The emf of the cell $\left({\mathrm{E}}_{{\mathrm{Zn}}^{2+}/ \mathrm{Zn}} = -0.76 \mathrm{V}\right)$

Zn/ Zn²⁺ (1M) || Cu²⁺ (1M) Cu

$\left({\mathrm{E}}_{{\mathrm{Cu}}^{2+}/ \mathrm{Cu}} = +0.34 \mathrm{V}\right)$ will be

• +1.10 V

• -1.10 V

• +0.42 V

• -0.42 V

For the redox reaction

Zn (s) + Cu²⁺ (0.1 M) → Zn²⁺ (1 M) + Cu (s)

taking place in a cell, E${}_{\mathrm{cell}}^{°}$ is 1.10 V. E_cell for the cell will be $\left(2.303 \frac{\mathrm{RT}}{\mathrm{F}} = 0.0591\right)$

• 2.14 V

• 1.80 V

• 1.07 V

• 0.82 V

553.

The highest electrical conductivity of the following aqueous solutions is of

• 0.1 M difluoroacetic acid

• 0.1 M fluoroacetic acid

• 0.1 M chloroacetic acid

• 0.1 M acetic acid

Aluminium oxide may be electrolysed at 1000°C to furnish aluminium metal (atomic mass = 27 amu; 1 F = 96,500 C). The cathode reaction is

Al³⁺ + 3e^- → Al⁰

To prepare 5.12 kg of aluminium metal by this method would require

• 5.49 × 10¹ C of electricity

• 5.49 × 10⁴ C of electricity

• 1.83 × 10⁷ C of electricity

• 5.49 × 10⁷ C of electricity

In acidic medium MO${}_4^{-}$ is converted to Mn²⁺. The quantity of electricity in faraday required to reduce 0.5 mole of MnO${}_4^{-}$ to M²⁺ would be:

• 2.5

• 5

• 1

• 0.5

During electrolysis of water the volume of O₂ liberated is 2. 24dm³. The volume of hydrogen liberated, under same conditions will be

• 2.24 dm³

• 1.12 dm³

• 4.48 dm³

• 0.56 dm³

The mass of carbon anode consumed (giving only carbon dioxide) in the production of 270 kg of aluminium metal from bauxite by the Hall process is (Atomic mass of Al = 27)

• 180 kg

• 270 kg

• 540 kg

• 90 kg

The best way to prevent rusting of iron is

• making it cathode

• putting in saline water

• Both (a) and (b)

• none of the above

stainless steel has iron and

• Cr

• Cu

• Co

• Zn

What flows in the internal circuit of a galvanic cell?

• ions

• electrons

• electricity

• atoms