PS4F07 - 3. a. Calculate S if 1 mol of liquid water is...

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Chemistry 391 Fall 2007 Problem Set 4 (Due, Monday October 1) 1. One mole of an ideal gas with C V = 3/2 R undergoes the transformations described in the following list from an initial state described by T = 300 K and P = 1.00 bar. Calculate q , w , Δ U , Δ H , and Δ S for each process. a. The gas is heated to 450 K at a constant external pressure of 1.00 bar. b. The gas is heated to 450 K at a constant volume corresponding to the initial volume. c. The gas undergoes a reversible isothermal expansion at 300 K until the pressure is half of its initial value. 2. Calculate Δ S surroundings and Δ S total = Δ S + Δ S surroundings for each of the processes described in Problem 1. Which of the processes is a spontaneous ( Δ S total >0) process? Note that the state of the surroundings for each part is as follows: a. 450 K, 1 bar b. 450 K, 1 bar c. 300 K, 0.500 bar
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Unformatted text preview: 3. a. Calculate S if 1 mol of liquid water is heated from 0 to 100C under constant pressure if C P,m = 75.291 J K 1 mol 1 . b. The melting point of water at the pressure of interest is 0C and the enthalpy of fusion is 6.0095 kJ mol 1 . The boiling point is 100C and the enthalpy of vaporization is 40.6563 kJ mol 1 . Calculate S for the transformation H 2 O( s , 0C) H 2 O( g , 100C). 4. One mole of H 2 O( l ) is compressed from a state described by P = 1.00 bar and T = 298 K to a state described by P = 800 bar and T = 450 K. In addition, = 2.07 10 4 K 1 and the density can be assumed to be constant at the value 997 kg m 3 . Calculate S for this transformation, assuming that = 0. You will need the Appendix in Levine, and see Section 4.6....
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This note was uploaded on 07/25/2008 for the course CEM 391 taught by Professor Cuckier during the Fall '08 term at Michigan State University.

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