On electrolysis of dil. sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be :

The number of Faradays(F) required to produce 20 g of calcium from molten CaCl₂ (Atomic mass of Ca = 40 g mol^-1) is :

For a cell involving one electron $$E_{cell}^\Theta $$ = 0.59 V at 298 K, the equilibrium constant for the cell reaction is :

[Given that $${{2.303RT} \over F}$$ = 0.059 V at T = 298 K ]

For the cell reaction
2Fe³⁺(aq) + 2I^– (aq) $$ \to $$ 2Fe²⁺(aq) + I₂(aq)
$${E_{cell}^\Theta }$$ = 0.24 V at 298 K. The standard Gibbs energy ($$\Delta $$_rG^o) of the cell reaction is :
[Given that Faraday constant F = 96500 C mol^–1]