1. (a) Deduce the SI units for the gas constant, R.
(b) Define the following terms:
(i) Catalyst
(ii) Adsorption
2. List various assumptions of the kinetic theory of gases.
3. Derive the equation of corresponding states.
4. Define surface tension. Which factors influence the magnitude of the surface tension?
5. State Bragg Law. What assumptions were made by Bragg in deriving Bragg equation?
6. Define the term ‘system’. What are three types of systems? Explain.
7. Define enthalpy of neutralisation. Why is its value constant for strong acid-strong base neutralisation? Why is its value different if a weak acid is used in place of the strong acid?
8. What are different statements of second law of thermodynamics?
9. Discuss the physical significance of G.
10. In a solution 0.200 kg each of water and ethanol are present. Calculate the mole fraction of each component.
11. What is critical solution temperature? Describe liquid pairs which have
(i). upper CST,
(ii). lower CST, and
(ii). both upper and lower CST.
12. An aqueous solution containing 10.00 ×10-4 kg of a solute in 8.00 ×10-2 kg of water was found to freeze at 272.72 K. Calculate the molar mass of the solute. Molar enthalpy of fusion of ice at its melting point 273.15 K is 6021 J mol-1.
13. State and deduce the phase rule.
14. For the reaction,
CO(g)+2H2 → CH3 OH(g)
1 mole of CO and 2 mol of H2 were taken. Derive an expression for the equilibrium constant, Kp, in terms of the extent of the reaction, and the total pressure, pt.
15. What is the molarity of an aqueous solution of ammonia for which the −OH in concentration is 1.0 ×10-3 M? Kb =1.8 ×10-5.
16. Discuss the Hittorf method of determination of transport number.
17. What are concentration cells? Calculate the Ecell0 for such a cell giving a suitable example.
18. Briefly give various experimental methods for studying the reaction rates.
19. Discuss photosensitised chemical reactions giving suitable examples.
20. What are lyophilic sols? Describe the methods of coagulation of these sols.
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