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?
Conductivity of KCl solution = 2.48 x 10-2 S cm-1
Concentration of KCl solution = 0.20 mol L-1
= 0.20 x 1000 mol cm -3
= 200 mol cm-3
Molar conductivity 
b) Mercury cell is a type of primary battery. In primary batteries , the charging reaction occurs only once and after it has been used over a period of time , the battery becomes dead and cannot be refused mercury cell is more advantage than dry cell has a very short life span due to the conversion of zinc to zinc chloride that makes the zinc casing porous . Due to this porous casing, the substance inside the cell leaks out and corrodes the metal, reducing the lifetime of the cell. While, in the case of mercury cell, the overall reaction does not involve the formation of any ion in the solution whose concentration can change during its life time.
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).
Calculate the emf of the following cell at 25°C:
Given E°cell = + 0.46 V and log 10n = n
Switch
