A certain current liberates 0.504 g of hydrogen in 2 hours. How many gram of copper can be liberated by the same current flowing for the same time in aqueous $CuS{O}_4$ solution :

(1) 12.7                                                             

(2) 16

(3) 31.8                                                             

(4) 63.5

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 temperature coefficient of a standard Cd-cell is $–5.0<mspace\; width="1em"></mspace>\times <mspace\; width="1em"></mspace>{10}^{-5}<mspace\; width="1em"></mspace>V{k}^{-1}$ whose emf at $25°C$ is 1.018 V. During the cell operation, the temperature will -

(1) increase                                      

(2) decreases

(3) either                                         

(4) remains constant

Calculate the useful work of the reaction \(Ag(s) + {1 \over 2} Cl_2(g) \rightarrow AgCl(s)\) 

$Given,$
${E^{°}}_{C{l}_2/C{l}^{-}}=+1.36<mspace\; width="1em"></mspace>V,<mspace\; width="1em"></mspace>{E^{°}}_{AgCl/Ag,C{l}^{-}}=0.22<mspace\; width="1em"></mspace>V$
$If<mspace\; width="1em"></mspace>P_{C{l}_2}=1<mspace\; width="1em"></mspace>atm<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>T=298<mspace\; width="1em"></mspace>K$

(1) 110 kJ/mol

(2) 220 kJ/mol

(3) 55 kJ/mol

(4) 1000 kJ/mol

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

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 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