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 

Calculate the energy obtainable from a lead storage battery in which 0.1 mol lead is consumed. Assume a constant concentration of 10.0 M $H_2 S{O}_4$ 

(1) 42.8 kJ                                         

(2) 12.8 kJ

(3) 32.3 kJ                                         

(4) 20.2 kJ

Adiponitrile is manufactured electrolytically from acrylonitrile $C{H}_2= CHCN \to CN – (C{H}_2 {)}_4 – CH$

How many kg of adiponitrile (molecular mass = 108) is produced in 9.65 hr using a current of 3750 A with 80% efficiency?

(1) 30 kg                                               

(2) 58 kg

(3) 60 kg                                               

(4) 80 kg

A certain metal salt solutions is electrolysed in series with a silver coulometer. The weights of silver and the metal deposited are 0.5094 g and 0.2653 g. Calculate the valency of the metal if its atomic weight is nearly that of silver. 

(1) 1                                                 

(2) 2

(3) 3                                                 

(4) 4

The temperature coefficient, of the emf is $\frac{d\epsilon }{dT}$= – 0.00065 volt. $de{g}^{-1}$ for the cell $Cd\left|CdC{l}_2\left(1m\right)\right| \left|\underset{\left(s\right)}{AgCl}\right|Ag at 25°C$. Calculate the entropy change $∆S_{298K, }$ for the cell reaction,$Cd + 2AgCl \to C{d}^{++} + 2C{l}^{⊝}+ 2Ag$

$\left(1\right) – 105.5 J{K}^{-1}$

$\left(2\right) – 150.2 J{K}^{-1}$

$\left(3\right) – 75.5 J{K}^{-1}$

$\left(4\right) – 125.5 J{K}^{-1}$

The reduction potential of a half-cell consisting of a Pt electrode immersed in $1.5 M F{e}^{2+}$and $0.015 M F{e}^{3+}$ solution at $25°C is \left(E_{\left(F{e}^{+3}, Fe+2\right)}^{°}=+0.770 v\right)$.

(1) 0.652 V                                                   

(2) 0.88 V

(3) 0.710 V                                                   

(4) 0.850 V

In a concentration cell, $Zn/Z{n}^{2+} (1.0 M) \left|\right| Z{n}^{2+} (0.15 M)/Zn$ as the cell discharges,

(1) reaction proceeds to the right

(2) the two solutions approach each other in concentration

(3) no reaction takes place

(4) water gets decomposed

In a half-cell containing $\left[T{l}^{3+}\right] = 0.1 M and [T{l}^{+} ] = 0.01 M,$ the cell potential is – 1.2496 V for the reaction $T{l}^{+}\to T{l}^{3+} + 2e^{-}$  The standard reduction potential of the $T{l}^{+} /T{l}^{3+}$ couple at $25°C$ is

(1) 1.44 V                                          

(2) 0.61 V

(3) 2.44 V                                          

(4) 1.22 V