ÐÏࡱá>þÿ )KþÿÿÿP#*ÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿì¥Ás ¿48jbjbÀ À †ªkªkd0ÿÿÿÿÿÿ]¸¸¸¸¸¸¸°°°°8è,l°ÿ'Z¤¨¾¾¾¾¾¾t'v'v'v'v'v'v',Y)ôM+L¢']¸¾¾¾¾¾¢'æ ¸¸¾¾¤æ æ æ ¾°¸¾¸¾t'Ìr>r¸¸¸¸¾t'æ fæ L´%”¸¸t'€$óÉ’¸°°nxH',Printed Last Name: |___|___|___|___|___|___|___|___|___|___|___|___| Printed First Name: |___|___|___|___|___|___|___|___|___|___|___|___| Social Security # |___|___|___| |___|___| |___|___|___| School: |___|Barnard |___|College |___|Engineering |___|General Studies Chemistry 1404y Exam 1 February 18, 2002 Instructions Fill in your name and CUID number as indicated above. On the bubble sheet: 1) On Side 2 of the Bubble Sheet print your first and last name in the box provided. 2) Then fill in the Identification No. in the space provided and as indicated. Your Identification No. is your Social Security Number. 3) Using a soft lead pencil, blacken the one response that best answers the question or completes the statement. There is only one correct answer to each question. Any question with more than one answer will not be counted. Your score will be the total number of correct answers; therefore, it is to your advantage to answer every question. 4) There are 27 questions. They are equally weighted. Under no circumstances are you to make any other marks... anywhere on the bubble sheet... except in the appropriate bubbles for marking an answer you believe to be correct. You may write on the exam sheets themselves for the purpose of doing calculations.... but do not write on the bubble sheet. A periodic table of the elements can be found on page10 of this exam. A SCRATCH SHEET is provided on PAGE 11. Check the front blackboard for time remaining, last-minute corrections and additional information. You will have 75 minutes to complete the exam. When you have finished the exam or at the end of the allowed time, deposit your exam questions and bubble sheets in the separate boxes provided at the front of the room. Do not forget! Print your first and last names in the box provided (1) on the bubble sheet, and (2) on the front page of the 11 pages of this exam. Remember! It is your responsibility to ensure that your bubble sheet and exam sheets are properly identified. 1. Nearly monochromatic light waves are produced by... 1) the Sun 2) an incandescent light filament 3) a red hot charcoal briquet 4) a laser pointer 5) a bunsen burner 2. The following graph shows the annual variation in atmospheric carbon dioxide concentration as recorded at the Mauna Loa observatory (Hawaii). To reduce this steady increase in atmospheric carbon dioxide (and its apparent contributions to global warming), it would be LEAST effective to limit …. 1. use of natural gas as fuel rather than coal or petroleum. 2. use of nuclear or solar energy instead of fossil fuels for electricity generation. 3. use of automobiles. 4. production of beef. 5. rates of deforestation.  3. Of the following molecules, the one(s) exhibiting NO C-to-C multiple bond infrared stretching frequencies is (are)….. a) H2C=CH2 ethene (ethylene) b) HC=CH ethyne (acetylene) c) CH3HC=CH2 propene (propylene) d) CH3C=CH propyne (methyl acetylene) 1) (a) and( c) 2) (b) and (d) 3) (a) and (b) 4) (c) and (d) 5) all have multiple bond infrared stretching frequencies 4. As a general rule, bond strengths (increase, decrease) with increasing multiplicity as you move from C-to-C single, to double, then to triple bonds; and as a general rule, as the masses of the halogen (X) atoms in monohalomethanes (CH3-X) increase from F, to Cl, to Br, the stretching frequencies can be expected to (increase, decrease), accordingly. 1) increase; decrease 2) decrease; increase 3) decrease; decrease 4) increase; increase 5) Bond strength and atom masses have nothing to do with frequencies. 5. The United Nations predicts an increase due to anthropogenic industrial activity of thermal waste on the order of 5% over the new century. Thermal waste is another way of saying that not all the solar input is eventually reradiated away from the earth-atmosphere system. That is, over the next hundred years, the heat content of the earth-atmosphere system might increase by 5%. If that turns out to be true, then the ambient earth-atmosphere temperature might be expected to increase from the current value of 257K by about …. NOTE: The intensity of radiation goes directly as the heat content and the fourth power of the absolute temperature… to a reasonable approximation. 1 degree 2 degrees 3 degrees 4 degrees 5 degrees 6. Thinking about “lightbulb earth,” the effective radiative blackbody temperature of the mean earth-atmosphere system displays its characteristic lðmaxin the (longer, shorter) wavelength infrared, compared to the sun s solar output with its lðmax. in the (higher, lower) frequency visible. 1) longer; lower 2) longer, higher shorter; lower shorter; higher None of the above, since lðmax can only be recorded in wavenumbers. 7. Consider the N-to-N and C-to-C stretching frequencies in the F2N2 and N2C2 molecules (respectively) and select the best answer from the list below: 1) Both are infrared active 2) Neither is infrared active 3) F2N2 is but N2C2 is not 4) N2C2 is but F2N2 is not 5) They are degenerate modes QUESTIONS 8-10 ARE BASED ON THE DATA SUPPLIED IN THE FOLLOWING PHASE DIAGRAM FOR WATER. Note that the pressure and temperature scales are not continuous - the scales change. Note also Tc = 374°C and Pc = 218 atm.  8. The phase changes occurring from point A to 800 torr upon compression of H2O at constant temperature are progressively .... 1) solid to liquid to gas 2) gas to liquid to solid 3) gas to solid to liquid solid to liquid to solid liquid to solid to gas 9. The phase change on heating from point D to point E at constant pressure is… 1) liquid to gas 2) solid to liquid 3) solid to gas 4) liquid to solid 5) gas to liquid 10. Consider the ideal solution suggested by the segment FG and determine the number of moles of water present for each mole of solute: 1)1:1 2) 1:9 3) 9:1 4) 9:10 5) 10:9 11. Select the statement from among the following that is most nearly correct: 1) A sufficient reduction in temperature CAN bring about the condensation of any gas to the liquid state, regardless of the pressure (unless the pressure is unreasonably small). 2) A sufficient increase in pressure CANNOT bring about the condensation of any gas to the liquid state, regardless of the temperature. 3) As T approaches Tc, DðHvap approaches ZERO. 4) As T approaches Tc, surface tension approaches ZERO. 5) All of the above are essentially true. 12. The critical conditions for radon and carbon dioxide are, respectively, 104°C and 62 atm, and 31.1°C and 73 atm. Therefore, at 31.1°C and 73 atm.... 1) only radon can be liquified. 2) only carbon dioxide can be liquified. 3) radon and carbon dioxide can both be liquified. 4) neither radon nor carbon dioxide can be liquified. 5) Radon is a permanent gas and carbon dioxide only exists in the solid state (as dry ice) 13. Assuming ideal behavior, what is the vapor pressure of a solution of 16.0 mol of toluene and 4.00 mol of benzene at 20 °C? Vapor Pressures at 20 °C benzene 75.0 torr toluene 22.0 torr 1) 32.6 torr 2) 61.8 torr 3) 64.4 torr 4) 87.6 torr 5) 97.0. torr 14. One of the most interesting and (arguably, perhaps) useful applications of polyacrylic acid (sodium salt) is the “super slurper” absorbent material that is the active ingredient in disposable diapers. Chemistry (of the absorbing molecules) and physics (of osmosis) at work in the benefit of humankind. When 4.0 g of the polyacrylic acid polymer are dissolved in 1 L of dioxane, the osmotic pressure at 25°C is 0.494 torr. Therefore the molecular weight of the polymer must be..... NOTE: Remember that R = 0.08205 L·atm mol-1 deg-1 1) 2.65 X 10-5 g/mol 2) 4.53 X 101 g/mol 3) 1.81 X 102 g/mol 4) 1.98 X 102 g/mol 5) 1.50 X 105 g/mol 15. This device, an inverted "thistle tube” across which a semipermeable membrane has been stretched, can be used to measure osmotic pressure. It is initially filled with fresh water and set in a beaker containing a saturated salt solution so that the height of the liquid stands a distance h above the surface level of the surrounding solution. At equilibrium......  1) h will be greater than the initial value. 2) h will be the same as the initial value. 3) h will be zero. 4) h will be less than the initial value. 16. Which of the equations below are accurate representations of Raoult’s Law? 1) p = p°X2 2) (p° - p)/p° = X2 3) DðT = K(g2/M2g1)1000 4) only 2 and 3 5) only 2 17. The substance which has the highest boiling point is....... 1) CH4 2) CO2 3) HF 4) Cl2 5) N2 18. A pure substance, above its melting point, is in a high pressure cylinder. Upon opening a valve on the cylinder a gas escapes. A pressure gauge on the cylinder shows a pressure of 56.5 atm. at 20 °C before opening the valve. After removing 10 ft3 of the gas, measured at standard conditions, the pressure in the cylinder …. still reads 56.5 atm at 20 °C. The pressure gauge is in good working order. Why should you not be surprised by this observation? 1) Because cylinder and contents will weigh the same before and after opening the valve. 2) Because the substance in the cylinder is in the gaseous state. 3) Because the substance in the cylinder is a liquid under its own vapor pressure. 4) Because the substance in the cylinder is probably carbon dioxide. 5) Because the substance in the cylinder is probably not carbon dioxide. 19. The mole fraction of water in 200. g of 95% (by mass) ethanol, C2H5OH, is..... 1) 0.050 2) 0.12 3) 0.56 4) 0.88 5) 1.00 20. A cellophane bag, which acts as a membrane permeable only to water, contains a 2 M sugar solution. When immersed in a 1 M sugar solution...... 1) the bag will soon contain more solution that will be more concentrated than 2 M. 2) the bag will soon contain more solution that will be less concentrated than 2 M. 3) the bag will soon contain less sugar and the solution in it will become less concentrated. 4) the bag will soon contain less water and the solution in it will become more concentrated. 5) there will be no change…. anytime soon. 21. The likely formula for a completely ionized salt if an aqueous 0.10 M solution of that salt has a freezing point of –0.74 °C is........ NOTE: Kf for water = -1.86 °C·m-1 1) MX 2) M2X 3) M2X3 4) MX3 5) MX2 22. A 2.00-g sample of a non-electrolyte is dissolved in 100 g H2O. If the resulting solution freezes at –0.186 °C, then the molar mass of the compound must be…. NOTE: Kf for water = -1.86 °C·m-1 1) 18 18.6 20.0 186 200 23. A proposed method for desalinating sea water is to submerge a long tube, its bottom closed by a semipermeable membrane, to a depth such that the hydrostatic pressure overbalances the osmotic pressure and forces pure water through the membrane. If seawater is an 0.50 M aqueous solution of NaCl at 17°C, then the pressure at which this process will begin must be… NOTE: R = 0.08205 L·atm mol-1 deg-1 1) 1.4 atm 2) 6.0 atm 3) 12 atm 4) 24 atm 5) 48 atm 24. The dunking bird is a most popular toy. As long as it keeps getting its head wet, it continues to bob up and down. What makes it go? 1) Osmotic pressure 2) Hydrostatic pressure 3) Vapor pressure 4) Atmospheric pressure 5) Peer group pressure 25. With respect to the temperature-dependence of viscosity and surface tension, it would be most correct to say…. 1) Neither is. 2) Only viscosity is. 3) Only surface tension is. 4) Both are. 26. A prune… that’s a (politically correct) dried plum…. a cucumber, and a raw egg from which the shell has been carefully removed, leaving the membrane in tact, are placed in the same salt solution, in separate beakers. The prune swelled, the cucumber shriveled, and not much seemed to happen to the egg. On that basis, you might best conclude the relative concentration of the solutions that constitute the cellular fluids of these common food items is in the order...... 1) prune < cucumber < egg 2) prune < egg < cucumber 3) egg < prune < cucumber 4) egg < cucumber < prune 5) cucumber < egg < prune 27. 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!"#$%&'()*+,-./0123456789:;<=>?YÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿÿEFGHIJKLMNOPQRSTUVWXYZ[\]^_`abcdefghijklmnopqrstuvwxyz{|}~€ì¥Ás ¿48jbjbÀ À ŠªkªkK1ÿÿÿÿÿÿ]¸¸¸¸¸¸°„t t t 8¬ ,Ø l4 ç6Z˜œ²²²²²²Â2Ä2Ä2Ä2Ä2Ä2Ä2,A8ô5:Lð2÷¸²²²²²ð2 ¸¸²²h0   ²˜¸²¸²Â2Ìr>r¸¸¸¸²Â2 � š1”¸¸Â2D$hÕ’¸4 @t JÀ–2,Printed Last Name: |___|___|___|___|___|___|___|___|___|___|___|___| Printed First Name: |___|___|___|___|___|___|___|___|___|___|___|___| Social Security # |___|___|___| |___|___| |___|___|___| School: |___|Barnard |___|College |___|Engineering |___|General Studies Chemistry 1404y Exam 1 February 18, 2002 Instructions Fill in your name and CUID number as indicated above. On the bubble sheet: 1) On Side 2 of the Bubble Sheet print your first and last name in the box provided. 2) Then fill in the Identification No. in the space provided and as indicated. Your Identification No. is your Social Security Number. 3) Using a soft lead pencil, blacken the one response that best answers the question or completes the statement. There is only one correct answer to each question. Any question with more than one answer will not be counted. Your score will be the total number of correct answers; therefore, it is to your advantage to answer every question. 4) There are 27 questions. They are equally weighted. Under no circumstances are you to make any other marks... anywhere on the bubble sheet... except in the appropriate bubbles for marking an answer you believe to be correct. You may write on the exam sheets themselves for the purpose of doing calculations.... but do not write on the bubble sheet. A periodic table of the elements can be found on page10 of this exam. A SCRATCH SHEET is provided on PAGE 11. Check the front blackboard for time remaining, last-minute corrections and additional information. You will have 75 minutes to complete the exam. When you have finished the exam or at the end of the allowed time, deposit your exam questions and bubble sheets in the separate boxes provided at the front of the room. Do not forget! Print your first and last names in the box provided (1) on the bubble sheet, and (2) on the front page of the 11 pages of this exam. Remember! It is your responsibility to ensure that your bubble sheet and exam sheets are properly identified. 1. Nearly monochromatic light waves are produced by... 1) the Sun 2) an incandescent light filament 3) a red hot charcoal briquet 4) a laser pointer 5) a bunsen burner 2. The following graph shows the annual variation in atmospheric carbon dioxide concentration as recorded at the Mauna Loa observatory (Hawaii). To reduce this steady increase in atmospheric carbon dioxide (and its apparent contributions to global warming), it would be LEAST effective to limit …. 1. use of natural gas as fuel rather than coal or petroleum. 2. use of nuclear or solar energy instead of fossil fuels for electricity generation. 3. use of automobiles. 4. production of beef. 5. rates of deforestation.  3. Of the following molecules, the one(s) exhibiting NO C-to-C multiple bond infrared stretching frequencies is (are)….. a) H2C=CH2 ethene (ethylene) b) HC=CH ethyne (acetylene) c) CH3HC=CH2 propene (propylene) d) CH3C=CH propyne (methyl acetylene) 1) (a) and( c) 2) (b) and (d) 3) (a) a4†4‡4–4¬4È4Ý4Þ4¹6º6Ô6î67"7<7=7>7É7Ê7Ô7Ü7â7è7î7ï7ñ7ööññññöïöööööñññêêêææææÞÞ„0ý ÆÐ„0ý ÆÐ1$„0ý 1$„0ý ÆÐñ7888"8$8%8182838480†È‡(ˆöòíëéçåççëÝØë ÆÐ„0ý ÆÐ$„0ý„0ý $„0ý ÆÐ "8#8&8'8-8.8/808480†¬†’‡È‡$ˆ&ˆ(ˆýöýöñöïïñ5�0JmH j0JU0J°Ð/ °à=!°"°#� $� %°can only NOTE: Subscript 1 denotes solvent; subscript 2 denotes solute. that 1) n viscosity nor surface tension temperature-dependent2) o temperature-dependent3) o temperature-dependent4) b temperature-dependent 5) one thing has nothing to