${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Ni}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Ni}$}\right.}^0<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-0.25<mspace\; width="1em"></mspace>\mathrm{V},<mspace\; width="1em"></mspace>{\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Au}}^{+3}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Au}$}\right.}^0<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1.50<mspace\; width="1em"></mspace>\mathrm{V}$

the emf of Voltaic cell

$\mathrm{Ni}<mspace\; width="1em"></mspace>|<mspace\; width="1em"></mspace>{\mathrm{Ni}}^{+2}(1\mathrm{M})<mspace\; width="1em"></mspace>||<mspace\; width="1em"></mspace>{\mathrm{Au}}^{+3}(1\mathrm{M})<mspace\; width="1em"></mspace>\mathrm{Au}<mspace\; width="1em"></mspace>\mathrm{is}:-$

(1) 1.25 V

(2) -1.75 V

(3) 1.75 V

(4) 4 V

The same amount of electric current is apassed through aqueous solution of MgSO₄ and AlCl₃. If 2.8 g Mg metal is deposited at amount of Al metal deposited in second cell will be

1. 2.1 g

2. 2.49 g

3. 3.15 g

4. 3.73g

For the cell reaction

${\mathrm{Cu}}_{{\mathrm{c}}_1}^{+2}<mspace\; width="1em"></mspace>\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>+\hspace{0.17em}\mathrm{Zn}\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>\stackrel{<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}{\to }<mspace\; width="1em"></mspace>{\mathrm{Zn}}_{{\mathrm{C}}_2}^{+2}<mspace\; width="1em"></mspace>\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\mathrm{Cu}\left(\mathrm{s}\right)$

the change in free energy at a given temperature is a function of 

(1) lnC₁

(2) ln$\frac{{\mathrm{C}}_2}{{\mathrm{C}}_1}$ 

(3) ln (C₁ +C₂)

(4) lnC₂

The cell reaction of micro electrochemical cell formed during rusting of iron is:-

1.  ${\mathrm{O}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>4{\mathrm{H}}^{\oplus }\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>4{\mathrm{e}}^{-}<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>2{\mathrm{H}}_2\mathrm{O}<mspace\; width="1em"></mspace>\left(\mathrm{l}\right)$

2. $4{\mathrm{Fe}}^{+2}\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{O}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)<mspace\; width="1em"></mspace>\to <mspace\; width="1em"></mspace>4\mathrm{FeO}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>4{\mathrm{H}}^{\oplus }\left(\mathrm{aq}\right)$

3. $2\mathrm{Fe}\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{O}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>4\mathrm{H}{°}^{\oplus }\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>\to 2{\mathrm{Fe}}^{+2}\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{aq}\right)$

4.  $\mathrm{Fe}\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>\to {\mathrm{Fe}}^{+2}\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{e}}^{-}$

What will be the value of $∆\mathrm{G}°$ for the rection ${\mathrm{Cu}}^{+2}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\mathrm{Fe}<mspace\; width="1em"></mspace>\stackrel{<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}{\rightleftharpoons }<mspace\; width="1em"></mspace>{\mathrm{Fe}}^{+2}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\mathrm{Cu}<mspace\; width="1em"></mspace>,<mspace\; width="1em"></mspace>$

if ${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Cu}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Cu}$}\right.}^{\circ }<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>+0.34<mspace\; width="1em"></mspace>\mathrm{V}<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Fe}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Fe}$}\right.}^{\circ }<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-0.44<mspace\; width="1em"></mspace>\mathrm{V}$$$

(1) -65.62 KJ

(2) -75.27 KJ

(3) -150.54 KJ

(4) +150.54 KJ

$2{\stackrel{\oplus }{\mathrm{Ag}}}_{\left(\mathrm{aq}\right)}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{Cu}}_{\left(\mathrm{s}\right)}<mspace\; width="1em"></mspace>\stackrel{<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}{\rightleftharpoons }<mspace\; width="1em"></mspace>{{\mathrm{Cu}}_{\left(\mathrm{aq}\right)}}^{+2}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$

The cell potential for this reaction is 0.46V. Which of the following change will increase the potential the most ?

(1) $\left[\stackrel{\oplus }{\mathrm{Ag}}\right]$ concentration is doubled

(2) [Cu²⁺] concentration is halved

(3) Size of Cu_(s) electrode is doubled

(4) size of Ag_(s) electrode is decreased to half

Pick out the incorrect statement

1. Equivalent conductance increases with dilution

2. Molar conductance increases with dilution

3. Specific conductance increases with dilution

4. Specific resistance increases with dilution

A device that converts energy of the combustion of fuels like hydrogen and methane, directly

into electrical energy is known as:

1. Fuel cell

2. Electrolytic cell

3. Dynamo

4. Ni-Cd cell

 $F_2$ gas can’t be obtained by the electrolysis of any $F^{-1}$salt because-

1. Fluorine is the strongest reducing agent

2. Fluorine is the strongest oxidising agent.

3. Fluorine easily combine with atmospheric $O_2$

4. All

If the E°_cell for a given reaction has a negative value then which of the following gives the

correct relationships for the values of $∆$G° and K_eq?

1. $∆$G° < 0;K_eq > 1

2. $∆$G° < 0; K_eq < 1

3. $∆$G°> 0; K_eq < 1

4. $∆$G° > 0; K_eq > 1