[Bush] Chemistry Exam #3 - Fall 2006

[Bush] Chemistry Exam #3 - Fall 2006 - NAME 1 Chemistry...

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Unformatted text preview: NAME 1 Chemistry 1301 Fall 2006 Exam #3 PLEASE READ THESE INSTRUCTIONS CAREFULLY BEFORE BEGINNING THIS EXAMINATION. Select the best response to each question. There is only one best response to each question unless otherwise indicated in the question. There are 30 questions on this examination worth 3.33 points each. (Total of 100 points.) Check your test booklet to be sure that you have a complete exam with all 30 questions. Write your NAME and TEST NUMBER on your Scantron. Write your name on the first page of the test booklet also. Work each problem carefully on the test booklet or on the scratch paper provided. Then select the answer, which you feel is the best response. If none of the choices is close to your calculated answer, or if none is correct, then select the response "none of the above." ALL ANSWERS MUST APPEAR ON THE SCANTRON. Your grade will be determined only by what appears on the Scantron, not by work on the test booklet. Look over your exam and work the easiest problems first, saving the more difficult ones for last. Be sure that you have correctly indicated your final choices on the Scantron before turning in your paper. If a question is incorrectly marked on the Scantron, it will be counted wrong even if it was correctly marked on the test booklet. If you have any questions about any of the problems on this exam, it is your responsibility to ask for a clarification from the instructor during the examination. For questions #1 and #2, consider three l—L flasks at STP. Flask A contains NH3 gas, flask B contains N02 gas, and flask C contains N2 gas. Assume the gases all behave ideally. 1. Which flask contains the largest number of molecules? a) flask A with NH3 gas almafiua ScurNLT b) flask B with N02 gas CymgLT>Vauw+€£écuvarnummbaxxi c) flask C with N2 gas amdngQb. AVOSQLCYO'S Lab.) (:9 all have the same number of molecules e) cannot predict with the information provided 2. In which flask do the molecules have the highest average velocity? ', E§y*Luficx“L flask A with NH3 gas ‘ . \ cnmieascoma b) flask B with No2 gas CQLL \um’ngmmgtm . " .L 2. c) flask C With N2 gas Elem: 2mv Vzd—L d) all have the same average velocity n“ e) cannot predict with the information provided 2 3. Use the ideal gas law to predict the relationship between H and T if ressure P and volume V are held constant. n = k/T ‘iflfl' :: 9U P _ cgnatlméz c) n=kP/V 7“ Ti? tongue )‘MRM d) n = kR b ‘ e) n = k/R hr: ‘nmufichwk‘p . I 4m don’t mm Tables: Jaocsrhm 4. A 6.35—L sample of carbon monoxide is collected at 55°C and 0.892 atm. What volume will the gas occupy at 1.05 atm and 20°C? 1 96 ’PLLI‘ :?°—V2 n‘: n1 MTMLSF‘OL‘“ a) . L “‘7'! ‘ 1T2- b) 5.46 L ?! KQ’W‘Y‘ c 4.82L V2“3§(‘,_7’ ‘J, d) 6 10 L P9” T: . 5 '1 . ~ ‘ L e) none of the above “ o'gciz “gig—$2 65$L>h482 \.Ck§cxkr\ SE;+JZI5 5. Which conditions of P and T, respectively, are most likely to produce an ideal gas? Fm mm m 4&1 @mV‘Q—kow?) \Mgh mag .50 \AWISXCQA MM so Gem ‘ OMS“? a) high P, high T b) low P, low T, c) high P, low T dd ) low P, high T e) any of these 6. It is found that 251 mL of gas at STP has a mass of 1.00 g. What is the molar mass of the gas? m2 mcuwetsampb 7@ 89.3 g/mol W: NET-- __m_(2,T : mfiaivnau/J b) 28.0 g/mol M . c) 14.0 g/mol M: £1: \.%(OW)(1B‘< d) 22.4 g/mol P" \Amol \aJUhQZSIL e) none of the above H: 8°13; m0! 7. A 250-mL flask is filled with oxygen that was collected 3 over water at 760 torr and 14 °C. If the vapor pressure of water at 14 °C is 12.0 torr, what is the partial pressure of oxygen in the flask? Q 748 torr p 3 13,420+ 02 2 7(90 few b) 760 torr c) 728 torr ?oz=<760- lZ.O>"DN a 748W d) 772 torr e) none of the above 8. What volume of oxygen gas will react with 30.0 L of sulfur dioxide if both gases are at 1.0 atm and 100.°C? 2502(9) + 02(9) —’ 2503(9) a) 3.75 L of 02 Sma’cee gmm wfiumTMV, b) 30.0 L of 02 Wmebcwwgfly c) 7.50 L of 02 (CxWVLuDSSGLS 1531033 ® 15.0 L of 02 ) none of the above 30.0L392(‘ L'O" : 'S'0 L 02— oc meow.wa 2L3) 9 prcb‘lom WAS W: NLTA QQS‘b\dALL¥MQ-Mg A sample of oxygen gas (32.0 g/mole) was found to effuse at a rate that was equal to two times that of an unknown gas. The molecular weight of the unknown gas should be about g/mol. a) 64 dun X @128 Taco;— 3 %_: t: 2 520 [mo] 0‘) 15 Sod“ 36.0, e) none of the above = 7‘ 60 7c 3 0325 lmo) 10. 11. The van der Waal's equation, 4 P + Big-(V — nb) = nRT v2 attempts to describe the behavior of "real" gases. This equation correctly describes gas behavior over a wider range of temperature and pressure than the "Ideal" Gas Equation because the van der Waal's equation incorporates two corrections to the ideal gas law. What is the purpose of the constant a? a) to correct for chemical reactions between gas molecules. b) to correct for the random motion of gas molecules C) to correct for the finite volume of gas molecules d) to correct for the average kinetic energy of gas molecules as a function of absolute temperature 6;» to correct for the intermolecular forces of attraction between gas molecules. a.p5 «\fim.pnanouua4ewnfi Which one of the following is not part of the kinetic— molecular theory? a) Attractive and repulsive forces between gas particles are negligible. b) Gases are made up of atoms and molecules. c) Gas particles are in continuous, random motion. Atoms are neither created nor destroyed by chemical mLch nO’V wisdomd. e) Collisions between gas particles do not result in a net reactions. change of energy. Te. Vacwh‘dD/J guano“- cwbomschvo szé melanoma/m .QJCQQP" Mini cotgmwm. 12. A state function is 5 a) a mathematical function that depends on the force times the distance. a mathematical function whose value depends only on the final and initial states of the systenn ti3=-Ugg,n"Lmeah& c) a mathematical function whose value depends on the precise manner in which a given process is conducted. d) a mathematical function whose value is always zero for processes conducted at constant pressure. e) none of the above. 13. Enthalpy is the heat associated with a process conducted at constant pressure. AH; (59 b) the heat associated with a process conducted at constant volume. c) the work associated with a process conducted at constant pressure. d) the work associated with expanding the system at constant pressure. e) none of the above. 14. Internal Energy, AU, is £91.: fis\/ a) the heat associated with a process conducted at constant pressure. the heat associated with a process conducted at constant volume. c) the work associated with a process conducted at constant pressure. d) the total energy associated with expanding the system at constant pressure. e) none of the above. 15. In mathematical form, the first law of thermodynamics is 6 a) AU = q/w b) AU = g X w c) AU = -PAV d) AU = (l/2)Inv2 q+W @ 16. Work is Lema‘b Job force times distance b) force per unit volume c) mass times acceleration d) mass times velocity e) none of the above 17. Iron metal reacts with oxygen gas to form 1.000 mole of solid Fe203 according to the following reaction, 2Fe(s) + 3/2 02(g) —9 Fe203(s) AHO = —824.0 kJ How much heat energy would be involved when 2.000 moles of solid Fe203 are produced by this reaction? a) —412.0 kJ b) +1648 kJ QC—gzqfioklb: .. @48ka c) +824.0 kJ d) —824.0 kJ <25>none of the above WMWQ r 18. Some beetles defend themselves b s ra in hot uinone 7 ypygzq l9. (C6H402) at their attackers. The beetles make quinone in a special chamber in their abdomen according to the following equation. C6H4(OH)2(1) + H202(1) ‘9 C6H402(l) + 2H20(l) WHQSS’S Law) Calculate AHO for this reaction given the following information. C6H4(OH)2(l) ’9 C5H402(l) + H2(g) AHO = +177.4 kJ H2(9) + O2(9) ‘9 H202(1) AHO = —187.8 kJ 2H2(g) + 02(g) “> 2H20(l) AHO = —-57l.6 kJ 19 AH a) +79.4 kJ CEHALOHBLV» CbHQOZ+Vé “TH-LG b) —296.2 kJ H201 _; (Wng «407.66 c) ——582 kJ gha+§9§ -—) 1H "'57wa @ ——206.4 kJ Ceramygzt H2029 CbH+OL+ZHzO e) none of the above 0 Is“: 40ng )o If 20 kJ of heat energy flow ingg a system and the surroundings QW1L do 15 kJ of work on the system, which of the following uo>0 statements is true? Au: +u:> a) AU = —35 kJ is —. 3 Hsz3 b) AU = —5 kJ “ 10h_ 2 3S led @AU = +35 kJ d) AU = +5 kJ e) none of the above 20. 21. Assuming one atmosphere pressure and a temperature of 8 25°C, the equation that corresponds to the standard molar enthalpy of formation of ethyl alcohol, C2H5OH(1), is a) C2He(g) + 1/2 02(9) —> C2H50H<l) (\md Wéasm “A +m3kcwc£cnu§ «StitUa b) 2C2H6(9’) + 02(9) —> 2C2H50H(l) @2C(s) + 3H2(g) + 1/2 02(g) —> C2H5OH(1) d) 20m + 6H(g) + 0(g) —> C2H50H(1> 9) C2H6(9) + 0(g) a C2H50H(l) Concrete hardens according to the following reaction, CaO(s) + H20(1) —> Ca(OH)2(s) Use the enthalpy of formation data given below to calculate AH° for the setting of concrete. a) AH° = b) AH" = c) AH° = Species Ali—of kJ/mOl H2003) "242 Hzom —286 Ca0(s) -635 Ca(OH)2(S) -987 - —1980 kJ Aggy-.mamzfiwjgm WCQE%D3 —638 kJ “‘0‘ m —352 kJ ——66 kJ -— \mm (LC) “9331?; e) none of the above 7- -9Q,\Q;S 22. How much heat, in kJ, is required to raise the 9 temperature of 125 g H5) from 24.3°C to64.9°C? The specific heat of water is 4.18 J / (g°C). 21.2 kJ 58); CAT: 4—.I83' ‘29prqu -24—5 42.4 kJ c) 33.9 kJ 105% d) 523 kJ e) none of the above 3‘ 219.:H'3 0“ mim— 23. The heat capacity of a bomb calorimeter is found to be 5.68 kJ/°C. When a 1.652 g sample of glucose, C6Hn06, (180.2 g/mol) is burned in the calorimeter, the temperature of the calorimeter increases from 24.56°C to 29.10°C. Calculate AU per mole of glucose from the combustion reaction: condo os’hux micng .onkamLc. C6H1206 (s) + 6 02 (g) 9 6 002 (g) + 6 H20 (9) a) 15.6 kJ/mol of glucose b) —42.6 kJ/mol of glucose 6cm, Shah; 2q.\O-2‘V.Sb:e’> @ —2.81 x 103 kJ/mol of glucose 7‘ d) —25.8 kJ/mol of glucose «i. $.18? be; 3 .. ,C ‘ XV\ e) none of the above t' 25 5 8”“: ‘25‘1" *5 30.2%; -a.8mo ("33‘ 'IQSZ m0! 24. Which one of the following types of e ectromagnetic radiation has the highest energy? ‘5’ x—rays )%“&%P>N1Haxduyzk)ifiéfik9)\ngnflmmg> “VLUDUUZW£% b) infrared rays 0) ultraviolet rays d) microwaves e) visible light 25. What is the relationship between wavelength A, frequency 10 v,and the velocity of light c? a) c = X/v = NJ=£12 C:) c NV 5’__ UQLCBEE> c) c = v/k d) c = v + A e) c = v — X 26. The scientist who studied blackbody radiation and first proposed that light emitted from hot objects is quantized was a) Louis de Broglie b) Niels Bohr c) Albert Einstein d) Werner Heisenberg (i) Max Planck 27. Experimental evidence for the wave properties of electrons is based on a) the equations describing the Bohr atom. b) the photoelectric effect. gm Ma 00w QnQd— (:3 studying electrons diffracted from metal surfaces. d) studying the scattering of alpha particles by metal foils. e) the existence of cathode “rays.” 28. A "light particle” is called a a) node b) quark c) beta—particle @ photon e) neutrino 29. The scientist who proposed that is it not possible to 11 know the exact position and energy of an electron at the same time was a) Niels Bohr @ Werner Heisenberg c) Max Planck d) Johannes Rydberg e) Johann Balmer 30. According to the experiments concerned with the photoelectric effect, what was the result of increasing the frequency of the light striking the metal surface? a The number of electrons emitted was increased. b) The energy of the electrons emitted was increased. c) Both the number and energy of the electrons was increased. d) Both the number and energy of the electrons was decreased. e) There was no change in the number or energy of the electrons. ...
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[Bush] Chemistry Exam #3 - Fall 2006 - NAME 1 Chemistry...

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