CHEM 108 (Spring-2008) Exam. 1 (105 pts)

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1 CHEM 108 (Spring-2008) Exam. 1 (105 pts) Name: , CLID # LAST NAME, First (Circle the alphabet segment of your LAST NAME): A-D E-J K-N O-Z Please answer the following questions: Part I: Multiple Choices (60 pts: 4 pts each). Circle the ONE best answer: 1. Which statement is incorrect regarding the solubility of gases in liquids? a) Henry s law states that C = kp. b) The solubility of a gas increases as the pressure increases. c) Increasing of the solution leads to decreasing solubility. d) The Henry s law constant, k is the same for different gases and liquids. 2. Which of the following solutions has the highest boiling point? a) 1.0 m glucose in water b) 1.0 m NaCl in water c) 1.0 m KNO 3 in water d) 1.0 m CaCl 2 in water 3. What is the osmotic pressure, in atm, produced by a 20.0% glucose (C 6 H 12 O 6, molar mass = 180 g/mol) solution (d = 1.08 g/ml) separated from pure water at 25 ºC? a) 36.7 b) 30.6 c) 29.3 d) Suppose that at some point in the reaction: A + 3 B 2 C + 2 D [B] = M, and that min later [B] = M. What is the average rate of the reaction during this time period, expressed in M/s? a) 1.01 x 10-5 M/s b) 6.06 x 10-4 M/s c) 3.03 x 10-5 M/s d) 4.20 x 10-4 M/s 5. A reaction follows the rate law, Rate = k[a] 2. To demonstrate the second order behavior of the reaction and determining the rate constant, the graphical plot of the quantity on the Y-axis vs. time (t) produced a straight line. What was the quantity that plotted on the y-axis? a) ln [A] b) [A] c) 1/[A] d) 1/ln [A] 6. If aqueous solution A is 0.15 M sucrose (C 12 H 22 O 11 ) and solution B has 5.15 g urea CO(NH 2 ) 2 in 75 ml of H 2 O and the two solutions are separating from each other by semipermiable membrane. Will the net flow of water through the semipermiable membrane to be a) from A to B b) from B to A c) no flow d) additional information is needed 1

2 7. Which of the following physical properties does not generally increase with increasing the strength of intermolecular forces? a) Boiling point b) P vap c) surface tension d) H vap 8. What is the minimum mass of glycerol, C 3 H 8 O 3, that must be dissolved in 100. g H 2 O to prevent the solution from freezing at -15 o C? a) 74 g b) 66 g c) 7.4 g d) Which would have the lowest freezing point? a) Cl 2 b) N 2 c) SO 2 d) CH 3 OH 10. Ethanol has a vapor pressure of 100 mm Hg at 34.9 o C. Taking its heat of vaporization to be 39.3 kj/mol. What is its vapor pressure at 63.5 o C? a) 106 b) 369 mmhg c) 258 d) no answer was given 11. What is the osmotic pressure, in atm, produced by a 18.0% glucose (C 6 H 12 O 6, molar mass = 180 g/mol) solution (d = 1.08 g/ml) separated from pure water at 25 ºC? a) 36.7 b) 30.6 c) 29.3 d) A 6.0 m H 2 SO 4 solution has d = 1.34 g/ml. What is the mass percent of H 2 SO 4 in this solution? a) 56.1 b) 58.8 c) 37.0 d) no answer was given 13. When water boils, what primary forces are overcome? a) An H-O bond is broken. b) Only the dispersion forces are overcome. c) Hydrogen bonding forces are overcome. d) The dipole-dipole intermolecular forces are overcome. 14. The solubility of O 2 (g), in water at 25 o C is 3.16 ml/100 g H 2 O when the gas pressure was maintained at 1 atm. What pressure of O 2 (g) would be required to produce a saturated solution containing 10.9 ml/100 g H 2 O? a) 4.45 b) 3.45 c) d) Consider the variation of the vapor pressure with temperature for some common solvents shown in the right side to answer this question. The Dead sea is approximately 1300 ft below Sea level and its barometric pressure is approximately 830 torr. Will be the boiling point of water be elevated from 100 C by? a) less than 10 C. b) 10 C to 25 C 2

3 c) 25 C to 50 C d) above 50 C Part II. Phase changes (12 pts): Consider the phase diagram of the substance shown here. 1) Approximately what is the normal boiling point? a) 170 K b) 300 K c) 460 K 2) What is the normal melting point of the substance? a) 170 K b) 180 K c) 300 K 3) What is the physical state of the substance of the substance under the conditions of T = 350 K, P = 0.9 atm? a) solid b) liquid c) gas 4) Consider the same phase diagram in the above question. Which statement applies? a) The path A C represents sublimation. b) Following the path A B C, the compound would first liquefy and then vaporize. c) If the compound is in state A, continued reduction of the pressure (at constant temperature) will cause it to melt. d) None of these statements is correct. Part III (33 pts: 11 pts each) Calculations: Show all work for full credit. Please express all answers with proper units and correct number of significant figures. 1. A ml sample of an aqueous solution contains 1.08 g of human serum albumin, a blood plasma protein. The solution has an osmotic pressure of 5.85 mmhg at 298 K. What is the molar mass of the albumin? MM = 6.86 x 10 4 g/mol 3

4 3. Glycerin, C 3 H 8 O 3 (92.1 g/mol), is a nonvolatile non-electrolyte with density of 1.26 g/ml at 25 C. a) Calculate the vapor pressure at 25 C of a solution made by adding 50.0 ml of glycerin to 500. ml of water. The vapor pressure of pure water at 25 C is 23.8 mmhg. b) Calculate the boiling point of the solution (K b for water = 0.52 C/m). a) Vapor pressure = 23.2 mm Hg b) Boiling point = C 3. Initial rate data were obtained at a particular temperature for the following reaction: 2 ClO 2 (aq) + 2 OH - (aq) ClO 3 - (aq) + ClO 2 - (aq) + H 2 O (l) Expt. Initial [ClO 2 ] Initial [OH - ] Initial Rate of Rxn (M) (M) (M.s -1 ) x x x 10-4 a) What is the overall order of the reaction? b) What is the rate law for the reaction? c) What is the rate constant of the reaction? a) Overall order = 3 b) Rate law = k [ClO 2 ] 2 [OH - ] c) k = 120 M -2 s -1 4

5 Exam 1 Spring 2008 You will have 60 minutes to complete this exam. The exam has 4 pages plus a reference page. When you are told to do so, tear off the Periodic cover sheet and use as required during exam. Constants & Useful Equation : PREFERENCE SHEET FOR CHEM 108 Gas Constant: R = J/K.mol = x 10-3 kj/k.mol = L atm/mol.k K = C 1 atm = 760 torr = 760 mmhg d (density) = m)/v ln (P 1 /P 2 ) = ( H vap /R){(T 1 -T 2 )/T 1 T 2 } C g = k.p g n i = P i /P t PV = nrt π = MRT T = i. Km. P 1 = χ 1.P 1 o P = χ 2.P 1 o Rate = k[a] ln [A] o = kt ln[a] = - kt + ln[a] o t 1/2 = ln 2/k = 0.693/k [A] Rate = k[a] 2 1/[A] - 1/[A] o = kt t 1/2 = 1/k[A] o Rate = k [A] = - kt + [A] o t 1/2 = [A] o /2k k = Ae -Ea/RT ln k = (-E a /R)(1/T) + ln A H Li Na K Rb Cs Fr (223) 4 Be Mg Ca Sr Ba Ra Periodic Table of the Elements Sc Ti V Cr Mn Fe Co Ni Cu Zn Y La Ac Zr Hf Rf (261) 41 Nb Ta Db (262) 42 Mo W Sg (263) 43 Tc (98) 75 Re Bh (262) 44 Ru Os Hs (265) 45 Rh Ir Mt (266) 46 Pd Pt Uun (269) 47 Ag Au Uuu (272) 48 Cd Hg Uub (277) B C N O F Al Ga In Tl Si Ge Sn Pb P As Sb Bi S Se Te Po (209) 17 Cl Br I At (210) 2 He Ne Ar Kr Xe Rn (222) Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (145) Th Pa U Np Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (260) 5

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B I N G O B I N G O. Hf Cd Na Nb Lr. I Fl Fr Mo Si. Ho Bi Ce Eu Ac. Md Co P Pa Tc. Uut Rh K N. Sb At Md H. Bh Cm H Bi Es. Mo Uus Lu P F.

B I N G O B I N G O. Hf Cd Na Nb Lr. I Fl Fr Mo Si. Ho Bi Ce Eu Ac. Md Co P Pa Tc. Uut Rh K N. Sb At Md H. Bh Cm H Bi Es. Mo Uus Lu P F. Hf Cd Na Nb Lr Ho Bi Ce u Ac I Fl Fr Mo i Md Co P Pa Tc Uut Rh K N Dy Cl N Am b At Md H Y Bh Cm H Bi s Mo Uus Lu P F Cu Ar Ag Mg K Thomas Jefferson National Accelerator Facility - Office of cience ducation

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