Which of following cell can produce more electrical work.

1. $$pt, H2 | NH4Cl || 0.1 M CH3COOH | H2 , pt

2. $pt, H_2 | 0.1 M HCl || 0.1 M NaOH | H_2 , pt$

3. $pt, H_2 | 0.1 M HCl || 0.1 M C{H}_{3}COOK | H_2 , pt$

4. $pt, H_2 | 0.1 M C{H}_{3}COOK || 0.1 M HCl | H_2 , pt$

The calomel electrode is reversible with respect to-

1. Mercury                                       

2. $H^{+}$

3. $H{g}^{2+}$                                          

4. $C{l}^{-}$

Zn amalgam is prepared by electrolysis of aqueous $ZnC{l}_2$ using Hg cathode (9 gm). How much current is to be passed through $ZnC{l}_2$ solution for 1000 seconds to prepare a Zn Amalgam with 25% Zn by wt. (Zn = 65.4)

(1) 5.6 amp 

(2) 7.2 amp

(3) 8.85 amp 

(4) 11.2 amp

The standard oxidation potentials of $Cu/C{u}^{2+}$and $C{u}^{+} /C{u}^{2+} are – 0.34V and – 0.16 V$respectively. The standard electrode potential of $C{u}^{+} /Cu$ would be :

1. 0.18V  

2. 0.52V

3. 0.82V    

4. 0.49V

Acidified water is electrolyzed using an inert electrode. The volume of gases liberated at

STP is 0.168L. The quantity of charge passed through the acidified water would be:

(1) 96,500 C 

(2) 9,650 C

(3) 965 C 

(4) 168 C

 ${\mathrm{E}}^0 \mathrm{for} \mathrm{the} \mathrm{reaction}$
$\mathrm{Fe} + {\mathrm{Zn}}^{2+} = \mathrm{Zn} + {\mathrm{Fe}}^{2+} \mathrm{is} – 0.35 \mathrm{V}.$
The   given   cell   reaction   is: 

1. Feasible  

2. Not feasible

3. In equilibrium 

4. None of the above

How much charge should be supplied to a cell for the electrolytic production of 245 gm $NaCl{O}_4$ from $NaCl{O}_3$ if the anode efficiency for the required reaction is 60%?

(1) 6.43 × ${10}^{5}C$                                                

(2) 3.67 F

(3) 6.43 × ${10}^6 C$                                               

(4) 5.67 F

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