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Midterm

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Department
Chemistry
Course
CHEM 110
Professor
Sebastien Breau
Semester
Fall

Description
FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Name:_________________________ Prof. A. Mittermaier Prof. J. Schwarcz AssFocateriner: 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 4). If not, fill that in. 2. This examination comprises 30 questions (14 pages including cover page and 4 blank pages). All questions are of equal value. 3. Transfer answers to the scantron computer scorecard provided. 4. Both the scorecard and the examination paper will be collected separately at the end of the examination period. 5. Simple Calculators are allowed, and translation dictionaries. 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. NOTE TO INVIGILATORS: At the end of the exam, both scorecards and exam papers should be collected. Collect scorecards separately. THESE DATA WILL BE PROVIDED ON THE MIDTERM EXAMINATION STP: 0°C and 1 a–23 1 mol gas at STP: 22.4 L k = 1.38 x 10 J/K 0 K = – 273.15 °C e = 2.718 1 Pa = 1 N/m2 g = 9.81 m/s 1 atm = 101.3 kPa = 760 Torr π = 3.14 1 bar = 100,000 Pa = 100 kPa R = 8.314 J/(mol K) 1 J = 1 kg m /s = 1 kPa L 23 = 0.08206 L atm /(mol K) 1 mol = 6.02 x 10 molecules P1 1 P2 2 MP MPV PV = nRT = d = m = n1 1 n 2 2 RT RT 1 N 2 3 RT 3 RT P = mu ek= urms= P = hdg 3 V 2 NA M Integrated Rate Laws:Arrhquastion: −E /RT Order 0: [A] = [A0 - k eA= a k2 − Ea ⎛⎞11 t - k ln = − ⎜⎟ Order 1: [A] = [A0 e 1 1 2 ⎝⎠ Order 2: 1/[A] = 1/[A0+ kt Standard states for various elements under STP conditions: Hydrogen: H (g)2 Carbon: C(s, graphite) Nitrogen: N (2) Oxygen: O (g)2op Cpues) SulpS(u)r: 1) The standard enthalpy of formation for CuSO · 5H O4s) is 22278.0 kJ/mole at 25°C. The chemical equation to which this value applies is: a) Cu(s) + S(s) + 5 H O(2) + 2 O (g) 2 CuSO · 5H O(s4 2 b) Cu(s) + SO (g4 + 5 H O(g2 → CuSO · 5H O(s4 2 c) Cu(s) + S(s) + 9/2 O (g)2+ 5 H (g) 2 CuSO · 5H O(s4 2 d) 2Cu(s) + 2 SO (g) + 5 H O(g) → 2CuSO · 5H O(s) 2 2 4 2 e) Cu(s) + S(s) + 5/9 O (g2 + 5 H (g)2→ CuSO · 5H O(4) 2 2) Choose the INCORRECT statement. a) The heat capacity is the quantity of heat required to change the temperature of the system by one degree. b) The temperature of two gases is equal when the average kinetic energy per molecule is the same in each. c) Specific heat capacity is an extensive quantity. d) The law of conservation of energy can be written: qsystem + qsurroundings = 0. e) In general, the specific heat capacity of a substance in solid form is lower than that of the liquid form. 3) Calculate ΔH° of fctane, C H (l8, 18ven the enthalpy of combustion of octane to CO (2) and H O(2), -5471 kJ/mol, and the standard enthalpies of formation of CO (g) 2 and H O2l), -393.5 kJ/mol and -285.8 kJ/mol, respectively. a) +4792 kJ/mol b) -4792 kJ/mol c) +249.2 kJ/mol d) -249.2 kJ/mol e) +589.1 kJ/mol 4) For the reaction H 2(g) + 1/2 O 2g) → H O(2) ΔH° = -241.8 kJ/mol, what quantity of heat, in kJ, evolved when a 72.0 g mixture containing equal parts of H and O (by 2 2 mass) is burned? a) 1088 kJ b) 544 kJ c) 272 kJ d) 8630 kJ e) 4860 kJ 5) Which of the following is NOT a thermodynamic function of state: a) temperature b) enthalpy c) density d) heat e) volume 6) For the reaction: 2N O (g) → 4NO (g) + O (g) at the time when N O is being 2 5 2 2 2 5 consumed at a rate of -1.2 × 10M/s, what is the rate at whi2h O is being formed? -4 a) 2.4 × 10 M/s b) 3.0 × 10-5 M/s -4 c) 1.2 × 10 M/s d) 4.8 × 10-4 M/s e) 6.0 × 10-5 M/s 7) Define "rate law". a) An equation derived using collision theory that describes how the rate of reaction depends on the concentration of reactants. b) A statement that describes how the rate of a reaction depends on the concentration of reactants derived from the balanced equation. c) An equation derived using collision theory that describes how the rate of reaction depends on temperature, orientation and number of collisions d) An experimentally determined equation that describes how the rate of reaction depends on temperature, orientation and number of collisions. e) An experimentally determined equation that describes how the rate of reaction depends on the concentration of reactants. 8) Data for the reaction A + B → C are given below. Find the rate constant for this system. Experiment  [A], M  [B], M  Initial rate, M/s    1  0.030  0.060  2.5 × 10   2  0.030  0.020  2.5 × 10   -5   3  0.060  0.060  10.0 × 10 a) 2.8 × 10-2 Ms-1 b) 2.8 × 10-2 M s -1 c) 1.7 × 10-3 M -1s-1 d) 2.8 × 10-2 M s1 -1 e) 1.7 × 10-3 Ms-1 9) In the first order, reaction A → products, [A] = 0.400 M initially and 0.250 M after 15.0 min, what will [A] be after 175 min? a) 2.31 × 10-1 M b) 3.70 × 10-2 M c) 1.04 × 10-3 M d) 6.024 × 10-3 M e) 1.67 × 10-3 M 10)Activation energy is: i) The minimum kinetic energy that each of the molecules involved in a collision must posses to produce a reaction. ii) The minimum total kinetic energy required for the molecules in a collision to produce a react
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