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Midterm

[Exam Tutorial] Chem 120 Term Test 1 2011 Questions

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Department
Chemistry
Course Code
CHEM 120
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FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Name:_________________________ Prof. A. Mittermaier Dr. A. Fenster 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. DATA THAT MAY BE USEFUL STP: 0°C and 1 bar 1 mol gas at STP: 22.4 L –23 k = 1.38 x 10 J/K 0 K = – 273215 °C e = 2.718 2 1 Pa = 1 N/m 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 = 0.08206 L atm /(mol K) 1 mol = 6.02 x 10molecules J4.14 cal 1 P1 1 P2 2 MP MPV PV  nRT  d  m  n1 1 n2 2 RT RT 1 N 2 3 RT 3RT P  mu ek urms P  hdg 3 V 2 N A M Integrated Rate Laws:Arrhequastion: E /RT Order 0: [A] = [A0 - k eA  a ln k2  E a 11 t - k  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) Calculate u rmsn m/s, for H (2) molecules at 30°C. 3 a) 5.26 × 10 2/s b) 6.09 × 10 m/s c) 6.13 × 10 m/s 3 d) 2.74 × 10 3/s e) 1.94 × 10 m/s 2) A 500.0 mL sample of O (g)2is at 780 mmHg and 30°C. What will be the new volume if, with constant pressure and amount of gas, the temperature is decreased to -15°C? a) 426 mL b) 587 mL c) 500 mL d) 250 mL e) 437 mL 3) Diethyl ether (CH C3 OC2 CH )2was 3he first general anesthetic. It was first used in 1846 for surgical procedures. What is the density in g/L of diethyl ether at 27 °C and 1.11 atm? a) 2.03 × 10 g/L b) 3.34 g/L c) 0.299 g/L d) 37.1 g/L e) 2.71 g/L 4) Calculate the height in meters of a column of liquid glycerol (density =1.26 g/cm 3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm ).3 a) 8.20 m b) 8.20 × 10 m c) 0.704 m d) 44.4 m e) 70.4 m 5) How many liters of H 2are needed to make 327 L of NH by3the reaction: N 2(g) + 3 H2(g) → 2NH (g3, if the gases are at the same temperature and pressure? a) 491 L b) 654 L c) 218 L d) 38.5 L e) 327 L 6) In a gaseous mixture of neon and xenon that contains 50% neon by volume, a) the Ne and Xe atoms have the same average speed. b) there are more Ne atoms than Xe atoms. c) the Ne atoms are on the average moving more slowly than the Xe atoms. d) the total mass of Xe is equal to the total mass of Ne. e) the average kinetic energy of the Ne atoms is equal to that of the Xe atoms 7) What volume (in liters) would be occupied by 25 g of oxygen gas (O ) 2t 1.50 atm and 95°C? a) 130 L b) 15.7 L c) 18.0 L d) 4.06 L e) 63.2 L 8) A 5.00 L container of unknown gas at 25.0 °C has a pressure of 2.45 atm. The mass of the gas is 19.06 g. What gas is in the container? a) NO 2 b) Cl 2 c) C 2 2 d) F 2 e) SO 3 9) A 10 L container holds a mixture of 5 gases at 0ºC. The composition of the mixture is given below. What is the partial pressure of 2? N 2g) 10 g O (g) 1 g 2 H 2g) 20 g CO (2) 7 g He (g) 3 g a) 608 torr b) 800 torr c) 1340 torr d) 932 torr e) 22 torr 10)A mercury manometer is used at a barometric pressure of 100.7 kPa. If the mercury level at the open end of the manometer is 50 cm higher than the mercury level at the closed end, as shown, what is the pressure of the enclosed gas? a) 50 torr b) 500 torr c) 1255 torr d) 150.7 torr e) 260 torr 11)The heat of combustion of several fuels are listed in the table below. On a per gram basis, which fuel releases the most energy? Fuel ΔH comb(kJ/mole) C(s) -393.5 CH 4g) -890.8 CH OH(l) 726.1 3 C3H 8g) 2219.2 H2(g) -285.8 a) C(s) b) C 3 (8) c) CH (4) d) H 2(g) e) CH OH(l) 3 12)250.0 g of hot coffee at 95.0 °C are placed in a 0.200 kg mug at 20.0 °C. The specific heat of the coffee is 4.00 J/g °C, while that of the mug is 0.80 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) 61.7 °C c) 76.0 °C d) 57.5 °C e) 117 °C 13)Some “beetles” defend themselves by spraying hot quinone, C 6H 4 (2), at their enemies. Calculate ΔH for the reaction: C6H 4OH) (2) + H O2(l2 → C H O6(l4 2 2H O(l) 2 Given: C H6(O4) (l) 2 C H O 6l)4+ 2 (g) 2 ΔH= +177.4 kJ, and the standard enthalpies of formation of H O2(l2 and H O(2) are -187.4 and -285.8 kJ/mol, respectively. a) +79.00 kJ b) -384.2 kJ c) -206.8 kJ d) -561.6 kJ e) 624.2 kJ 14)Enthalpy is defined as: a) the energy contained within a system b) the heat of combustion c) the work not limited to pressure volume work d) the sum of the kinetic and potential energies e) the sum of the internal energy and the pressure-volume product of a system. 15)The standard ent
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