Exam Details
| Subject | Physical Chemistry | |
| Paper | ||
| Exam / Course | Bachelor Degree Programme(Elective Course: Chemistry) | |
| Department | School of Sciences (SOS) | |
| Organization | indira gandhi national open university | |
| Position | ||
| Exam Date | December, 2015 | |
| City, State | new delhi, |
Question Paper
1. What is the SI unit for electrical conductance?
2. If a gas expands against vacuum, what is the workdone on it?
3. State Bragg's law.
4. State Konowalof'f's rule.
5. Name two experimental methods used for measuring the elevation of boiling point.
6. State Le Chatelier's principle.
7. State Kohlrausch's law.
Answer any five of the following questions:
8. The value of the gas constant R is often expressed as 1.987 cal mol^-1 Find its value in SI units. It is given that 1 cal =4.184 J.
9. In what way is an isotropic substance different from an anisotropic substance?
10. What. are extensive variables Give any two examples.
11. NH4HS(s) evaporates m an evacuated container at 298 K according to the equation NH4HS NH3 H2S Find the pressure of each gas at equilibrium if K =1·10 x 10^9 Pa^2 at 298 K.
12. We cannot prepare absolute ethanol by fractional distillation. Explain why.
13. Calculate the number of components for dissociation of NH3 in a closed vessel.
14. State Faraday's laws of electrolysis.
15. For the second order reaction
2HI
the rate constant at 700 K is 1·83 x Calculate the time taken for 1·00 x 10^-2M HI to fall to half of its value.
16. Define colloidal dispersion, and give two examples.
17. The heterogeneous catalyst is used in finely divided powder form rather than as a smooth surface. Explain why.
18. What are photosensitised chemical reactions? Explain with the help of an example.
19. At 298 the standard enthalpies of formation of N02 and N20 4 are 33·2 and 9·2 kJ respectively. Calculate the standard enthalpy of the following reaction
N204 2NO2
20. Derive Nernst's distribution law thermodynamically.
21. Which of the following solutions will exert greater osmotic pressure:
0·1 M NaCl or 0.1 M sucrose?
Explain why.
22. A mixture of 2.0 x kg of H2 and 2·0 x kg of He exerts a pressure of 1·5 x 10^5 Pa. What are the partial pressures ofH2 and He
23. Calculate the pressure change if two moles of steam at 5 x 10^2 K occupying 0·03 m^3 of volume is heated up to 1 x 10^3 K at constant volume. Assume that steam behaves as Van der Waals gas. It is given that
a =0·5536 Pa m6 mol^-2 b =3·049 x m3 mol^-1.
24. An orthorhombic crystal has the following parameters:
a=8·2x10^-10 m
b =9·4 x 10^-10 m
c.= 7·5 x 10^-10 m
Find the distance between planes.
25. A solution contains 0·05 M acetic acid and 0·1 M sodium acetate. Calculate the concentration of when HCI is added to the solution such that
1·0 x M. Ka for acetic acid 1·8 x 10^-5.
26. Using kinetic theory of gases, derive an expression for pressure of a gas.
27. Calculate the equilibrium constant at 298 K for the cell reaction taking place in the cell
Al
given that EoAl3+/Al) -1.66 V and Cu2+/Cu 0.34 V
28. 1·0 x 10^2 mol of an ideal gas at 3·0 x 10^2 K temperature and 6.0 x 10^6 Pa pressure occupies 4·16 x 10-2 m^3 space. Calculate the work done and heat absorbed by the gas if it undergoes expansion isothermally and reversibly to 0·832 m^3 volume and 3.0 x 10^5 Pa pressure.
2. If a gas expands against vacuum, what is the workdone on it?
3. State Bragg's law.
4. State Konowalof'f's rule.
5. Name two experimental methods used for measuring the elevation of boiling point.
6. State Le Chatelier's principle.
7. State Kohlrausch's law.
Answer any five of the following questions:
8. The value of the gas constant R is often expressed as 1.987 cal mol^-1 Find its value in SI units. It is given that 1 cal =4.184 J.
9. In what way is an isotropic substance different from an anisotropic substance?
10. What. are extensive variables Give any two examples.
11. NH4HS(s) evaporates m an evacuated container at 298 K according to the equation NH4HS NH3 H2S Find the pressure of each gas at equilibrium if K =1·10 x 10^9 Pa^2 at 298 K.
12. We cannot prepare absolute ethanol by fractional distillation. Explain why.
13. Calculate the number of components for dissociation of NH3 in a closed vessel.
14. State Faraday's laws of electrolysis.
15. For the second order reaction
2HI
the rate constant at 700 K is 1·83 x Calculate the time taken for 1·00 x 10^-2M HI to fall to half of its value.
16. Define colloidal dispersion, and give two examples.
17. The heterogeneous catalyst is used in finely divided powder form rather than as a smooth surface. Explain why.
18. What are photosensitised chemical reactions? Explain with the help of an example.
19. At 298 the standard enthalpies of formation of N02 and N20 4 are 33·2 and 9·2 kJ respectively. Calculate the standard enthalpy of the following reaction
N204 2NO2
20. Derive Nernst's distribution law thermodynamically.
21. Which of the following solutions will exert greater osmotic pressure:
0·1 M NaCl or 0.1 M sucrose?
Explain why.
22. A mixture of 2.0 x kg of H2 and 2·0 x kg of He exerts a pressure of 1·5 x 10^5 Pa. What are the partial pressures ofH2 and He
23. Calculate the pressure change if two moles of steam at 5 x 10^2 K occupying 0·03 m^3 of volume is heated up to 1 x 10^3 K at constant volume. Assume that steam behaves as Van der Waals gas. It is given that
a =0·5536 Pa m6 mol^-2 b =3·049 x m3 mol^-1.
24. An orthorhombic crystal has the following parameters:
a=8·2x10^-10 m
b =9·4 x 10^-10 m
c.= 7·5 x 10^-10 m
Find the distance between planes.
25. A solution contains 0·05 M acetic acid and 0·1 M sodium acetate. Calculate the concentration of when HCI is added to the solution such that
1·0 x M. Ka for acetic acid 1·8 x 10^-5.
26. Using kinetic theory of gases, derive an expression for pressure of a gas.
27. Calculate the equilibrium constant at 298 K for the cell reaction taking place in the cell
Al
given that EoAl3+/Al) -1.66 V and Cu2+/Cu 0.34 V
28. 1·0 x 10^2 mol of an ideal gas at 3·0 x 10^2 K temperature and 6.0 x 10^6 Pa pressure occupies 4·16 x 10-2 m^3 space. Calculate the work done and heat absorbed by the gas if it undergoes expansion isothermally and reversibly to 0·832 m^3 volume and 3.0 x 10^5 Pa pressure.
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