In producing chlorine by electrolysis 100 kW power at 125V is being consumed.How much chlorine per minute is liberated (ECE of chlorine is 0.367$\times {10}^{-6}kg{C}^{-1}$)

(1) $1.76\times {10}^{-3}kg$                                   

(2) $9.67\times {10}^{-3}kg$

(3) $17.61\times {10}^{-3}kg$                                 

(4) $3.67\times {10}^{-3}kg$ 

Assertion : In electrochemical cell, we cannot use $\mathrm{KCI}$ in the salt bridge if anodic or cathodic

                  compartment consists of ${\mathrm{Ag}}^{+}$ of ${\mathrm{Pb}}^{2+}$ ion.

Reason : Salt bridge is employed to maintain the electrical neutrality and to minimize the liquid-liquid

               junction potential.

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

(D)The reaction for the cell,

$Zn<mspace\; width="1em"></mspace>|<mspace\; width="1em"></mspace>Z{n}^{2+}<mspace\; width="1em"></mspace>(1.0<mspace\; width="1em"></mspace>M)<mspace\; width="1em"></mspace>||<mspace\; width="1em"></mspace>C{d}^{2+}<mspace\; width="1em"></mspace>(1.0<mspace\; width="1em"></mspace>M)<mspace\; width="1em"></mspace>|<mspace\; width="1em"></mspace>Cd<mspace\; width="1em"></mspace>is-$

$\left(A\right)<mspace\; width="1em"></mspace>Cd<mspace\; width="1em"></mspace>\to C{d}^{2+}+<mspace\; width="1em"></mspace>2e^{-}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

$\left(B\right)<mspace\; width="1em"></mspace>Z{n}^{2+}\to <mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>Zn<mspace\; width="1em"></mspace>–<mspace\; width="1em"></mspace>2e^{-}$

$\left(C\right)<mspace\; width="1em"></mspace>Cd<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>Z{n}^{2+}\to <mspace\; width="1em"></mspace>C{d}^{2+}+<mspace\; width="1em"></mspace>Zn<mspace\; width="1em"></mspace>$

$\left(D\right)<mspace\; width="1em"></mspace>Zn<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>C{d}^{2+}<mspace\; width="1em"></mspace>\to Cd<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>Z{n}^{2+}$

Specific conductance has the unit:
1. \(\mathrm{ohm}^{-1} \mathrm{~cm}^{-1}\)
2.\(\text { ohm.cm }\)
3.\(\text { ohm } \mathrm{cm}^{-1}\)
4. \(\mathrm{ohm}^{-1} . \mathrm{cm}\)

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

At $25°C$, the standard emf of cell having reactions involving two electron change is found to be 0.295 V. The equilibrium constant of the reaction is-

$\left(A\right)<mspace\; width="1em"></mspace>29.5<mspace\; width="1em"></mspace>\times <mspace\; width="1em"></mspace>{10}^{-2}$

$\left(B\right)<mspace\; width="1em"></mspace>10<mspace\; width="1em"></mspace>$

$\left(C\right)<mspace\; width="1em"></mspace>{10}^{10}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

$\left(D\right)<mspace\; width="1em"></mspace>29.5<mspace\; width="1em"></mspace>\times <mspace\; width="1em"></mspace>{10}^{10}$

The number of faradays required to produce one mole of water from a hydrogen-oxygen fuel cell containing aqueous alkali as an electrolyte is-

1. 1                               

2. 3

3. 2                               

4. 4

How much current is necessary to produce $H_2$ gas at the rate of 1 $c{m}^3$ per second under STP ?

(A) 4.305 amp                                           

(B) 17.22 amp

(C) 8.61 amp                                            

(D) 2.1525 amp.

A current of 0.250 A is passed through 400 ml of a 2.0 M solution of NaCl for 35 minutes. What will be the pH of the solution after the current is turned off ?

(A) 12.98                            

(B) 12.13

(C) 10.48                            

(D) 9.24