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. $6.022$ $\times$ ${10}^{22}$

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:

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.

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 molar conductivity of a 0.5 mol/dm³ solution of AgNO₃ with electrolytic conductivity of 5.76 × 10^–3 S cm^–1 at 298 K is:

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:

(Given: Charge on electron = 1.60 × 10^–19 C)

1.  $6\times {10}^{23}$

2.  $6\times {10}^{20}$

3.  $3.75\times {10}^{20}$

4.  $7.48\times {10}^{20}$

The pressure of H₂ required to make the potential of H₂ - electrode zero in pure water at 298 K is:

A device that converts the energy of combustion of fuels, like hydrogen and methane, directly into electrical energy is known as: 

When 0.1 mol MnO₄^2– is oxidized, the quantity of electricity required to completely oxidise MnO₄^2– to MnO₄^– is:

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