Short Answer TypeFollowing reactions occur at cathode during the electrolysis of aqueous silver chloride solution:
Ag+ (aq) + e- → Ag(s) E° = +0.80 V
H+ (aq) + e- → 1/2 H2 (g) E° = 0.00 V
On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why?
Define limiting molar conductivity. Why conductivity of an electrolyte solution decreases with the decrease in concentration?
Calculate emf of the following cell at 25 °C:
Fe | Fe2+(0.001 M) || H+ (0.01 M) | H2 (g) (1 bar) | Pt(s)
E°(Fe2+ | Fe) = –0.44 V E°(H+ | H2 ) = 0.00 V
The resistance of a conductivity cell filled with 0.1 mol L-1 KCl solution is 100 . If the resistance of the same cell when filled with 0.02 mol L-1 KCl solution is 520
, calculate the conductivity and molar conductivity of 0.02 mol L-1 KCl solution. The conductivity of 0.1 mol L-1 KCl solution is 1.29x 10-2
-1cm-1
State Faraday's first law of electrolysis. How much charge in terms of Faraday is required for the reduction of 1 mol of Cu2+ to Cu.
Faraday's first law of electrolysis states that "the amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through the electrolytic solution or melt".
The reduction of one mol of Cu2+ to Cu can be represented as:
Cu2++ 2e-----> Cu
Since, in this reaction, there are two moles of electrons involved, so the amount of charge required is 2F.
Calculate emf of the following cell at 298 K: Mg(s) | Mg2+(0.1 M) || Cu2+ (0.01) | Cu(s)
[Given E0 cell = +2.71 V, 1 F = 96500 C mol-1]
The conductivity of 0.20 M solution of KCl at 298 K is 0.025 S cm-1. Calculate its molar conductivity?
a) What type of a battery is the lead storage battery? Write the anode and the cathode reactions and the overall reaction occurring in a lead storage battery when current is drawn from it.
(b) In the button cell, widely used in watches, the following reaction takes place
Determine E° and G° for the reaction 
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