LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034

WD 14

B.Sc. DEGREE EXAMINATION – CHEMISTRY

FOURTH SEMESTER – April 2009

CH 4502 – ELECTROCHEMISTRY

 

 

 

Date & Time: 24/04/2009 / 9:00 – 12:00  Dept. No.                                                   Max. : 100 Marks

 

 

                                                                      PART – A                   

Answer ALL questions.                                  (10 x 2 = 20 marks)

 

1. Define electromotive series. Give its application.
2. What is a reversible cell?
3. What is LJP? How can it be minimised?
4. What are Fuel cells? Give its application.
5. State Faraday’s first law of electrolysis.
6. Distinguish between Strong and Weak electrolyte.
7. Define the term activity of an electrolyte.
8. Explain the principle involved in the conductometic titration of AgNO₃.
9. Define the term limiting current.
10. Define Overvoltage.

 

PART – B

Answer any EIGHT questions.                                   (8 x 5 = 40 marks)

 

11. Explain the following with an example.

(i)         Metal – Metal ion electrode.

(ii)        Amalgam electrode.

12. Describe the construction and working of Weston cell.
13. Calculate the EMF of the concentration cell

Pt;  H₂(P₁),  HCl,  H₂(P₂);  Pt at 25^oC.

If P₁ = 600 torr and P₂ = 400 torr.

14. How will you determine the standard electrode potential of copper electrode.
15. How will you determine the pH of a solution using glass electrode.
16. Derive expressions for ΔG; ΔH  and  ΔS  in terms of EMF of a cell.
17. How is transport number determined by moving boundary method?
18. Calculate the equivalent and molar conductivities of 0.08N H₂SO₄  solution

having specific conductivity  1.72 x 10^-3  Scm^-1.

19. How is K_b of a weak base determined by conductance measurement?
20. Discuss the principle and procedure for conductometric titration of a

Strong acid with a strong base.

21. Discuss on the applications of decomposition potential.
22. Explain the electrochemical theory of corrosion.

 

                                                                      PART – C

Answer ANY FOUR questions.                                 (4 x 10 = 40 marks)

 

23. How is solubility of sparingly soluble salt determined by EMF measurements.
24. (i) Derive the Nernst electrochemical equation.

(ii)        Calculate the reduction potential of the electrode

Pt/Cl_2(g)  (1.15)atm/2Cl^– (0.01M).

Given that E^oCl₂/2Cl^– = 1.8V.

25. What are concentration cells? Derive an expression for the EMF of an electrolyte  for a concentration cell without transference.
26. Explain any four applications of EMF.
27. (i) Discuss the Arrhenius theory of electrolytic dissociation.

Give its limitations.

• Explain the principle involved in the potentiometric titrations.

28. (i) Discuss on the Debye-Huckel theory of strong electrolytes.

(ii)        Explain the principle of polarography.

 

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