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# Hw3 - (C Finally the gas is cooled reversible and...

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CHEM 342 Physical Chemistry I Fall 2006 Problem set 3 Due 09/19/2006 (Monday) 1. Textbook 3.4 2. Textbook 3.12 3. Textbook 3.14 4. Textbook 3.30 or 3.32 5. Textbook 3.38 6. One mole of a van der Waals gas at 298.15 K expands isothermally and reversibly from 10 to 30 liters. Compute the work w. (a=5 L 2 atm mole -2 , b=0.03 L/mole). 7. One mole of an ideal gas at 298.15 K is expanded adiabatically to a final P=1 atm against a constant opposing pressure P=1 atm. Calculate T final , q, w, U, H for C V =7/2 R. 8. An ideal monatomic gas (C v =3/2 R, C p =5/2R) is subject to the following steps: (A) The gas is heated reversibly at a constant pressure of 1 atm from 25 0 C to 100 0 C. (In a reversible heating process direct heat flow must occur between vanishingly small temperature differences, just as reversible expansion and compression must involve infinitesimal differences in pressure between the opposing pressure and the pressure of the gas.) (B) The gas is expanded reversibly and isothermally to double its volume.
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Unformatted text preview: (C) Finally the gas is cooled reversible and adiabatically to 35 C. Calculate U, H, q, and w for the whole process (A+B+C). 9. (a) 10 g of ice at –10 C are dropped into 25 g of water at 15 C, and the system is allowed to reach equilibrium adiabatically. What is the final state of affairs? C v (water) = 1.0 cal g-1 K-1 , C v (ice) = 0.5 cal g-1 K-1 , and the H fusion =80 cal g-1 . (b) Suppose that 10 g of ice at -10 C were dropped into 100 g of water at 15 C and the system is allowed to reach equilibrium adiabatically. What would be the final state of affairs? 10. 0.5 mole of CH 4 at 25 C is exploded in a large excess, 10 moles of Oxygen, burning completely to CO 2 and water. Calculate the final temperature under adiabatic conditions, H vaporization (H 2 0) = 40.656 kJ mol-1 . Hint: H 2 O(g) and H 2 O(l) have different heat capacity. (a) assuming the explosion to be at constant pressure (b) assuming it to be at constant volume...
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