acetic acid, if ${\wedge }_m^0$ for acetic acid is 400 S $c{m}^{2}mo{l}^{-1}$ will be: