How much time is required for complete decomposition of 4 moles of water using 4 ampere?

1. 3.86 X ${10}^5$ sec

2. 1.93 X ${10}^5$ sec

3. 96500 sec

4. 48250 sec

What will be the quantity of iron deposited by ferrous and ferric ion by 1F (Fe = 56)

(1) 14g, 9.3 g                                          

(2) 28g, 18.6 g

(3) 56g, 37.2g                                         

(4) None of these

Specific conductance has the unit:

1. $oh{m}^{-1}<mspace\; width="1em"></mspace>c{m}^{-1}$                           

2. ohm.cm

3. $ohm<mspace\; width="1em"></mspace>c{m}^{-1}$                             

4. $oh{m}^{-1}.cm$

What is the value of ${\mathrm{pK}}_{\mathrm{b}}<mspace\; width="1em"></mspace>({\mathrm{CH}}_3{\mathrm{COO}}^{-}<mspace\; width="1em"></mspace>)$ if ${\mathrm{\lambda }}_{\mathrm{m}}^0=<mspace\; width="1em"></mspace>390<mspace\; width="1em"></mspace>\&<mspace\; width="1em"></mspace>{\mathrm{\lambda }}_{\mathrm{m}}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>7.8$ for 0.04 of a $<mspace\; width="1em"></mspace>{\mathrm{CH}}_3\mathrm{COOH}$  at $25°\mathrm{C}$ ?

(A) 9.3                                               

(B) 9.2

(C) 4.7                                               

(D) 4.8

The metal that cannot be produced on reduction of its oxide by aluminium is :

(1) K                                                        

(2) Mn

(3) Cr                                                      

(4) Fe

 ${\mathrm{E}}^0<mspace\; width="1em"></mspace>\mathrm{for}<mspace\; width="1em"></mspace>\mathrm{the}<mspace\; width="1em"></mspace>\mathrm{reaction}<mspace\; width="1em"></mspace>$
$\mathrm{Fe}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{Zn}}^{2+}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>\mathrm{Zn}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{Fe}}^{2+}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>–<mspace\; width="1em"></mspace>0.35<mspace\; width="1em"></mspace>\mathrm{V}.$
The   given   cell   reaction   is: 

1. Feasible  

2. Not feasible

3. In equilibrium 

4. None of the above

Adiponitrile is manufactured electrolytically from acrylonitrile $C{H}_2=<mspace\; width="1em"></mspace>CHCN<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>CN<mspace\; width="1em"></mspace>–<mspace\; width="1em"></mspace>(C{H}_2<mspace\; width="1em"></mspace>{)}_4<mspace\; width="1em"></mspace>–<mspace\; width="1em"></mspace>CN$

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 reduction potential of a half-cell consisting of a Pt electrode immersed in $1.5<mspace\; width="1em"></mspace>M<mspace\; width="1em"></mspace>F{e}^{2+}$and $0.015<mspace\; width="1em"></mspace>M<mspace\; width="1em"></mspace>F{e}^{3+}$ solution at $25°C<mspace\; width="1em"></mspace>is<mspace\; width="1em"></mspace>\left(E_{\left(F{e}^{+3},<mspace\; width="1em"></mspace>Fe+2\right)}^{°}=+0.770<mspace\; width="1em"></mspace>v\right)$.

(1) 0.652 V                                                   

(2) 0.88 V

(3) 0.710 V                                                   

(4) 0.850 V

In a half-cell containing $\left[T{l}^{3+}\right]<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>0.1<mspace\; width="1em"></mspace>M<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>[T{l}^{+}<mspace\; width="1em"></mspace>]<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>0.01<mspace\; width="1em"></mspace>M,$ the cell potential is – 1.2496 V for the reaction $T{l}^{+}\to <mspace\; width="1em"></mspace>T{l}^{3+}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2e^{-}$  The standard reduction potential of the $T{l}^{+}<mspace\; width="1em"></mspace>/T{l}^{3+}$ couple at $25°C$ is

(1) 1.44 V                                          

(2) 0.61 V

(3) 2.44 V                                          

(4) 1.22 V