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

The specific conductance of 0.1 M NaCl solution is 1.06 × 10^–2 ohm^–1 cm^–1. Its molar conductance in ohm^–1 cm² mol^–1 is

Among the following cells
Leclanche cell (I)
Nickel–cadmium cell (II)
Lead storage battery (III)
Mercury cell (IV)

Primary cells are

The hydrogen electrode is dipped in a solution of pH 3 at 25°C. The potential would be (the value of 2.303 RT/F is 0.059 V)

When same quantity of electricity is passed for half an hour, the amount of Cu and Cr deposited are respectively 0.375 g and 0.30 g. Ratio of electrochemical equivalent of Cu and Cr is

Given the data at 25°C,

Ag + I^– → AgI + e^– ; E° = 0.152 V

Ag → Ag⁺ + e^–; E° = –0.800 V

What is the value of log K_sp for AgI? $\left(2.303dfrac{ ext{RT}}{ ext{F}} = 0.059 ext{ V} ight)$

The quantity of electricity needed to separately electrolyze 1 M solution of ZnSO₄, AlCl₃ and AgNO₃ completely is in the ratio of

An infinite dilution of aqueous solution of BaCl₂, molar conductivity of Ba²⁺ and Cl^– ions are = 127.32 S cm²/moland 76.34 S cm²/mol respectively. What is Λ∞
m for BaCl₂ at same dilute?

Aqueous copper sulphate solution is electrolyzed using platinum electrodes. The electrode reaction occurring at cathode is

Zn | Zn²⁺ (a = 0.1M) || Fe²⁺ (a = 0.01M) | Fe. The emf of the above cell is 0.2905 V. Equilibrium constant for the cell reaction is