# Test I and answers - I CFE QUIZ 1 JULY 2009 Assume the missing data and mention the assumptions in your calculations Part A Answer all the

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I CFE QUIZ 1 JULY 2009 Assume the missing data and mention the assumptions in your calculations Part A Answer all the questions (10 x 1 = 10 Marks) 1. A thermos flask is an example for (a) Isolated system (b) Closed system (c) Open system (d) Heterogeneous system 2. The mathematical relation for the first law of thermodynamics is (a) ∆E = q-w (b) ∆E = 0 for a cyclic process (c) ∆E = q for an isochoric process (d) all of these 3. The change in free energy is a measure of (a) net work done (b) net change in entropy (c) net change in enthalpy (d) net change in internal energy 4. The efficiency of heat engine is maximum when (a) Temperature of source and sink are equal (b) source temperature is high than sink (c) sink temperature is high than source (d) All of these 5. The triple point of most fluids is close to (a) Boling point (b) Melting point (c) Critical Point (d) None of above 6. Which of the following has a negative value for a reaction that occurs spontaneously, that is, one that is a feasible reaction? (a) ∆G (b) ∆H (c) ∆S (d) Specific heat capacity 7. In a reaction where entropy decreases, it is found that the reaction has a positive Delta G, but becomes spontaneous as the temperature decreases. Which of the following is true? (a) ∆S and ∆H both are positive (b) ∆ S and ∆H both are negative (c) ∆ S is positive and ∆H both is negative (d) ∆ S is negative and ∆H both is positive 8. A spontaneous reaction always occurs when: (a) H o < 0 and S o < 0 (b) H o > 0 and S o < 0 (c) H o < 0 and S o > 0 (d) H o > 0 and S o > 0 9. Which of the following is not correct? (a) H = E + PV (b) H - E = PV (c) H - E – PV = 0 (d) H = E - PV 10. When water is cooled to ice, its entropy (a) Increases (b) decreases (c) remains the same (d) becomes zero Dr. TVN. Padmesh Turn Over 1

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I CFE QUIZ 1 JULY 2009 Part B Answer all the questions (5 x 2 = 10 Marks) 1. Define the Enthalpy & Gibbs free energy 2. Define Internal Energy 3. Distinguish between Reversible and Irreversible processes with suitable examples 4. Explain the terms “intensive property” and “extensive property” 5. What is standard free energy change in the case of a chemical reaction? Part C Answer any two questions (2 x 10 = 20 Marks) 1. (a) Calculate the maximum work done when pressure on 10 g of hydrogen is reduced from 20 to one atmosphere at a constant temperature of 273 K. The gas behaves ideally. Will there be any change in internal energy? Also calculate ‘q’. (b) Calculate the equilibrium constant at 25 ° C for the following reaction: AgCl (s) Ag + (aq) + Cl - (aq) ∆G o = +55.6 kJ/mol; R = 8.314 J/mol.K 2. Calculate ∆H for the following reaction: H 2 (g) + Cl 2 (g) 2HCl(g) Given the following: NH 3 (g) + HCl (g) NH 4 Cl(s) ∆H = -176 kJ N 2 (g) + 3H 2 (g) 2NH 3 (g) ∆H = -92 kJ N 2 (g) + 4H 2 (g) + Cl 2 (g) 2NH 4 Cl(s) ∆H = -629 kJ 4. 3 kg of an ideal gas is expanded from a pressure 7 bar and volume 1.5 m 3 to a pressure 1.4
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## This note was uploaded on 06/06/2011 for the course CHEM 3040 taught by Professor Reddy during the Spring '10 term at Taylor's.

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Test I and answers - I CFE QUIZ 1 JULY 2009 Assume the missing data and mention the assumptions in your calculations Part A Answer all the

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