Chemistry 11 Exam I October 12, 2006 Solutions

NAME: ________SOLUTIONS Exam I October 12, 2006 Good evening! While everyone is getting their exams and as you get settled, it might be a good idea for you to work on relaxing. Know that you can do your best work when you believe you can. I know you have studied hard to get to tonight, and I am really interested to see how you do with these questions. I am not just looking for the right answer, but a thought and thought process that leads you to that answer. NEVER EVER LEAVE A QUESTION BLANK This exam contains four questions on the exam, I, II, III, and IV on 11 pages. You should divide your time evenly between the four questions. That means, for the first time through the exam, don’t take more than 30 minutes per Roman numeral. Formula sheet and periodic table are on the back, you may tear off the back sheet and have it available for ready reference. Use average atomic weights to four decimal points as provided in that table. When we start the exam, I will ask you to put all your books, notes, peripherals away. You should have a calculator and an assortment of pens and pencils. Write ONLY on the white spaces underneath the questions unless otherwise instructed to do so. Extra credit (2 points) What substance was the focus of research by father and son Arthur and Roger Kornberg over the past 50 years. Arthur won a Nobel in Physiology or Medicine for his work on the basic chemistry of this structure in 1955 and Roger was awarded the Nobel Prize in Chemistry announced just last week for his work on its more complex structures. a) cholesterol b) estrogen c) testosterone d) RNA Chemistry 11 Exam I I. Fall 2006 Stoichiometry, Mass Relationships, (25 points) Last Monday, the 2006 Nobel Prize in Selection Committee announced that the Nobel Prize in Chemistry (and $1.3 million dollars) was awarded to Roger Kornberg of Stanford University. The biological material Dr. Kornberg worked with is in fact a family of compounds under one general heading. The questions below refer to one member of that family. 1. The purified substance is found to contain four elements: carbon, nitrogen, oxygen, and hydrogen. Combustion of a 4.2456 mg sample of this material produces 6.5968 mg of carbon dioxide and 1.3498 mg of water. By another method, the substance was determined to contain 24.726 % by mass nitrogen. What is the empirical formula of the compound? C2H2NO compound is related to the RNA base guanosine 2. The average molar mass for this compound 283.24 g/mole. What is the molecular formula? 5 x empirical formula: C10H10N5O5 3. Many people believe that consumption of this compound provides health benefits. It is possible to buy either a bottle of one hundred 500.0 mg capsules 5.000% (by mass) or a bottle containing 250.00 mL of 24.00 mM (1 mM = 0.001 M). The two bottles are the same price. Which formulation is the better buy (i.e. which bottle contains more moles of compound?) 0.05 x .500g x 100 /283.24 g/mole = 0.008824 moles 0.02400 x .250 = 0.006 moles Capsules are a slightly better deal 4. Mass spectrum. This compound is not easily monitored in the mass spec because it tends to fall apart. One piece of it is however quite stable, and resists fragmentation. The mass spec of the stable fragment is shown below. 2 Chemistry 11 Exam I Fall 2006 a. The x axis is labeled m/z. Define z and explain why it is important in the detection of a molecular ion or fragment in the mass spectrometer. Z is the charge on the ion, which needs to be charged in order to be deflected in the mass spectrometer b. Assuming a z of +1, what is the approximate molar mass of this stable fragment? 152amu c. If this molecular ion or fragment contained chlorine, and knowing that the two isotopes of chlorine are 35Cl 75.77% and 37Cl 24.23%, what would you have seen in the mass spectrum? (use back of page3 to explain)two peaks separated by 2 amu with 3/1 heights 3 Chemistry 11 Exam I Fall 2006 Balancing Equations, Redox, Acid/Base (25 points) 1. A potent sterilizing solution poured on open wounds is a solution of potassium permanganate and hydrogen peroxide. These two materials will react in acidic solution according to the following equation (ions such as potassium are not written here AND since this is in acidic solution, H+ and H2O are not added here buy you may add them as you need to answer questions below): UNBALANCED EQUATION [MnO4]-1 + H2O2 Æ Mn+2 + O2 a. Write down the oxidation states of all of the atoms on both sides of the equation. Mn+7O-2 + H+1 O-1 Æ Mn+2 + O2o b. Identify first, the substance being oxidized, the number of electrons produced in that half reaction, and the number of product H+ needed to balance this half of the reaction. Put all of this together to write a balanced half reaction for the oxidation reaction. H2O-12 Æ O2 + 2e- + 2H+ c. Next, identify the substance being reduced, the number of electrons needed as a reactant in that half reaction, the number of product water molecules necessary to mass balance the extra oxygen, and the number of reactant H+ necessary to balance this reaction. Put all of this together to write a balanced half reaction for the reduction reaction. 8 H+ + [MnO4]-1 + 5 e- Æ Mn+2 + 4H2O d. Finally, write a net balanced equation for the reaction. 5x[H2O-12 Æ O2 + 2e- + 2H+] 2x[8 H+ + [MnO4]-1 + 5 e- Æ Mn+2 + 4H2O] _____________________________________________ 2 [MnO4]-1 + 5 H202 + 6 H+ Æ 2 Mn +2 + 5 O2 + 8 H2O 4 Chemistry 11 Exam I Fall 2006 First rewrite above the balanced equation from the previous page (if you did not manage to balance this equation assume the ratio of permanganate ion to peroxide is 1:2 (note this is NOT the correct mole ratio): 2 [MnO4]-1 + 5 H202 + 6 H+ Æ 2 Mn +2 + 5 O2 + 8 H2O 2. Limiting Reagent: If 5.268 g of KMnO4 is dissolved in an acidified solution of exactly 100 mL 30.00 % hydrogen peroxide (assume 1.000 g/mL) identify the limiting reagent, predict the masses of products formed in acid solution and the mass of left over reactant. (Assume here that you have plenty of acid in the solution so that the acid is NOT the limiting reagent) 1. Identify Limiting Reagent: KMnO4: 5.268 g /Molar Mass 158.04 g/mol = 0.03333 moles H2O2: 30.00 g/34.00 g/mole= 0.8824 moles MnO4/H2O2 = 2/5 = 0.4000 ideally 0.03333/0.8824 < 0.4 so MnO4 is limiting, H2O2 is excess 2. Calculate Mass Products and left over reactants Product Mn2+ is 0.03333 x 54.938 = 1.8311 g Mn Product O2 is 0.03333(5/2) x 32.000 = 2.6663 g O2 Left Over H2O2 [0.8824 moles – 0.03333(5/2) moles] x 34.016 = 27.169 g left over 3. The reaction above proceeds with the consumption of three moles of acid for every mole of KMnO4. If the initial pH of the 100.0 mL of acidified peroxide is 0.0000, , predict the final pH (Assume the final volume is 101.8 mL). [H+ = 1.000 M in 100.0 ml is 0.1000 moles KMnO4 sucked up 0.099999 moles acid, 0.1000 – 0.0999 = 0.0001 moles [H] = 0.0001 moles/.1018L = M pH = -log [H+] = 3.008 (could have been up to pH 7 depending on how many sig figs you were working with. All were accepted. 5 Chemistry 11 Exam I Fall 2006 Empirical Gas Laws (25 points) You may be somewhat sad to learn that some scientists believe fall foliage may be harmful to your health. That's the focus of studies being done at the National Center for Atmospheric Research in Colorado. Dr. Alex Guenther is an atmospheric chemist at the National Center for Atmospheric Research, and he studies the effects of vegetation and fall foliage on air quality and climate. The emissions of these chemicals play a role in producing ozone and smog. The emissions from the plants are called “volatile organic compounds” or VOC’s. 1. Dr. Guenther’s graduate student purified a sample of VOC from the air above the forest canopy (the air above the top of the trees). This purified VOCs has a density of 3.0406 g/L at STP. What is the molar mass? Molar Mass of VOC is 68.11 g/mole (isoprene) 2. She determined the density of the original air mixture (molecular nitrogen, molecular oxygen and the VOC) collected at a pressure of 0.9856 atm and 17.82oC to be 29.01 g/mole, determine the “apparent molar mass” of the gas mixture of air above the forest canopy. Apparent Molar Mass of mixture is 29.02 g/mole 3. Assume that the air just above the tops of the trees is composed of nitrogen, oxygen, and a single type of VOC with a molar mass calculated above . The nitrogen and oxygen in the air will retain the mole ratio of 2.89/1 seen in normal air. Determine the mole fraction of the contaminating VOC. Mole fraction of VOC is between 0.002 -0.003 depending on how many sig figs you chose to keep working with. Mole fraction of O2 is 0.2566 Mole fraction of N2 is 0.7416 6 Chemistry 11 Exam I Fall 2006 Calculate the partial pressures of each of the gases. PVOC = 0.002 atm PO2 = 0.253 atm PN2 = 0.731 atom 4. If diffusion of these three gases is related to the effusion predicted from Graham’s Law, predict the relative rate of diffusion for oxygen, nitrogen, and this VOC. N2/O2 = 1.068 VOC/O2 = 0.685 7 Chemistry 11 Exam I Fall 2006 Kinetic Molecular Theory of Gases (25 points) 1. Calculate the urms for the Nitrogen, Oxygen, and the VOC components of the gas mixture in problem III at 17.82oC. (If you could not calculate a molar mass for this gas, assume 68.11 g/mole.) VOC: 326.3 m/s N2: 509.0 m/s O2: 476.2 m/s 2. Sketch the Boltzmann distribution for the three component gas mixture above. Remember to label your axes and provide as much information as possible. nitrogen Number of atoms oxygen voc Velocity m/s 8 Chemistry 11 Exam I Fall 2006 3. As night falls in the forest, the temperature drops. Describe qualitatively what happens to the velocity distributions of the three gases in this mixture as night falls? As the temperature drops, the rms velocity decreases and the distributions narrow, causing the entire graph on the previous page to shift to the left and narrow. 4. As sun rises the next day, the temperature rises and more VOC escapes from the trees and joins the mixture of gases above the forest canopy. What prevents this mixture of gases (and any mixture of gas) to separate out into layers of different gas densities with the heaviest gas on the bottom? The diffusion and the constant random motion of the particles cause the gases to totally mix despite the differences in their masses. 9 Chemistry 11 Exam I Fall 2006 Assorted Equations, Constants, and Conversion Factors pH: pH = –log[H+] Ideal gas law: PV = nRT Dalton’s law: Ptotal = ∑ Pi i Mole fraction: χa = na/ntotal = Pa /Ptotal Force of collision: F= Average kinetic energy: KE = Most probable speed: ump = 2RT M Average speed: uavg = 8RT πM Root mean square speed: urms = 3RT M Maxwell-Boltzmann distribution: ⎛ mi ⎞ 2 − mi u 2 ⎟⎟ u e f(u) = 4π ⎜⎜ ⎝ 2π k BT ⎠ Graham’s law of effusion: Rate of effusion of gas 1 = Rate of effusion of gas 2 Mean free path: λ= Δmu Δt 3 2 RT = 1 2 M u2 32 2 k BT M2 M1 1 2 (N V )(πd 2 ) Collision rate with container wall (collisions per second): ZA = 1N 8RT A 4V πM Collision rate between gas particles (collisions per second): Z=4 N 2 πRT d M V Van der Waals equation: ⎡ ⎛ n ⎞2 ⎤ ⎢Pobs + a ⎜ ⎟ ⎥(V – nb) = nRT ⎝V ⎠ ⎦ ⎣ NA = 6.022 × 1023 mol–1 R = 8.3145 J mol–1 K–1 = 0.08206 L atm mol–1 K–1 1 atm = 760 torr = 1.01325 × 105 Pa 1 L = 1000 mL = 1000 cm3 T(K) = t(°C) + 273.15 me = 9.10939 × 10–31 kg 1 nm = 10-9 m 1 Pa = 1 kg m–1 s–2 1 J = 1 kg m2 s-2 STP ≡ 1.000 atm, 273.15 K 10 Chemistry 11 Exam I Fall 2006 http://chemlab.pc.maricopa.edu/periodic/printable.gif Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Bohrium Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curium Dubnium Dysprosium Einsteinium Ac Al Am Sb Ar As At Ba Bk Be Bi Bh B Br Cd Ca Cf C Ce Cs Cl Cr Co Cu Cm Db Dy Es Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Hassium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanum Lawrencium Lead Lithium Lutetium Magnesium Manganese Meitnerium Mendelevium Er Eu Fm F Fr Gd Ga Ge Au Hf Hs He Ho H In I Ir Fe Kr La Lr Pb Li Lu Mg Mn Mt Md Mercury Molybdenum Neodymium Neon Neptunium Nickel Niobium Nitrogen Nobelium Osmium Oxygen Palladium Phosphorus Platinum Plutonium Polonium Potassium Praesodymium Promethium Protactinium Radium Radon Rhenium Rhodium Rubidium Ruthenium Rutherfordium Samarium Hg Mo Nd Ne Np Ni Nb N No Os O Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Rf Sm Scandium Seaborgium Selenium Silicon Silver Sodium Strontium Sulfur Tantalum Technetium Tellurium Terbium Thallium Thorium Thulium Tin Titanium Tungsten Uranium Vanadium Xenon Ytterbium Yttrium Zinc Zirconium Sc Sg Se Si Ag Na Sr S Ta Tc Te Tb Tl Th Tm Sn Ti W U V Xe Yb Y Zn Zr 11 Chemistry 11 Exam I Fall 2006 12