hw10 - Gu Phillip Homework 10 Due Dec 7 2007 11:00 pm Inst...

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Gu, Phillip – Homework 10 – Due: Dec 7 2007, 11:00 pm – Inst: Brodbelt 1 This print-out should have 15 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. The due time is Central time. Brodbelt CH301 HW 10 Due December 7, 11:00 pm 001 (part 1 of 1) 10 points “You can’t unscramble an egg” might be a layman’s view of 1. the second law of thermodynamics. cor- rect 2. the woeful lament of a student contem- plating checking his work on an exam. 3. the first law of thermodynamics. 4. the third law of thermodynamics. Explanation: The Second Law of Thermodynamics states that in spontaneous changes the universe tends toward a state of greater disorder. 002 (part 1 of 1) 10 points Which substance has the lower molar en- tropy? 1. O 2 (g) at 450 K and 1.00 atm 2. O 2 (g) at 273 K and 1.00 atm correct 3. Unable to determine 4. They are the same Explanation: O 2 (g) at 450 K has increased molecular randomness (1 mol of O 2 at 1.00 atm pressure will occupy a larger volume at 450 K than at 273 K), hence a higher molar entropy. 003 (part 1 of 1) 10 points Without performing any calculations, de- termine whether the entropy of the system increases or decreases in Cl 2 (g) + H 2 O( ) HCl(aq) + HClO(aq) 1. Unable to determine 2. The entropy does not change. 3. increases 4. decreases correct Explanation: Entropy should decrease because there are fewer moles of gas on the product side of the reaction. 004 (part 1 of 1) 10 points The temperature of 2.00 mol Ne(g) is in- creased from 25 C to 200 C at constant pres- sure. Assume the heat capacity of Ne is 20.8 J/K-mol. Calculate the change in the entropy of neon. Assume ideal behavior. 1. +19.2 J · K - 1 correct 2. - 19.2 J · K - 1 3. +9.60 J · K - 1 4. +7.68 J · K - 1 5. - 7.68 J · K - 1 Explanation: 005 (part 1 of 1) 10 points Consider the following processes. (Treat all gases as ideal.) I) The pressure of one mole of oxygen gas is allowed to double isothermally.
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