Standard electrode potential of three metals X, Y and Z are -1.2 V, +0.5 V and -3.0 V respectively. The reducing power of these metals will be : 

1.  Y > X > Z

2.  Z > X > Y

3.  X > Y > Z

4.  Y > Z > X

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

The molar conductance of $\frac{\mathrm{M}}{32}$ solution of a weak monobasic acid is 8.0 ohm^-1 cm² and at infinite dilution is 400 ohm^-1 cm². The dissociation constant of this acid is : 

1. $1.25\times {10}^{-5}$

2. $1.25\times {10}^{-6}$

3. $6.25\times {10}^{-4}$

4. $1.25\times {10}^{-4}$

Given, 
(i) ${\mathrm{Cu}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Cu}$    E^o = 0.337 V 
(ii) ${\mathrm{Cu}}^{2+}+{\mathrm{e}}^{-}\to {\mathrm{Cu}}^{+}$  E^o = 0.153 V 
Electrode potential, E^o for the reaction, 
${\mathrm{Cu}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Cu}$, will be : 

1. 0.52 V

2. 0.90 V

3. 0.30 V

4. 0.38 V