Chemistry 1465-001 Name (please print)________________________________________ Test #2 Last name, First name Brown/Holme, Chapters 5, 6, and 7 __________ June 22, 2010 Seat Number Instructions: 1. This exam consists of 25 questions. Select the one best answer to each question. 2. No scratch paper is allowed. You may do the work in the test margins and on the backs of the test pages. 3. Mark the answers you choose on the test itself for your own information and also on the standard answer sheet you provided. Scoring will be based on the answer sheet. 4. When you finish, turn in both the test form and the answer form. Write your name on both forms. Useful Information: NA = 6.022 x 1023 c = 2.998 x 108 m/s h = 6.626 x 10-34 J.s 1. A small canister of compressed gas has a volume of 25.0 L. If the pressure of the gas is 35.0 atm at 25°C, what volume would the gas occupy under STP conditions? a) 875 L b) 802 L c) 955 L d) 213 L e) 350 L 2. A certain amount of gas in a rigid container is heated from 200°C to 400°C. Which of the following responses best describes what will happen to the pressure of the gas? a) The pressure will remain the same. b) The pressure will increase by a factor of 2. c) The pressure will decrease by a factor of 2. d) The pressure will increase by a factor greater than 2. e) The pressure will increase by a factor less than 2.2 3. You and a friend have gas samples in open manometers as shown: You have Hg(l) in your manometer and your friend has water. The height h is the same in both manometers. Which of the following statements is true? a) Your sample of gas has the higher pressure. b) Your friend’s sample of gas has the higher pressure. c) Both samples of gas have the same pressure. d) There is not enough information to answer the question. e) None of these is correct. 4. If a 5.00 L steel cylinder contains nitrogen gas at a pressure of 22.5 atm at 25ºC, what mass of nitrogen is in the cylinder? a) 4.60 g b) 64.4 g c) 57.6 g d) 129 g e) 32.2 g 5. A flask with a volume of 3.16 L contains 9.33 grams of an unknown gas at 32.0°C and 1.00 atm. What is the molar mass of the gas? a) 10.3 g/mol b) 73.9 g/mol c) 7.76 g/mol d) 98.0 g/mol e) 1.18 g/mol 6. Fluorine gas reacts with solid calcium bromide to form calcium fluoride and liquid bromine. What volume of fluorine gas (in mL) is required to react with 2.67 g of calcium bromide at 41°C and 4.31 atm? a) 10.4 mL b) 210. mL c) 420. mL d) 79.9 mL e) 104 mL 7. A flask contains a mixture of He(g) and Ne(g) at a total pressure of 7.50 atm. There are 2.50 mol of He and 4.25 mol of Ne in the flask. What is the partial pressure of He? a) 2.78 atm b) 1.88 atm c) 4.41 atm d) 4.72 atm e) 3.00 atm3 8. Consider two identical flasks filled with different gases: Flask A: N2 at 10.0 atm and 100°C Flask B: H2 at 0.500 atm and 100°C Which of the statements below are correct? I. The N2 molecules have a higher average kinetic energy than the H2 molecules. II. The H2 molecules have a higher average kinetic energy than the N2 molecules. III. The N2 molecules have the same average kinetic energy as the H2 molecules. IV. The N2 molecules have a higher average velocity than the H2 molecules. V. The H2 molecules have a higher average velocity than the N2 molecules. VI. The N2 molecules have the same average velocity as the H2 molecules. a) I and IV b) II and V c) III and VI d) III and V e) II and VI 9. The decomposition of potassium chlorate can be used to produce oxygen gas in the laboratory: 2KClO3(s)  2KCl(s) + 3O2(g) What volume of gas, measured under STP conditions, can be produced by the decomposition of 12.7 g of KClO3(s)? (The molar mass of KClO3 is 122.5 g/mol.) a) 4.65 L b) 3.48 L c) 1.55 L d) 2.32 L e) 6.97 L 10. List the following types of electromagnetic radiation in order of increasing wavelength: (i) the gamma rays produced by a radioactive nuclide used in medical imaging (ii) radiation from an FM radio station at 93.1 MHz on the dial (iii) a radio signal from an AM radio station at 680 kHz on the dial (iv) the yellow light from sodium-vapor streetlights (v) the red light of a light-emitting diode, such as in a calculator display a) iii < ii < iv < v < i b) i < iv < v < iii < ii c) i < v < iv < ii < iii d) i < v < iv < iii < ii e) i < iv < v < ii < iii 11. A photon of ultraviolet (UV) light possesses enough energy to mutate a strand of human DNA. What is the energy (in kJ) of one mole of photons having a wavelength of 15 nm? a) 470 kJ b) 940 kJ c) 8.0 x 103 kJ d) 8.0 x 104 kJ e) 1.3 x 10-17 kJ 12. What is the wavelength of a radio signal from KSCS FM operating at a frequency of 96.3 MHz? a) 3.11 m b) 0.321 m c) 0.0311 m d) 0.00311 m e) 289 m4 13. According to the aufbau procedure, which orbital is filled immediately after a 4d subshell is filled in a multielectron atom? a) 5s b) 6s c) 3p d) 4f e) 5p 14. What is the ground state electron configuration for Pb? a) [Xe] 6s2 6d10 6p2 b) [Xe] 6s2 5d10 6p2 c) [Xe] 6s2 4f14 5d10 6p2 d) [Xe] 6s2 3f14 4d10 5p2 e) [Xe] 7s2 4f14 5d10 6p2 15. Which of the following electron configurations is correct? a) Ga: [Kr] 4s23d104p1 b) Cu: [Ar] 4s23d9 c) Sn: [Kr] 5s25d105p2 d) Br: [Ar] 5s24d105p7 e) Bi: [Xe] 6s24f145d106p3 16. Comparing the size of the following atoms and ions, which is not expected to be true? a) N > F d) F- > Cl- b) Ba2+ > Mg2+ e) As > S c) F- > Al3+ 17. In which pair do both compounds exhibit predominantly ionic bonding? a) RbCl and CaO b) Na2SO3 and BH3 c) KI and O3 d) NaF and H2O e) PCl5 and HF 18. In the ion BrCl4–, how many lone pairs of electrons are around the central bromine atom? a) 0 b) 1 c) 2 d) 3 e) 4 19. Of those shown below, which of the following is the best Lewis structure for sulfur dioxide? a) d) b) e) c) O S OO S OO S OO S OO S O5 20. Of the atoms listed below, which is the most electronegative? a) Mg b) Si c) S d) As e) Se 21. Of the bonds listed below, which is …