Assignment%203 - -1 at its boiling point, 334.88 K....

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Assignment 3 CHM 2131 Due: Nov. 6 Q1.  Consider the following system: 1.0 moles of an ideal gas initial contained in a 1L balloon at 298  K.  The gas is heated to 350 K and expands to 5 L.  Determine the entropy change for this expansion  following three reversible pathways:  a) Pathway 1: Isothermal expansion 1L  à  5L followed by constant volume heating. b) Pathway 2: Reversible expansion against constant external pressure Pi to 350 K followed by  constant T expansion to 5 L c) Pathway 3: Reversible adiabatic expansion to 5L followed by constant volume heating.   Which process requires the greatest input of heat ? Q2. The enthalpy of vaporization of chloroform is 29.4 kJ mol
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Unformatted text preview: -1 at its boiling point, 334.88 K. Calculate (a) the entropy of vaporization of chloroform at its boiling point and (b) the entropy change of the surroundings. Q3. Calculate the change in the entropies of the system and the surroundings, and the total change in entropy, when a sample of N 2 (g) of mass 14 g at 298 K and 1.5 bar increases from 1.2 l to 4.6 l in (a) an isothermal reversible expansion, (b) an isothermal irreversible expansion against p ex = 0, and (c) an adiabatic reversible expansion. Q4. Suppose that 3.0 mmole N 2 (g) occupies 36 cm 3 at 300 K and expands to 60 cm 3 . Calculate ∆ G for the process....
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This note was uploaded on 02/23/2010 for the course CHM Chm3120 taught by Professor Olgilvie during the Fall '09 term at University of Ottawa.

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