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 | June, 2016 | |
| City, State | new delhi, |
Question Paper
No. of Printed Pages: 12
I CHE-04 1
BACHELOR OF SCIENCE (B.Se.)
Term-End Examination
June, 2016
01.21.7
CHEMISTRY CHE-04 PHYSICAL CHEMISTRY
Time: 2 hours Maximum Marks: 50
Note: Attempt all the parts. Answer five questions from each ofthe parts C and D. .
PART A
Answer any five questions. 5x1=5
1. What is the S.I. unit of temperature? 1
2. State Graham's law of effusion of gases. 1
3. Name the crystal system whose unit cell has the following characteristics 1
a b c and a B 90°
4. Identify the type of thermodynamic system in each of the following cases 1
A sealed bottle of flavoured milk.
Ice in a closed thermos flask
5. Write the equation for the phase rule. 1
6. Explain why an aqueous solution of NH4Cl is acidic in nature. 1
7. Write the expression for the instantaneous rate of the following reaction in terms of changes in concentrations of O3 or O2 1
2 3
PART B
Answer any five questions. 5x2=10
8. Which among the following is expected to have the highest surface tension at room temperature water, methyl cyanide or methanol? State the reason also. 2
9. Differentiate between intrinsic and extrinsic semiconductors in terms of the origin of conductivity in them. 2
10. Identify the intensive and extensive variables from among the following: 2
Temperature of a body
Number of moles present in a substance
Quantity of cooking gas burnt for boiling milk
Specific heat
11. Give one example each of chemical reactions undergoing homogeneous catalysis and heterogeneous catalysis. 2
12. State the principle of corresponding states. 2
13. Addition of NH4Cl to an aqueous solution of NH40H results in a decrease of pH. Explain. 2
14. Explain the effect of
increase in pressure and
increase in temperature on the following reaction: 2
N2 3 H2 2 NH3 DrH° =-92.2 kJ mol^-1
PART C
Answer any five questions. 5x3=15
15. Derive Van der Waals equation from the ideal gas equation.
16. Draw a labelled phase diagram of Bi -Cd system. 3
17. Derive an expression for Van't Hoff factor for a solute undergoing association. 3
18. Differentiate between 'Bond Dissociation Energy' and 'Bond Enthalpy' with the help of one example each. 3
19. Starting from the definition of Helmholtz free energy derive relations for its variation with
temperature at a constant volume, and
volume at a constant temperature. 3
20. What is an ideal solution? When 100 cm^3 of liquid A and 250 cm^3 of liquid B were mixed, the volume of the solution formed was 353 cm^3. What type of solution is it, ideal or non-ideal Give another example of such solutions. 3
21. Differentiate between 'activated complex' and 'transition state'.
What is transmission coefficient? 3
PART D
Answer any five questions. 5x4=20
22. Calculate DG° for the reaction occurring in the following cell 4
Al Cu
Standard electrode potentials
E° Al3+/Al =-1.66V and E° =+0.34V.
23. State the two laws of photochemistry. Define quantum efficiency for the formation of a product. Why do some reactions show very high quantum efficiency? 4
24. Two electrolytic cells were connected in series. In one
an AgNO3 solution and in the other
500 cm^3 of a solution in which 10.0 g of CuS04 . 5 H20 is dissolved are present. After passing electric current for 30 minutes, it was found that 1.307 g silver has been deposited. Calculate the concentration of copper expressed in gram per litre in the copper sulphate solution after the electrolysis.
[Atomic masses are: Cu 63.54; Ag 108] 4
25. Explain the following phenomena and give their cause: 4
Brownian motion
Tyndall effect
26. Explain the principle of steam distillation. When a liquid which is immiscible with water was steam distilled at 95.6°C under a total pressure of 7.5x 10^4 Pa, the distillate contained 1.20 g of the liquid per gram of water. Calculate the molar mass of the liquid. Vapour pressure of water is 6.5 x 10^4 Pa at 95.6°C. 4
27. 2.0 g of benzoic acid dissolved in 25.0 g of benzene shows a depression in freezing point equal to 1.62 K. What is the percentage association of benzoic acid Kf for benzene is 4.9 K kg mol^-1. 4
28. Give the two statements of the second law of thermodynamics given by
Clausius and
Kelvin. What is the entropy change of 3.5 mol of an ideal gas during its isothermal and reversible expansion from 2.5 x m^3 to 0.25 4
I CHE-04 1
BACHELOR OF SCIENCE (B.Se.)
Term-End Examination
June, 2016
01.21.7
CHEMISTRY CHE-04 PHYSICAL CHEMISTRY
Time: 2 hours Maximum Marks: 50
Note: Attempt all the parts. Answer five questions from each ofthe parts C and D. .
PART A
Answer any five questions. 5x1=5
1. What is the S.I. unit of temperature? 1
2. State Graham's law of effusion of gases. 1
3. Name the crystal system whose unit cell has the following characteristics 1
a b c and a B 90°
4. Identify the type of thermodynamic system in each of the following cases 1
A sealed bottle of flavoured milk.
Ice in a closed thermos flask
5. Write the equation for the phase rule. 1
6. Explain why an aqueous solution of NH4Cl is acidic in nature. 1
7. Write the expression for the instantaneous rate of the following reaction in terms of changes in concentrations of O3 or O2 1
2 3
PART B
Answer any five questions. 5x2=10
8. Which among the following is expected to have the highest surface tension at room temperature water, methyl cyanide or methanol? State the reason also. 2
9. Differentiate between intrinsic and extrinsic semiconductors in terms of the origin of conductivity in them. 2
10. Identify the intensive and extensive variables from among the following: 2
Temperature of a body
Number of moles present in a substance
Quantity of cooking gas burnt for boiling milk
Specific heat
11. Give one example each of chemical reactions undergoing homogeneous catalysis and heterogeneous catalysis. 2
12. State the principle of corresponding states. 2
13. Addition of NH4Cl to an aqueous solution of NH40H results in a decrease of pH. Explain. 2
14. Explain the effect of
increase in pressure and
increase in temperature on the following reaction: 2
N2 3 H2 2 NH3 DrH° =-92.2 kJ mol^-1
PART C
Answer any five questions. 5x3=15
15. Derive Van der Waals equation from the ideal gas equation.
16. Draw a labelled phase diagram of Bi -Cd system. 3
17. Derive an expression for Van't Hoff factor for a solute undergoing association. 3
18. Differentiate between 'Bond Dissociation Energy' and 'Bond Enthalpy' with the help of one example each. 3
19. Starting from the definition of Helmholtz free energy derive relations for its variation with
temperature at a constant volume, and
volume at a constant temperature. 3
20. What is an ideal solution? When 100 cm^3 of liquid A and 250 cm^3 of liquid B were mixed, the volume of the solution formed was 353 cm^3. What type of solution is it, ideal or non-ideal Give another example of such solutions. 3
21. Differentiate between 'activated complex' and 'transition state'.
What is transmission coefficient? 3
PART D
Answer any five questions. 5x4=20
22. Calculate DG° for the reaction occurring in the following cell 4
Al Cu
Standard electrode potentials
E° Al3+/Al =-1.66V and E° =+0.34V.
23. State the two laws of photochemistry. Define quantum efficiency for the formation of a product. Why do some reactions show very high quantum efficiency? 4
24. Two electrolytic cells were connected in series. In one
an AgNO3 solution and in the other
500 cm^3 of a solution in which 10.0 g of CuS04 . 5 H20 is dissolved are present. After passing electric current for 30 minutes, it was found that 1.307 g silver has been deposited. Calculate the concentration of copper expressed in gram per litre in the copper sulphate solution after the electrolysis.
[Atomic masses are: Cu 63.54; Ag 108] 4
25. Explain the following phenomena and give their cause: 4
Brownian motion
Tyndall effect
26. Explain the principle of steam distillation. When a liquid which is immiscible with water was steam distilled at 95.6°C under a total pressure of 7.5x 10^4 Pa, the distillate contained 1.20 g of the liquid per gram of water. Calculate the molar mass of the liquid. Vapour pressure of water is 6.5 x 10^4 Pa at 95.6°C. 4
27. 2.0 g of benzoic acid dissolved in 25.0 g of benzene shows a depression in freezing point equal to 1.62 K. What is the percentage association of benzoic acid Kf for benzene is 4.9 K kg mol^-1. 4
28. Give the two statements of the second law of thermodynamics given by
Clausius and
Kelvin. What is the entropy change of 3.5 mol of an ideal gas during its isothermal and reversible expansion from 2.5 x m^3 to 0.25 4
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