A button cell used in watches functions as following 

Zn(s) + Ag2O(s) + H2O(l) \(\rightleftharpoons\) 2Ag(s) + Zn2+(aq) + 2OH–(aq)

If half-cell potentials are:

Zn2+(aq) + 2e–→ Zn(s)	Eo = – 0.76 V
Ag2O(s) + H2O(l) + 2e– → 2Ag(s) + 2OH–(aq)	Eo = 0.34 V

The cell potential will be:

1. 0.42 V

2. 0.84 V

3. 1.34 V

4. 1.10 V

Limiting molar conductivity of NH₄OH (i.e., ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{OH}\right)}^0$ is equal to -

1. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0$

2. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{Cl}\right)}^0$

3. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{OH}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{Cl}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left(HCl\right)}^0$

4. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{Cl}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^0$

If the  $E_{cell }^0$for a given reaction has a negative value, then which of the following gives the correct relationship for the values of $∆G^0 and K_{eq}$?

1.  $∆{\mathrm{G}}^0<0; {\mathrm{K}}_{\mathrm{eq}}>1$

2.  $∆{\mathrm{G}}^0<0; {\mathrm{K}}_{\mathrm{eq}}<1$

3.  $∆{\mathrm{G}}^0>0; {\mathrm{K}}_{\mathrm{eq}}<1$

4.  $∆{\mathrm{G}}^0>0; {\mathrm{K}}_{\mathrm{eq}}>1$

Standard electrode potential for Sn⁴⁺/Sn²⁺ couple is +0.15 V and that for Cr³⁺/Cr couple is -0.74. These two couples in their standard state are connected to make a cell. The cell potential will be:

1. +0.89 V

2. +0.18 V

3. +1.83 V

4. +1.199 V

In producing chlorine by electrolysis, 100 kW power at 125 V is being consumed. How much chlorine per minute is liberated (ECE of chlorine is 0.367 X 10-6 kgC^-1)

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

2. $9.67\times {10}^{-3} kg$

3. $17.61\times {10}^{-3} kg$

4. $3.67\times {10}^{-3} kg$

For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25 °C. The value of standard Gibbs energy, ΔG^o will be : 

(F = 96500 C mol^-1)

1. -89.0 kJ

2. -89.0 J

3. -44.5 kJ

4. -98.0 kJ

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

1. increase in ionic mobility of ions

2. 100% ionization of electrolyte at normal dilution

3. increase in both, i.e, number of ions and ionic mobility of ions

4. increase in the number of ions

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.0 x 10⁴ A of current is passed through molten Al₂O₃ for 6 hours, what mass of aluminium is produced ?

(Assume 100 % current efficiency, atomic mass of Al = 27 g mol^-1)

1. 9.0 x 10³ g

2. 8.1 X 10⁴ g

3. 2.4 x 10⁵ g

4. 1.3 X 10⁴ g