Download SGBAU B-Tech 2nd Sem FPOPC Poly Plast Applied Physical Chemistry I Question Paper

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TSUANKET Second Semester Examination

11708 : Applied Physical Chemistry - I

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AW -2931 Pages: 3

Time : Three Hours Max. Marks : 80

Notes:

1. Answer three questions from Section A and three questions from Section B.
2. Due credit will be given to neatness and adequate dimensions.

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3. Assume suitable data wherever necessary.
4. Diagrams and chemical equations should be given wherever necessary.
5. Use of pen Blue/Black ink/refill only for writing the answer book.

SECTION - A

1. 1. Define activity coefficient and describe the experimental method of determination of activity and activity coefficient. 6

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   2. Explain in brief, Heisenberg's uncertainty principle. 4
   3. What is an ideal solution ? Write the statement of Raoult's law. 3

   OR

2. 1. Discuss the application of Schrodinger equation for determination of energy of a particle confined in one dimensional potential well. 6

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   2. Show that, λ = h/p, where h is plank constant, λ is wave length and p is momentum. 4
   3. Define: 3
      1. Rigid rotator
      2. Zero point energy and
      3. Wave number

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3. 1. State the law of corresponding state and deduce the reduced form of Van-der-Waals equation. 4
   2. Define the terms : 3
      1. Mean free path
      2. Co-volume of gas
      3. Compressibility factor

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   3. Derive an equation PV = 1/3 mnc² 6

   OR

4. 1. Discuss the Maxwell Boltzmann's law of distribution of molecular speed and express the formula for average velocity. 6

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   2. Write the assumptions of kinetic theory of gases. 4

AW -2931 1 P.T.O

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Calculate the pressure exerted by 1 mol of gas at 300 k having volume 1.32 dm³ using Van-der-Waal's equation. The Van-der-Waal's constants are, a = 3.59 dm⁶ atm mol^-2 and b=0.0427 dm³ mol^-1 (R =0.08206 dm³ atm k^-1 mol^-1).

5. 1. What is collision frequency ? Derive an expression for collision number. 6
   2. Define: 4
      1. Root mean square velocity
      2. Average velocity
      3. Most probable velocity

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      4. Collision diameters
   3. Calculate r.m.s and average speed of oxygen molecule at 273 k. (R=8314 kgm² s^-2 k^-1 mol^-1) 3

   OR

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6. 1. Express the three critical constants in terms of Van-der-Waal's constants using Van-der-Waal's equation. 6
   2. Discuss the heat conduction in gases. 4
   3. The density of carbon monoxide at 0°C at 1 atm is 1.2504 kg m^-3. Calculate the average and most probable speeds. 3

SECTION-B

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7. 1. Give the difference between order and molecularity. 4
   2. Define zero order reaction with suitable examples. 3
   3. Derive an integrated rate equation of second order reaction for equal initial concentration of reactants. 6

   OR

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8. 1. Discuss the effect of following factors on reaction rate : 6
      1. Surface area of reactant
      2. Temperature
   2. Show that, if one of the reactant is present in large excess in reaction vessel, the second order reaction follows first order kinetic equation. 4
   3. In a second order reaction, where the initial concentration of the reactants is the same, half of the reactants are consumed in 6 minutes. If the specific reaction rate is 5x10^-2 mol^-1 dm³ min^-1, what is the initial concentration of the reactants. 3

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9. 1. Discuss the Ostwald isolation method. 6

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9. 1. In first order reaction, the concentration is reduced to 1/4 of its initial value in 60 minutes. Calculate the rate constant of the reaction. 4
   2. In a first order reaction, the initial concentration is halved, the half-life period is 25 minutes. What is order of reaction ? 3
   3. What is energy of activation ? How does it calculate from Arrhenius equation ? 6

   OR

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10. 1. Discuss the following methods of determination of order of reaction. 6
       1. Van't - Hoff's differential method.
       2. Fractional change method.
    2. Write the limitations of Integration method. 4

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    3. The specific rate constants of second order reaction are 0.03466 mol^-1 dm³ min^-1 and 0.13864 mol^-1 dm³ min^-1 at temperatures 300 k and 350 k respectively. Calculate energy of activation (R = 8.314J) 3
11. 1. Define the following thermodynamic systems and processes. 6
       1. Open system
       2. Isolated system
       3. Adiabatic process

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       4. Isobaric process
    2. Write any two statements of second law of thermodynamic. 4
    3. Define Gibb's free energy and explain the spontaneity of chemical reaction. 3

    OR

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12. 1. State the first law of thermodynamics and derive its mathematical equation. 6
    2. What do you mean by state function ? Give any three examples of state functions. 4
    3. Derive Gibb's Helmholtz equation. 3

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