lyon practice Exam 3 - Exam 3 — Due: Oct 27 2006, 5:00 pm...

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Unformatted text preview: Exam 3 — Due: Oct 27 2006, 5:00 pm — lnst: Donna C Lyon 1 This print—out should have 20 questions. Multiple—choice questions may continue on the next column or page — find all choices before answering. The due time is Central time. 001 (part 1 of 1) 10 points Which of the following can form intermolecu— lar hydrogen bonds? 1. CflchgCHgCHgCHg 2. Ang 3. CH30H 4. CflgOCHg 5. HBr Explanation: 002 (part 1 of 1) 10 points A mixture of 0.75 mol H2 gas and 0.75 mol N2 gas is introduced into a 15 liters container having a pinhole leak at 3000. After a period of time. which of the following is true? 1. The partial pressure of N2 exceeds that of H2 in the container. 2. The partial pressures of the two gases change, but they remain equal. 3. The partial pressure of Hg exceeds that of N2 in the container. 4. The partial pressures of both gases in— crease above their initial values. Explanation: 003 (part 1 of 1) 10 points Real gases behave most nearly like ideal gases at 1. low temperatures and high pressures. 2. high pressures and low molar masses. 3. low temperatures and low pressures. 4. high temperatures and high pressures. 5. high temperatures and low pressures. Explanation: 004 (part 1 of 1) 10 points A 0.479 g sample of nitrogen, oxygen or neon gas occupies a volume of 265 mL at 157 kPa and 2000. What is the molar mass and iden— tity of the gas? 1. 14.0 g . mol_1., N 2. 28.0 g . mol_1., N2 3. 32.0 g*]fI10l—1.Og 4. 20.1 g * mol_1., Ne 5. 16.0 g . mol_1., o Explanation: 005 (part 1 of 1) 10 points A gaseous mixture made from 6.00 grams of oxygen gas and 9.00 grams of chlorine gas is placed in a 15.0 L vessel at 10.0 degrees Celsius. What is the total pressure in the vessel? — Exam 3 — Due: Oct 27 2006, 5:00 pm — lnst: Donna C Lyon 2 1. 0.800 atm 2. 0.488 atm 3. 1.00 atm 4. 0.655 atm 5. 0.244 atm Explanation: 006 (part 1 of 1) 10 points Which of the following statements about the Kinetic—Molecular Theory of gases is false? 1. The distance between molecules is much larger than the diameter of each molecule. 2. Collisions between molecules are elastic. 3. The average kinetic energy of a gas molecule is independent of the temperature. 4. Gases consist of molecules in continuous. random motion. 007 (part 1 of 1) 10 points The main composition of dry air at sea level is about 75.5% nitrogen. 23.1% oxygen. and 1.3% argon. ln a 1.00 g sample of dry air at 1.00 atm. calculate the partial pressure of argon gas. 1. 0.43 >< 10—3 atm 2. 10.2 >< 10—3 atm 3. 4.17 >< 10—3 atm 4. 3.33 >< 10—3 atm 5. 5.45 >< 10—3 atm Explanation: 008 (part 1 of l) 10 points Consider the following van der Waals coeffi— cients: 0.034 0.0237 hydrogen 0.244 0.0266 0.211 0.0171 krypton 0.0398 0.0511 0.0562 0.0427 0.0371 0.0305 Which of the following gases has the largest attractive forces? 1. ammonia 2. chlorine 3. water 4. helium 5. neon Explanation: 009 (part 1 of l) 10 points At STP. 0500 L of fluorine gas will have a mass of 1. 12.3 g. 2. 0.424 g. 3. 19.0 g. 4. 11.2 g. 5. 0.343 g. Explanation: 010 (part 1 of l) 10 points A sample of neon (Ne) occupies 1700 mL at — Exam 3 — Due: Oct 27 2006; 5:00 pm — lnst: Donna C Lyon 3 STP. At constant pressure; what temperature is necessary to increase the volume to 2100 mL? 1. —14DC 2. 3200 3. 6400 4. 5200 5. —52DC Explanation: 011 (part 1 of 1) 10 points Adhesive forces are forces 1. Neither of these is correct. 2. between the molecules of a liquid. 3. between the molecules of the liquid and another surface. Explanation: 012 (part 1 of 1) 10 points What is the density of nitrogen gas at STP? 1. 2.50 g/L 2. 1.25 g/L 3. 0.500 g/L 4. 4.00 g/L 5. 0.525 g/L Explanation: 013 (part 1 of 1) 10 points What type of intermolecular forces would you expect to find in a pure liquid sample of HCl? 1.London 2. There would be no intermolecular forces in this sample. 3. hydrogen bonding 4. dipole—dipole 5. interionic Explanation: 014 (part 1 of 1) 10 points The properties of a given substance are gov— erned by various forces or interactions. Con— sider the following 4 forces or interactions: covalent bonding dispersion forces hydrogen bonding dipole—dipole interactions Which of the following correctly lists these four types of interactions/ forces according to increasing strength (weakest to strongest)? 1. hydrogen; dispersion; covalent; dipole 2. dispersion; dipole; hydrogen; covalent 3. hydrogen; dipole; covalent; dispersion — Exam 3 — Due: Oct 27 2006; 5:00 pm — lnst: Donna C Lyon 4 4. dispersion; hydrogen; dipole; covalent 016 (part 1 of 1) 10 points Consider the solids 5. covalent; hydrogen; dipole; dispersion ice (solid); CsCl (solid); and Fe (solid) . Which of the following correctly identifies the type of solid for Fe; CsCl; and ice; respec— tively? 1. molecular; crystalline; ionic 2. metallic; ionic; molecular 3. molecular; ionic; metallic 4. metallic; ionic; covalent 5. metallic; covalent; ionic 015 (part 1 of 1) 10 points At constant temperature if the volume of a gas sample is tripled the pressure will 1. be increased by a factor of 6. 017 (part 1 of 1) 10 points 2. 1:) th' d th ' ' l. . . 8 one If e orlgma Whlch would you expect to be most v1scous? 3. remain the same. 1. CSH18 at 5000 4. be cut in half. 2. C4H8 at 3000 5. be tripled. Explanation: 3. 041—18 8.1; 5000 4. (3ng8 at 3000 Explanation: 018 (part 1 of 1) 10 points Which of the following is a true statement about a fixed amount of ideal gas at constant pressure? 1. If a sample of gas is heated from 10000 to — Exam 3 — Due: Oct 27 2006, 5:00 pm — lnst: Donna C Lyon 5 20000., the volume will decrease by a factor of Consider the reaction two. 4 KOfls) + 2 002 (g) a 2 K2003(S) + 3 02(g). 2. If a sample of gas is heated from 000 to Hovv much oxygen is produced at STP if 27300, the volume will double. 10.5 moles of carbon dioxide are used at STP? 3. If a sample of gas is cooled from 40000 to 1. 15.8 L 20000., the volume will decrease by a factor of two. 2. 706 L Explanation: 3. 0703 L 4. 235 L 5. 353 L Explanation: 019 (part 1 of 1) 10 points What is the molecular weight of a (hypothet— ical) gas that diffuses 1.414 times faster than nitrogen (N2)? 1. 14.0 g/mol 2. 46.6 g/mol 3. 23.5 g/mol 4. 32.6 g/mol 5. 4.85 g/mol Explanation: 020 (part 1 of 1) 10 points ...
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This note was uploaded on 02/04/2010 for the course CH 301 taught by Professor Fakhreddine/lyon during the Fall '07 term at University of Texas at Austin.

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lyon practice Exam 3 - Exam 3 — Due: Oct 27 2006, 5:00 pm...

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