(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 (K_C) and  G° for the following reaction: 

How much charge is required for the reduction of 1 mol of Zn²⁺ to Zn?

Define rate of reaction? Write two factors that affect the rate of reaction.

Calculate E.M.F. and G for the following cell:

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).

320.

Calculate the emf of the following cell at 25°C: 

 

Given E°_cell = + 0.46 V and log 10ⁿ = n