Thermo - Thermodynamics Question 1(1 point 1-4 When 44.0 g of solid carbon dioxide at 1.00 atm pressure is reversibly converted to vapour at 1 atm

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Thermodynamics Question 1 (1 point) 1-4. When 44.0 g of solid carbon dioxide at 1.00 atm pressure is reversibly converted to vapour at 1 atm pressure and -78°C, 25.33 kJ of heat is absorbed by the system. The density of solid CO 2 is 1.56 g cm -3 . 1. ΔH for this process is a. -23.71 kJ b. +23.71 kJ c. -25.33 kJ d. +25.33 kJ e. +26.95 kJ Question 2 (1 point) 2. ΔS for the process is nearest to a. 130.0 J K -1 b. -130.0 J K -1 c. 121.5 J K -1 d. -121.5 J K -1 e. 138.1 J K -1 Question 3 (1 point) 3. ΔG for the process is a. 50.66 kJ b. -50.66 kJ c. -46.71 kJ d. 46.71 kJ e. 0 kJ Question 4 (1 point) 4. If S° of CO 2 (g) is 197.7 J K -1 mole -1 at -78 °C, the standard entropy of solid CO 2 is nearest to: a. 67.70 J K -1 b. -67.70 J K -1 c. 327.7 J K -1 d. 0 J K -1 e. 130.0 J K -1 Question 5 (1 point) 5. Given the following data at 298 K, evaluate the standard enthalpy of formation of ICl(g) at 298 K (in kJ mole - 1 ). ΔH° = 242.0 kJ mol -1 for: Cl 2 (g) → 2Cl(g) ΔH° = 151.0 kJ mol -1 for: I 2 (g) → 2I(g) ΔH° = 211.2 kJ mol
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This note was uploaded on 04/19/2008 for the course CHEM 121 taught by Professor Donnecke during the Winter '07 term at The University of British Columbia.

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Thermo - Thermodynamics Question 1(1 point 1-4 When 44.0 g of solid carbon dioxide at 1.00 atm pressure is reversibly converted to vapour at 1 atm

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