FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY MIDTERM 1. Examiners: Prof. B. Siwick Prof. I. Butler Dr. A.
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1 FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY MIDTERM 1 Examiners: Prof. B. Siwick Prof. I. Butler Dr. A. Fenster Name: INSTRUCTIONS 1. Enter your student number and name on the computer scorecard provided by filling in the appropriate circles. Check that your scorecard has the correct version number filled in (version 1). If not, fill that in. One mark will be awarded for correctly recording your student number on the scantron card. Double check that you have done that properly! 2. This examination comprises 30 questions (16 pages including cover page and 4 blank pages), but will be marked out of 31 (see point 1 above). All questions are of equal value. 3. Transfer all answers to the scantron computer scorecard provided. 4. Only the scantron card will be collected at the end of the examination period. 5. ONLY the SHARP EL510RB calculator may be used in the Midterm. Translation dictionaries are also permitted. NO notes or texts are allowed. 6. The Examination Security Monitor Program detects pairs of students with unusually similar answer patterns on multiple-choice exams. Data generated by this program can be used as admissible evidence, either to initiate or corroborate an investigation or a charge of cheating under Section 16 of the Code of Student Conduct and Disciplinary Procedures.
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3 DATA THAT MAY BE USEFUL STP: 0 C and 1 bar 1 mol gas at STP: 22.7 L k = 1.38 x J/K 0 K = C e = Pa = 1 N/m 2 g = 9.81 m/s 2 1 atm = kpa = 760 Torr π = bar = 100,000 Pa = 100 kpa R = J/(mol K) 1 J = 1 kg m 2 /s 2 = 1 kpa. L = L. atm/(mol. K) 1 mol = 6.02 x molecules ΔH vap (H 2 O) = kj. mol -1 1 cal = J Density of Water: 1 g/cm 3 d MP RT P 1 3 N V 3RT u rms P hdg M mu 2 e k 3 2 RT N A
4 Standard states for various elements under STP conditions: Hydrogen: H 2 (g) Carbon: C(s, graphite) Nitrogen: N 2 (g) Oxygen: O 2 (g) Copper: Cu(s) Sulphur: S(s) Cobalt: Co(s) Chlorine: Cl 2 (g)
5 1) Which statement regarding a sample of an ideal gas is false? A) If the pressure is doubled at constant temperature, the volume decreases by a factor of two. B) If the temperature is doubled at constant pressure, the volume decreases by a factor of two. C) If the temperature is doubled at constant volume, the pressure increases by a factor of two. D) If the volume is doubled at constant temperature, the pressure decreases by a factor of two. E) If the number of moles of gas is doubled at constant temperature and pressure, the volume increases by a factor of two. 2) Halothane is a modern anesthetic that is nonflammable and relatively safe for patients. What is the molar mass of halothane (in grams per mole) if 798 milligrams occupies 92.4 milliliters at 16.5 ºC and 790 Torr? A) 197 B) 304 C) 1.24 x 10 3 D) 27.4 E) 209 3) A 1.54 L vessel contains He at a temperature of 22 ºC and a pressure of 270 mmhg. A 688 ml vessel contains Ne at a temperature of 36.2 ºC and a pressure of.165 atm. Both of these gases are placed in a 2.00 L vessel at 302 K. What is the final pressure (in atm) in the 2.00 L vessel? A) B) C) D) E) ) A 54.6 ml sample of nitrogen gas was collected over water at 23.7 ºC and a barometric pressure of 752 mmhg. What mass of nitrogen was collected? [Vapor pressure of water at 23.7 ºC is 22 mmhg] A) 60.3 mg B) 58.7 mg C) 56.8 mg D) 61.4 mg E) 63.3 mg
6 5) In a sample of air at STP, the ratio of the root-mean-square velocity of O 2 to that of N 2 (i.e. u rms (O 2 )/u rms (N 2 )) is equal to: A) 1.27 B) 1.00 C) 0.94 D) 0.82 E) ) The complete combustion of octane (C 8 H 18 (l)) is given by the equation: 2 C 8 H 18 (l) + 25 O 2 (g) 16 CO 2 (g) + 18 H 2 O(g) How many liters of CO 2 (g) are produced at 72.4 C and 659 mmhg for every L of octane burned? (density of C 8 H 18 (l) = g/ml) A) 6.10 L B) 8.48 x 10 2 L C) 6.09 x 10 3 L D) 2.78 x 10 3 L E) 9.45 L 7) The measured Pressure of a non-ideal van der Waals gas compared to an ideal gas is: A) lower, because the gases expand B) lower, because of intermolecular attractive forces C) higher, because the molecules repel each other D) lower, because the molecules occupy space E) higher, because of intermolecular attractive forces 8) Which of the following is not a part of the kinetic-molecular theory of gases? A) A gas is composed of a large number of extremely small particles B) Individual molecules may gain or lose energy as a result of collisions, but the total energy remains constant at fixed temperature C) Gas particles are involved in constant, random straight line motion. D) Gas particles collide only with the walls of the container E) Gas particles are separated by great distance; a gas is mostly empty space. 9) A gaseous mixture consists of 50.0% O 2, 25.0% N 2, and 25.0% Cl 2, by mass. At standard temperature and pressure, the partial pressure of: A) O 2 (g) is equal to 380 torr B) Cl 2 (g) is less than 0.25 atm C) O 2 (g) is equal to 1.6 atm D) N 2 (g) is equal to 0.20 atm E) Cl 2 (g) is greater than 0.25 atm
7 10) Assuming ideal gas behavior, which of the following gases would have the lowest density at standard temperature and pressure? A) N 2 B) Kr C) SF 6 D) Ne E) CO 2 11) The heat of fusion for water is 6.25 kj/mol and for ethyl alcohol is 5.67 kj/mol. The amount of heat that would melt 30.0 grams of water would melt how many grams of ethyl alcohol (C 2 H 5 OH)? A) 33.1 g B) 11.7 g C) 31.0 g D) 8.2 g E) 84.5 g 12) The standard enthalpy of formation for CoCl 2 6H 2 O(s) is kj/mole at 25 C. The chemical equation to which this value applies is: A) Co(s) + Cl 2 (g) + 6 O 2 (g) + 6 H 2 (g) CoCl 2 6H 2 O(s) B) Co(s) + Cl 2 (g) + 6 H 2 O(g) CoCl 2 6H 2 O(s) C) CoCl 2 (s) + 6H 2 O(g) CoCl 2 6H 2 O(s) D) Co(s) + Cl 2 (g) + 3 O 2 (g) + 6 H 2 (g) CoCl 2 6H 2 O(s) E) CoCl 2 (s) + 3 O 2 (g) + 6 H 2 (g) CoCl 2 6H 2 O(s) 13) g of hot coffee at 92.1 C are placed in a kg mug at 21.0 C. The specific heat of the coffee is 4.10 J/g C, while that of the mug is 0.82 J/g C. Assuming no heat is lost to the surroundings, what is the final temperature of the system: mug + coffee? A) 84.7 C B) 56.6 C C) 74.0 C D) C E) 82.1 C
8 14) Given the following thermochemical equations: 2 O(g) -> O 2 (g) ΔH o = -249 kj/mol 2 H(g) + O(g) -> H 2 O(g) ΔH o = -803 kj/mol C(graphite) + 2 O(g) -> CO 2 (g) ΔH o = -643 kj/mol C(graphite) + 2 H 2 (g) -> CH 4 (g) ΔH o = -75 kj/mol 2 H(g) -> H 2 (g) ΔH o = -436 kj/mol Calculate the heat of combustion of methane: CH 4 (g) + 2O 2 (g) -> CO 2 (g) + 2H 2 O(g) A) kj B) kj C) kj D) -804 kj E) kj 15) Calculate ΔH f of pentane, C 5 H 12 (l), given the enthalpy of combustion of pentane to CO 2 (g) and H 2 O(l), kj/mol, and the standard enthalpies of formation of CO 2 (g) and H 2 O(l), kj/mol and kj/mol, respectively. A) kj/mol B) kj/mol C) kj/mol D) kj/mol E) kj/mol 16) For the reaction: H 2 (g) + 1/2 O 2 (g) H 2 O(g) ΔH = kj/mol What quantity of heat is evolved when a kg mixture containing equal parts of H 2 and O 2 (by mass) is burned? A) kj B) 544 kj C) kj D) kj E) kj
9 17) What is the final temperature if 5 grams of octane (C 8 H 18 ) is combusted in a bomb calorimeter with heat capacity of 25.0 kj/ C and an initial temperature of 22.0 C? The heat of combustion of octane is kj/g. A) C B) C C) C D) C E) C 18) Which statement is correct? A) The standard heat of formation of an element is always negative B) Since H = U + (PV), H cannot equal U C) q and w are state functions D) The first law of thermodynamics says q = -w for a closed system E) q + w is a state function 19) Steam engines have been extremely important devices. To get a sense of why, answer the following question: How much work is done when 18.0g of liquid water is vaporized at 100 C against a constant external pressure of kpa? A) No work is done B) 1.3 kj C) 2.3 kj D) 3.1 kj E) 3100 kj 20) An Exothermic reaction will (choose the best answer): A) Decrease the temperature of an isolated system B) Result in a positive heat flow in a closed system C) Decrease the internal energy of a closed system D) Increase the internal energy of an isolated system E) Increase the internal energy of a closed system. 21) What is the maximum number of hydrogen bonds in which an isopropyl alcohol molecule, (CH 3 ) 2 CH(OH), could theoretically participate? A) 0 B) 1 C) 2 D) 3 E) 4
10 22) Which one of the following substances is most likely to be a solid at room temperature? A) CO 2 B) (COOH) 2 C) CClF 3 D) SO 2 E) C 2 H 5 Cl 23) Which of the following molecules would be most likely to be moderately soluble in both toluene and water? (a) CCl 4 (b) KCl (c) (C 5 H 11 )OH (d) C 6 H 5 OH A) None of them B) Only (c) C) Only (a) and (d) D) Only (b) E) Only (c) and (d) 24) What is the boiling point of water, in C, on top of a mountain about 3000 m above sea level, if the atmospheric pressure is 70.6 kpa? [ΔH vap (H 2 O) = kj. mol -1, standard atmospheric pressure = kpa] A) 2.75 x 10-3 B) 95.4 C) 90.7 D) 100 E) ) Which one of the following labels is not found on a typical phase diagram? A) Sublimate B) Solid C) Liquid D) Pressure E) Gas
11 26) Which of the following famous scientists have a mathematical chemistry law or equation associated with their names? (a) Hess (b) Boyle (c) Dalton (d) Clausius (e) Van der Waals A) All of them B) None of them C) All of them but (d) D) Only (c) and (e) E) Only (b) and (d) 27) Which one of the following molecules would you least expect to be intermolecularly hydrogen bonded? A) HF B) C 2 H 5 OH C) CH 3 NH 2 D) CH 3 COOH E) H 2 S 28) You want to find out how long it would take to soft-boil an egg on top of Mount Everest in boiling water. If it normally takes 5 minutes in Montreal, which one of the following statements would be correct? A) It will take less than 5 minutes. B) It will take more than 5 minutes. C) It depends on the volume of water used. D) It depends on the amount of steam produced by boiling the water. E) None of the other answers is correct
12 29) Which the following statements are correct? (a) Methanol, CH 3 OH, has a higher surface tension than does n-butyl alcohol, C 4 H 9 OH (b) n-pentane, C 5 H 12, has a higher viscosity than does n-octane, C 8 H 18 (c) Hydrogen bonding interactions are stronger than are London forces (d) A liquid will boil when its vapor pressure is equal to the atmospheric pressure (e) Freezing is an exothermic process A) (a) and (b) B) (c), (d) and (e) C) (a) and (e) D) (b) and (d) E) None of the answers is correct 30) Which of the following statements concerning phase diagrams are correct? (a) Two different phases can coexist above the critical point (b) The triple point is the same for every substance (c) Sublimation is the term used to describe a solid-to-gas phase change (d) Deposition is the reverse process of evaporation (e) Supersaturated is the term used to describe substances above their critical point. A) All of them B) None of them C) (c) D) (a), (b) and (e) E) (c) and (d).
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