According to Faraday's first law

• $\mathrm{w} = \frac{ 96500 \times \mathrm{E}}{\mathrm{I} \times \mathrm{t}}$

• $\mathrm{w} = \frac{ \mathrm{I} \times \mathrm{t} \times \mathrm{E}}{96500}$

• $\mathrm{E}=\frac{\mathrm{I} \times \mathrm{t} \times 96500}{\mathrm{w}}$

• $\mathrm{E} = \frac{ \mathrm{I} \times \mathrm{w}}{\mathrm{t} \times 96500}$

The standard reduction potential for Fe²⁺/Fe and Sn²+/Sn electrodes are - 0.44 and- 0.14 V respectively. For the cell reaction,  ${\mathrm{Fe}}^{+} + \mathrm{Sn} \to \mathrm{Fe} + {\mathrm{Sn}}^{2+}$  the standard emf is

• + 0.30 V

• - 0.58 V

• + 0.58 V

• - 0.30 V

How is electrical conductance of a conductor related with length and area of cross section of the conductor?

• G = κ· l· a^-1

• G = l· a· κ^-1

• G = κ· a· l^-1

• G = κ· a· l^-2

84.

The overall reaction taking place at anode during electrolysis of fused sodium chloride using suitable electrode is

• oxidation of chloride

• reduction of sodium ions

• reduction of chlorine

• oxidation of sodium atoms

Which among the following solutions is not used in determination of the cell constant?

• 10^-2 M KCl

• 10^-1 M KCl

• 1 M KCl

• Saturated KCl

How many Faradays of electricity are required to deposit 10g of calcium from molten calcium chloride using inert electrodes? ( Molar mass of calcium = 40g mol^-1)

• 0.5 F

• 1F

• 0.25 F

• 2 F

In the cell represented by

Pb(s)|Pb²⁺(1M) || Ag⁺(1M)| Ag(s), the reducing agents is

• Pb²⁺

• Pb

• Ag

• Ag⁺

What is the SI unit of conductivity?

• Sm

• Sm^-1

• Sm²

• Sm^-2

Consider the equilibrium obtained by electrically connecting zinc-amalgam Zn(Hg) and HgO electrodes in mercury cell,

Au(Hg) + HgO (s) $\rightleftharpoons$ ZnO (s) + Hg (l)

Under this equilibrium, what is the relation between the potential of the Zn(Hg) and HgO electrodes measured against the standard hydrogen electrode?

• Zn(Hg) electrode potential is equal to HgO electrode potential.

• Zn(Hg) electrode potential is more than HgO electrode potential.

• HgO electrode potential is more than Zn(Hg) electrode.

• Cell voltage at above said equilibrium is 1.35 V

The standard reduction potential for Zn²⁺ /Zn, Ni²⁺ /Ni and Fe²⁺ /Fe are respectively -0.76, -0.23 and -0.44 V. The reaction X + Y²⁺ → X²⁺ + Y will have more negative $∆$G value when X and Y are

• X = Ni; Y = Fe

• X = Ni; Y = Zn

• X = Fe; Y = Zn

• X = Zn; Y = Ni