Short Answer Type(a) Define molar conductivity of a solution and explain how molar conductivity changes with a change in concentration of solution for a weak and a strong electrolyte.
(b) The resistance of a conductivity cell containing 0.001 M KCl solution at 298 K is Ω 1500 . What is the cell constant if the conductivity of 0.001 M KCl solution at 298 K is 0.146x10-3 S cm-1?
The chemistry of corrosion of iron is essentially an electrochemical phenomenon. Explain the reactions occurring during the corrosion of iron in the atmosphere.
Determine the values of equilibrium constant (KC) and 
G° for the following reaction: 
The conductivity of 0.20 mol L-1 solution of KCl is 2.48 x 10-2 S cm-1. Calculate its molar conductivity and degree of dissociation (K+) = 73.56 S cm2 mol-1 and (Cl-)= 76.5 S
(b) What type of battery is mercury cell? Why is it more advantageous than dry cell?
The standard electrode potential (E°) for Daniell cell is +1·1 V. Calculate the G° for the reaction
Zn(s) + Cu2+ (aq) ----> Zn+ (aq) + Cu (s)
(1 F = 96500 C mol-1).
E° for Daniel cell = 1.1 V
Zn(s) + Cu2+ (aq)---> Zn2+ (aq) + Cu(s)
1F = 96500 C mol-1
G° =?
n = 2 (no. of e-s exchanged)
Since, G° = -nFE°
Therefore, G° = -2 x 96500 x 1.1
G° = -212300 J mol-1
G° = -212.3 kJ mol-1
Calculate the emf of the following cell at 25°C:
Given E°cell = + 0.46 V and log 10n = n
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