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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- Fall '08
- Thermodynamics, Fundamental physics concepts, reversible isothermal expansion, constant external pressure, kJ mol1