24 kpa f 86 kpa 7 g 61 kpa h 57 kpa i 16x10 kpa

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Unformatted text preview: at 500.K. Given that the process is at equilibrium at 300.K and that the entropy change and enthalpy change associated with this process are independent of temperature, calculate the free energy change for this process at 363 K. a) 950. J b) 1080 J c) 1260 J d) 1930 J e) 2740 J f) 4500 J g) 5420 J h) 6280 J Show your calculations. Question 18: (5 points) Which equation correctly describes the change in the vapor pressure above a pure liquid with temperature? Show your derivation for any credit! " P2 % Δ subH " 1 1 % '= $−' R # T1 T2 & # P1 & Δ fus V $ T2 ' ln& ) e) P2 − P1 = Δ fusH % T1 ( € a) ln$ € € " % " 1 1% −' P1 & R # T2 T1 & # %T ( f) P2 − P1 = Δ vapH × ln' 2 * & T1 ) € b) ln$ P2 ' = Δ subH $ " % H" % c) ln$ P2 ' = vap $ 1 − 1 ' R # T1 T2 & # P1 & " P2 % Δ fusH " 1 1 % g) ln$ ' = $−' # P1 & R # T1 T2 & Δ !P $ Δ H ! 1 # P1 & R # T2 Question 19: (5 points) € € € Indicate which, among the following statements, is incorrect o o a) µ(H2O(g), 90 C, 1 atm) > µ(H2O(l), 90 C, 1 atm) o o b) µ(H2O(s), 0 C, 1 atm) = µ(H2O(l), 0 C, 1 atm) o o c) µ(H2O(l), 25 C, 1 atm) < µ(H2O(l), 25 C, 5 atm) o o d) µ (H2O(l), 25 C, 1 atm) < µ (H2O(l), 45 C, 1 atm) o o e) µ(H2O(l), 25 C, 1 atm) < µ(H2O(s), 25 C, 1 atm) o o f) µ(H2O(l), 25 C, 1 atm) < µ(H2O(g), 25 C, 1 atm) o o g) µ(H2O(s), - 10 C, 1 atm) < µ(H2O(g), - 10 C, 1 atm) o o h) µ(H2O(l), 100 C, 1 atm) = µ(H2O(g), 100 C, 1 atm) Justify your answer. Question 20: (5 points) Which among the following expressions is a...
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This note was uploaded on 01/26/2014 for the course CHEM 3615 taught by Professor Aresker during the Spring '07 term at Virginia Tech.

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