Electrochemistr...

On passing 0.5 F of electricity through molten sodium chloride, sodium deposited at cathode will be

Calculate the volume of H₂ gas at NTP obtained by passing 4 A through acidified H₂O for 30 min is

The charge required for reduction of 1 mole o f Cr₂ O^2-₇ ions to Cr³⁺ is

The standard emf for the cell reaction
2Cu⁺ (aq) → Cu(s) + Cu²⁺ (aq)
is + 0.36 V at 298 K. The equilibrium constant of the reaction is

Given that; Zn²⁺ / Zn = -0.762 V, Mg²⁺ / Mg = - 2.37V. Then, Zn + MgCl₂ → ?

The standard emf of a cell involving one electron change is found to be 0.591 V at 25°C. The equilibrium constant of the reaction is (F = 96500 C mol^-1)

E^o values of Mg²⁺ / Mg is -2.37 V of Zn²⁺ / Zn is -0.76 V and Fe²⁺ / Fe is -0.44 V.
Which of the statements is correct ?

If the standard electrode potential of Cu²⁺ / Cu electrode is 0.34 V, What is the electrode potential at 0.01 M concentration of Cu²⁺ ?
(T = 298 K)

In which of the following pairs, the constants/ quantities are not mathematically related to each other?

Dipping iron article into a strongly alkaline solution of sodium phosphate