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# PS4F07 - 3 a Calculate Δ 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 Δ S if 1 mol of liquid water is heated from 0º to 100ºC 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 0ºC and the enthalpy of fusion is 6.0095 kJ mol –1 . The boiling point is 100ºC and the enthalpy of vaporization is 40.6563 kJ mol –1 . Calculate Δ S for the transformation H 2 O( s , 0ºC) → H 2 O( g , 100ºC). 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, α = 2.07 × 10 –4 K –1 and the density can be assumed to be constant at the value 997 kg m –3 . Calculate Δ S for this transformation, assuming that κ = 0. You will need the Appendix in Levine, and see Section 4.6....
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