Download GTU B.Tech 2020 Summer 5th Sem 2150503 Chemical Engineering Thermodynamics Ii Question Paper

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GUJARAT TECHNOLOGICAL UNIVERSITY
BE - SEMESTER- V EXAMINATION - SUMMER 2020

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Instructions:

1. Attempt all questions.

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2. Make suitable assumptions wherever necessary.
3. Figures to the right indicate full marks.

MARKS

Q.1

1. (a) What are the characteristics of an ideal solution ? 03

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2. (b) Discuss any two methods to determine fugacity of pure gases. 04
3. (c) Answer the followings: 07
   1. What do you mean by activity of pure fluid? How would you estimate activity of an incompressible fluid? 02
   2. How activity coefficient is related to the molar Excess Gibbs free energy in solution ? 01
   3. Why does the boiling point diagram at high pressures lie above that at a lower pressure? 01
   4. What do you mean by “extent of reaction “? 01

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   5. What is the degree of freedom for the following non —reactive equilibrium system? Two partially miscible liquid phases are in equilibrium with vapor phase. 01
   6. How would you predict the feasibility of reaction from the value of the standard free energy change? 01

Q.2

1. (a) Discuss effect of increasing pressure on T-x-y diagram in brief. 03

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2. (b) Discuss Lewis-Randall rule, clearly mentioning its limitations. 04
3. (c) Define “Partial Molar property”. Describe different methods to determine partial molar properties in detail. 07

   OR

4. (c) Derive the equation for the criteria for phase equilibrium in terms of fugacity for mixture of N components and JI phases 07

Q.3

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1. (a) Discuss any two methods to check consistency of experimental VLE data in detail. 03
2. (b) Discuss effect of temperature and pressure on chemical potential. 04
3. (c) Prove that if Henry’s law is obeyed by component 1 in a binary solution over certain concentration range, Lewis-Randall rule will be obeyed by component 2 over the same concentration range. 07

   OR

Q.3

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1. (a) Discuss excess Gibbs free energy in brief. 03
2. (b) Discuss effect of temperature and pressure on equilibrium constant. 04
3. (c) Discuss van Laar and Margulies Equations in detail. 07

Q.4

1. (a) Discuss phase rule for non reacting systems in brief. 03

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2. (c) The vapour pressures of acetone(1) and acetonitrile (2) can be evaluated by the following Antoine equations, where P is in kPa and T is in K. 07

   lnP{ = 14.5463 - 294046 / (T —35.93)

   lnP§ = 142724 - 2945.47 / (T—49.15)

   Assuming ideal solutions, calculate

   1. x; and y; at 327 K and 65 kPa
   2. T and y; at 65 kPa and x1=0.4

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   3. P and y; at 327K and x; =0.4

   OR

Q.4

1. (a) Discuss Duhem’s Theorem briefly. 03

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2. (b) Write short note on VLE for completely immiscible systems with neat diagram. 04
3. (c) The partial molar volumes of acetone and chloroform in a mixture in which mole fraction of acetone is 0.5307 are 74.166x 10 ~® m³/mol and 80.235 x 10 ~® m³/mol respectively. What is the volume of 1 kg of the solution? 07

Q.5

1. (a) Discuss effect of presence of Excess of reactants and products on equilibrium conversion. 03
2. (b) Wilson’s parameters A12 and A21 for the system nitromethane (1) and carbon tetrachloride(2) at 45 °C are 0.1156 and 0.2879 respectively. Calculate the activity coefficients of the components in a solution containing 30 mol % nitromethane. 04

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3. (c) Derive equation for standard heat of reaction. 07

   OR

Q.5

1. (a) Discuss Heterogeneous reaction equilibria with reference to “reactions in solutions”. 03
2. (b) Calculate the fugacity of pure ethylene at 100 bar and 373 K. The van der Waals constants are a = 0.453 J m³/mol² and b = 0.571 x 10?4 m³/mol and molar volume at 100 bar and 373 K =2.072 x 10?4 m³/mol. 04

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3. (c) Discuss minimum and maximum boiling azeotropes with neat sketch. 07

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