Aluminium oxide may be electrolysed at 1000°C to furnish aluminium metal (At. Mass =27 amu; 1 Faraday = 96,500 Coulombs). The cathode reaction is Al³⁺ + 3e^– ⟶ Al
To prepare 5.12 kg of aluminium metal by this method would require

A gas X at 1 atm is bubbled through a solution containing a mixture of 1 MY^– and 1 MZ^–at 25°C. If the reduction potential of Z > Y > X, then

1. 0 L each of a buffer containing 1 mole NH₃ and 1 mol of \(NH_{4}^{+}\) were placed in the cathodic and anodic half-cells and 965 C of electricity was passed. If anodic and cathodic half cells reactions involve oxidation and reduction of water only as

2H₂O ⟶ 4H⁺ + O₂ – 4e^–

2H₂O + 2e ⟶ H₂ + 2OH^–
Then pH of

Aluminium displaces hydrogen from acids but copper does not. A galvanic cell prepared by combining Cu / Cu²⁺ and Al / Al³⁺ has an e.m.f.of 2.0 V at 298 K. If the potential of copper electrode is + 0.34 V, that of aluminium is

A solution containing one mole per litre of each Cu(NO₃)₂,AgNO₃, Hg₂(NO₃)₂ and Mg(NO₃)₂, is being electrolysed by using inert electrodes. The values of standard electrode potentials in volts (reduction potentials) are Ag⁺ / Ag= +0.80, \(Hg_{2}^{2+}\) / 2Hg = +0.79, Cu²⁺ / Cu= +0.34, Mg²⁺ / Mg= –2.37 with increasing voltage, the sequence of deposition of metals on the cathode will be

The specific conductance of a 0.1N KCl solution at 23°C is 0.012 ohm^-1 cm^-1. The resistance of cell containing the solution at the same temperature was found to be 55 ohm.The cell constant will be

At 25°C, the molar conductance at infinite dilution for the strong electrolytes NaOH, NaCl and BaCl₂ are 248 × 10^-4,126 × 10^-4 and 280 × 10^-4 S m₂ mol^-1 respectively.
\(\Lambda _{m}^{o}\) Ba(OH)2 in S m₂ mol^-1 is

In anodising :

Sodium is made by the electrolysis of a molten mixture of about 40% NaCl and 60% CaCl₂ because