FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY MIDTERM 1. Examiners: Prof. B. Siwick Prof. I. Butler Dr. A.

Size: px
Start display at page:

Download "FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY MIDTERM 1. Examiners: Prof. B. Siwick Prof. I. Butler Dr. A."

Transcription

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.

2

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).

13

14

15

16

Practice Midterm 1 CHEMISTRY 120 GENERAL CHEMISTRY. Examiners: Prof. B. Siwick Prof. A. Mittermaier Prof. A. Fenster

Practice Midterm 1 CHEMISTRY 120 GENERAL CHEMISTRY. Examiners: Prof. B. Siwick Prof. A. Mittermaier Prof. A. Fenster Practice Midterm 1 CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Prof. A. Mittermaier Prof. A. Fenster Name: INSTRUCTIONS (for the actual Midterm) 1. Enter your student number and name on

More information

FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY. Examiners: Prof. B. Siwick Prof. A. Mittermaier Prof. J.

FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY. Examiners: Prof. B. Siwick Prof. A. Mittermaier Prof. J. FACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Prof. A. Mittermaier Prof. J. Schwarcz Name: Associate Examiner: A. Fenster INSTRUCTIONS 1. Enter your

More information

FACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, :30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY

FACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, :30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY FACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, 2011. 6:30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Prof. A. Mittermaier Dr. A. Fenster Name: Associate Examiner: A. Fenster

More information

MCGILL UNIVERSITY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEM 120 MONDAY MARCH 16, :30PM 8:30PM VERSION NUMBER: 1

MCGILL UNIVERSITY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEM 120 MONDAY MARCH 16, :30PM 8:30PM VERSION NUMBER: 1 MCGILL UNIVERSITY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEM 120 MONDAY MARCH 16, 2009 6:30PM 8:30PM VERSION NUMBER: 1 Instructions: BEFORE YOU BEGIN: Enter your student number and name on the computer

More information

Chemistry Lab Fairfax High School Invitational January 7, Team Number: High School: Team Members Names:

Chemistry Lab Fairfax High School Invitational January 7, Team Number: High School: Team Members Names: Chemistry Lab Fairfax High School Invitational January 7, 2017 Team Number: High School: Team Members Names: Reference Values: Gas Constant, R = 8.314 J mol -1 K -1 Gas Constant, R = 0.08206 L atm mol

More information

Chem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.

Chem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question. Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. An open-tube manometer is used to measure the pressure in a flask. The atmospheric

More information

Useful Information to be provided on the exam: 1 atm = 760 mm Hg = 760 torr = lb/in 2 = 101,325 Pa = kpa. q = m C T. w = -P V.

Useful Information to be provided on the exam: 1 atm = 760 mm Hg = 760 torr = lb/in 2 = 101,325 Pa = kpa. q = m C T. w = -P V. Chem 101A Study Questions, Chapters 5 & 6 Name: Review Tues 10/25/16 Due 10/27/16 (Exam 3 date) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach

More information

Unit Five: Intermolecular Forces MC Question Practice April 14, 2017

Unit Five: Intermolecular Forces MC Question Practice April 14, 2017 Unit Five: Intermolecular Forces Name MC Question Practice April 14, 2017 1. Which of the following should have the highest surface tension at a given temperature? 2. The triple point of compound X occurs

More information

CHEMISTRY 110 EXAM 3 April 2, 2012 FORM A 1. Which plot depicts the correct relationship between the volume and number of moles of an ideal gas at constant pressure and temperature? 2. The height of the

More information

A) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance.

A) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance. PX0411-1112 1. Which of the following statements concerning liquids is incorrect? A) The volume of a liquid changes very little with pressure. B) Liquids are relatively incompressible. C) Liquid molecules

More information

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW Version A UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, 2015 5-6 pm (60 minutes) Version A DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW Answer all multiple choice questions

More information

SUPeR Chemistry CH 222 Practice Exam

SUPeR Chemistry CH 222 Practice Exam SUPeR Chemistry CH 222 Practice Exam This exam has been designed to help you practice working multiple choice problems over the material that will be covered on the first CH 222 midterm. The actual exams

More information

a) 1.3 x 10 3 atm b) 2.44 atm c) 8.35 atm d) 4.21 x 10-3 atm e) 86.5 atm

a) 1.3 x 10 3 atm b) 2.44 atm c) 8.35 atm d) 4.21 x 10-3 atm e) 86.5 atm 1. (6 pts) A sample of gas with a volume of 750 ml exerts a pressure of 756 mm Hg at 30.0 0 C. What pressure (atm) will the sample exert when it is compressed to 250 ml and cooled to -25.0 0 C? a) 1.3

More information

General Chemistry 1 CHM201 Unit 3 Practice Test

General Chemistry 1 CHM201 Unit 3 Practice Test General Chemistry 1 CHM201 Unit 3 Practice Test 1. Heat is best defined as a. a substance that increases the temperature and causes water to boil. b. a form of potential energy. c. a form of work. d. the

More information

(E) half as fast as methane.

(E) half as fast as methane. Name AP Chem / / AP Chem Practice Exam #2 Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the BLUE SIDE of your scantron for each of the following.

More information

HEMISTRY 110 EXAM 3 April 6, 2011 FORM A When the path is blocked, back up and see more of the way. 1. A 250 L vessel is evacuated and then connected to a 50.0 L bulb with compressed nitrogen. The pressure

More information

DATA THAT YOU MAY USE UNITS Conventional Volume ml or cm 3 = cm 3 or 10-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = Pa CONSTANTS

DATA THAT YOU MAY USE UNITS Conventional Volume ml or cm 3 = cm 3 or 10-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = Pa CONSTANTS DATA THAT YOU MAY USE UNITS Conventional S.I. Volume ml or cm 3 = cm 3 or 0-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr =.03 0 5 Pa torr = 33.3 Pa Temperature C 0 C = 73.5 K PV L-atm =.03 0 5 dm 3

More information

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW Version B UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, 2015 5-6 pm (60 minutes) Version B DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW Answer all multiple choice questions

More information

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes Thermochemistry Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes heat flows from high to low (hot cool) endothermic reactions: absorb energy

More information

Chem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.

Chem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question. Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Determine the oxidation number of the underlined element in K 2CO 3. a. 1 b. 2 c.

More information

Enthalpies of Reaction

Enthalpies of Reaction Enthalpies of Reaction Enthalpy is an extensive property Magnitude of H is directly related to the amount of reactant used up in a process. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) H = 890 kj 2CH 4 (g)

More information

Thermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation

Thermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation THERMOCHEMISTRY Thermochemistry Energy 1st Law of Thermodynamics Enthalpy / Calorimetry Hess' Law Enthalpy of Formation The Nature of Energy Kinetic Energy and Potential Energy Kinetic energy is the energy

More information

PX-III Chem 1411 Chaps 11 & 12 Ebbing

PX-III Chem 1411 Chaps 11 & 12 Ebbing PX-III Chem 1411 Chaps 11 & 12 Ebbing 1. What is the name for the following phase change? I 2 (s) I 2 (g) A) melting B) condensation C) sublimation D) freezing E) vaporization 2. Which of the following

More information

Chapter 11. Liquids and Intermolecular Forces

Chapter 11. Liquids and Intermolecular Forces Chapter 11 Liquids and Intermolecular Forces States of Matter The three states of matter are 1) Solid Definite shape Definite volume 2) Liquid Indefinite shape Definite volume 3) Gas Indefinite shape Indefinite

More information

Gases. A gas. Difference between gas and vapor: Why Study Gases?

Gases. A gas. Difference between gas and vapor: Why Study Gases? Gases Chapter 5 Gases A gas Uniformly fills any container. Is easily compressed. Mixes completely with any other gas. Exerts pressure on its surroundings. Difference between gas and vapor: A gas is a substance

More information

Chapter 6 The States of Matter. Examples of Physical Properties of Three States of Matter

Chapter 6 The States of Matter. Examples of Physical Properties of Three States of Matter Chapter 6 The States of Matter Examples of Physical Properties of Three States of Matter 1 Three States of Matter Solids: Fixed shape, fixed volume, particles are held rigidly in place. Liquids: Variable

More information

Exam 4, Enthalpy and Gases

Exam 4, Enthalpy and Gases CHEM 1100 Dr. Stone November 8, 2017 Name_ G Exam 4, Enthalpy and Gases Equations and constants you may need: ΔE system = q + w PV = nrt R = 0.0821 (L*atm)/(mole*K) w = -PΔV K.E. = 1 2 m *µ 2 rms µ rms=

More information

Kwantlen Polytechnic University Chemistry 1105 S10 Spring Term Test No. 3 Thursday, April 4, 2013

Kwantlen Polytechnic University Chemistry 1105 S10 Spring Term Test No. 3 Thursday, April 4, 2013 Kwantlen Polytechnic University Chemistry 1105 S10 Spring Term Test No. 3 Thursday, April 4, 2013 Name: Student Number Instructions: Ensure that this exam contains all eight pages including this page.

More information

Gases: Their Properties & Behavior. Chapter 09 Slide 1

Gases: Their Properties & Behavior. Chapter 09 Slide 1 9 Gases: Their Properties & Behavior Chapter 09 Slide 1 Gas Pressure 01 Chapter 09 Slide 2 Gas Pressure 02 Units of pressure: atmosphere (atm) Pa (N/m 2, 101,325 Pa = 1 atm) Torr (760 Torr = 1 atm) bar

More information

Thermochemistry: Energy Flow and Chemical Reactions

Thermochemistry: Energy Flow and Chemical Reactions Thermochemistry: Energy Flow and Chemical Reactions Outline thermodynamics internal energy definition, first law enthalpy definition, energy diagrams, calorimetry, theoretical calculation (heats of formation

More information

CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A

CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A 1. Consider a balloon filled with 5 L of an ideal gas at 20 C. If the temperature of the balloon is increased by 70 C and the external pressure acting on the

More information

0. Graphite is thermodynamically less stable that diamond under standard conditions. 1. True 2. False

0. Graphite is thermodynamically less stable that diamond under standard conditions. 1. True 2. False 0. Graphite is thermodynamically less stable that diamond under standard conditions. 1. True 2. False 1. Which statement would be the best interpretation of the First Law of Thermodynamics? 1. The total

More information

Homework 01. Phase Changes and Solutions

Homework 01. Phase Changes and Solutions HW01 - Phase Changes and Solu!ons! This is a preview of the published version of the quiz Started: Jan 16 at 1:pm Quiz Instruc!ons Homework 01 Phase Changes and Solutions Question 1 Given that you have

More information

This should serve a s a study guide as you go on to do the problems in Sapling and take the quizzes and exams.

This should serve a s a study guide as you go on to do the problems in Sapling and take the quizzes and exams. CHM 111 Chapter 9 Worksheet and Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding

More information

Comparison of Solids, Liquids, and Gases

Comparison of Solids, Liquids, and Gases CHAPTER 8 GASES Comparison of Solids, Liquids, and Gases The density of gases is much less than that of solids or liquids. Densities (g/ml) Solid Liquid Gas H O 0.97 0.998 0.000588 CCl 4.70.59 0.00503

More information

Thermochemistry: Heat and Chemical Change

Thermochemistry: Heat and Chemical Change Thermochemistry: Heat and Chemical Change 1 Heat or Thermal Energy (q) Heat is a form of energy Is heat the same as temperature? Heat flows between two objects at different temperatures. Hot Cold 2 Chemical

More information

Chapter 11 Gases 1 Copyright McGraw-Hill 2009

Chapter 11 Gases 1 Copyright McGraw-Hill 2009 Chapter 11 Gases Copyright McGraw-Hill 2009 1 11.1 Properties of Gases The properties of a gas are almost independent of its identity. (Gas molecules behave as if no other molecules are present.) Compressible

More information

1. Increasing the pressure above a liquid will cause the boiling point of the liquid to:

1. Increasing the pressure above a liquid will cause the boiling point of the liquid to: JASPERSE CHEM 210 PRACTICE TEST 1 VERSION 2 Ch. 11 Liquids, Solids, and Materials Ch. 10 Gases Ch. 15 The Chemistry of Solutes and Solutions Ch. 13 Chemical Kinetics 1 Constants and/or Formulas Formulas

More information

Chapter Elements That Exist as Gases at 25 C, 1 atm. 5.2 Pressure basic physics. Gas Properties

Chapter Elements That Exist as Gases at 25 C, 1 atm. 5.2 Pressure basic physics. Gas Properties 5.1 Elements That Exist as Gases at 25 C, 1 atm Chapter 5 The Gaseous State YOU READ AND BE RESPONSIBLE FOR THIS SECTION! Gaseous compounds include CH 4, NO, NO 2, H 2 S, NH 3, HCl, etc. Gas Properties

More information

Please print: Provided information: A periodic table and conversion chart are provided for you inside this exam booklet.

Please print: Provided information: A periodic table and conversion chart are provided for you inside this exam booklet. Please print: Last name: First name: Chem 1061 Exam 3 Fall 2004 Andy Aspaas, Instructor Tuesday, November 9, 2004 Instructions: Time: You have 85 minutes to complete this exam. Allowed items: This exam

More information

Chapter 12 Intermolecular Forces of Attraction

Chapter 12 Intermolecular Forces of Attraction Chapter 12 Intermolecular Forces of Attraction Intermolecular Forces Attractive or Repulsive Forces between molecules. Molecule - - - - - - Molecule Intramolecular Forces bonding forces within the molecule.

More information

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 14, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW

UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 14, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW Version A UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 14, 2014 5-6 pm (60 minutes) Version A DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW Answer all multiple choice questions

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following is most likely not a gas at room temperature? 1) A) H2 B) Cl2

More information

CHEM 101 Fall 09 Final Exam (a)

CHEM 101 Fall 09 Final Exam (a) CHEM 101 Fall 09 Final Exam (a) On the answer sheet (scantron) write your name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on

More information

Chapter 11. Intermolecular Forces, Liquids, and Solids

Chapter 11. Intermolecular Forces, Liquids, and Solids Sample Exercise 11.1 (p. 450) In which of the following substances is hydrogen bonding likely to play an important role in determining physical properties: methane (CH 4 ), hydrazine (H 2 NNH 2 ), methyl

More information

Gases. Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures.

Gases. Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures. Gases Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures Gases Properties of Gases All elements will form a gas at

More information

Unit 6. Unit Vocabulary: Distinguish between the three phases of matter by identifying their different

Unit 6. Unit Vocabulary: Distinguish between the three phases of matter by identifying their different *STUDENT* Unit Objectives: Absolute Zero Avogadro s Law Normal Boiling Point Compound Cooling Curve Deposition Energy Element Evaporation Heat Heat of Fusion Heat of Vaporization Unit 6 Unit Vocabulary:

More information

Chem 112 Exam 1 Version A Spring /16/ :00am/Odago, M. O.

Chem 112 Exam 1 Version A Spring /16/ :00am/Odago, M. O. Chem 112 Exam 1 Version A Spring 2011 02/16/2011 10:00am/Odago, M. O. 1. The pressure of a certain gas is measured to be 25.1 mmhg. What is this pressure expressed in units of pascals? (1 atm=1.0125 x10

More information

Chapter 5 Thermochemistry

Chapter 5 Thermochemistry Chapter 5 Thermochemistry Learning Outcomes: Interconvert energy units Distinguish between the system and the surroundings in thermodynamics Calculate internal energy from heat and work and state sign

More information

1. When two pure substances are mixed to form a solution, then always

1. When two pure substances are mixed to form a solution, then always Name: Date: 1. When two pure substances are mixed to form a solution, then always A) there is an increase in entropy. B) there is a decrease in entropy. C) entropy is conserved. D) heat is released. E)

More information

Lecture 7 Enthalpy. NC State University

Lecture 7 Enthalpy. NC State University Chemistry 431 Lecture 7 Enthalpy NC State University Motivation The enthalpy change ΔH is the change in energy at constant pressure. When a change takes place in a system that is open to the atmosphere,

More information

CHEMISTRY 110 EXAM 3 Nov. 11, 2013 ORM A!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!" 1. The cylinder shown below is filled with enough N 2 gas at 25 o C to reach a

More information

Energy Heat Work Heat Capacity Enthalpy

Energy Heat Work Heat Capacity Enthalpy Energy Heat Work Heat Capacity Enthalpy 1 Prof. Zvi C. Koren 20.07.2010 Thermodynamics vs. Kinetics Thermodynamics Thermo = Thermo + Dynamics E (Note: Absolute E can never be determined by humans!) Can

More information

Chapter 5 The Gaseous State

Chapter 5 The Gaseous State Chapter 5 The Gaseous State Contents and Concepts Gas Laws We will investigate the quantitative relationships that describe the behavior of gases. 1. Gas Pressure and Its Measurement 2. Empirical Gas Laws

More information

Name: REGENTS CHEMISTRY

Name: REGENTS CHEMISTRY Name: REGENTS CHEMISTRY 1 Key Ideas Matter is classified as a pure substance or as a mixture of substances. (3.1q) Mixtures are composed of two or more different substances that can be separated by physical

More information

Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided.

Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided. CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. a. The gas

More information

Gases and Kinetic Molecular Theory

Gases and Kinetic Molecular Theory 1 Gases and Kinetic Molecular Theory 1 CHAPTER GOALS 1. Comparison of Solids, Liquids, and Gases. Composition of the Atmosphere and Some Common Properties of Gases 3. Pressure 4. Boyle s Law: The Volume-Pressure

More information

Ch. 6 Enthalpy Changes

Ch. 6 Enthalpy Changes Ch. 6 Enthalpy Changes Energy: The capacity to do work. In Physics, there are 2 main types of energy Kinetic (energy of motion) = ½ mv 2 Potential (energy of position due to gravity)= mgh In Chemistry,

More information

Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c

Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system

More information

Chemistry 1A, Spring 2008 Midterm Exam III, Version A April 14, 2008 (90 min, closed book)

Chemistry 1A, Spring 2008 Midterm Exam III, Version A April 14, 2008 (90 min, closed book) Chemistry 1A, Spring 2008 Midterm Exam III, Version A April 14, 2008 (90 min, closed book) Name: KEY SID: A Name: 1.) Write your name on every page of this exam. 2.) his exam has 15 multiple-choice questions

More information

Class work on Calorimetry. January 11 and 12, 2011

Class work on Calorimetry. January 11 and 12, 2011 Class work on Calorimetry January 11 and 12, 2011 Name 1. The number of calories needed to raise the temperature of 100 grams of water 10 degrees Celsius is the same as the number of calories needed to

More information

Thermodynamics- Chapter 19 Schedule and Notes

Thermodynamics- Chapter 19 Schedule and Notes Thermodynamics- Chapter 19 Schedule and Notes Date Topics Video cast DUE Assignment during class time One Review of thermodynamics ONE and TWO Review of thermo Wksheet Two 19.1-4; state function THREE

More information

Name Date Class THE FLOW OF ENERGY HEAT AND WORK

Name Date Class THE FLOW OF ENERGY HEAT AND WORK 17.1 THE FLOW OF ENERGY HEAT AND WORK Section Review Objectives Explain the relationship between energy, heat, and work Distinguish between exothermic and endothermic processes Distinguish between heat

More information

= = 10.1 mol. Molar Enthalpies of Vaporization (at Boiling Point) Molar Enthalpy of Vaporization (kj/mol)

= = 10.1 mol. Molar Enthalpies of Vaporization (at Boiling Point) Molar Enthalpy of Vaporization (kj/mol) Ch 11 (Sections 11.1 11.5) Liquid Phase Volume and Density - Liquid and solid are condensed phases and their volumes are not simple to calculate. - This is different from gases, which have volumes that

More information

Slide 1 / A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m 2 A 55 B 0.55 C 5.5 D 1.8 E 18

Slide 1 / A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m 2 A 55 B 0.55 C 5.5 D 1.8 E 18 Slide 1 / 76 1 A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m 2 A 55 B 0.55 C 5.5 D 1.8 E 18 Slide 2 / 76 2 A pressure of 1.00 atm is the same as a pressure of of mm Hg. A 193 B

More information

ENERGY (THERMOCHEMISTRY) Ch 1.5, 6, 9.10, , 13.3

ENERGY (THERMOCHEMISTRY) Ch 1.5, 6, 9.10, , 13.3 ENERGY (THERMOCHEMISTRY) Ch 1.5, 6, 9.10, 11.5-11.7, 13.3 Thermochemistry Prediction and measurement of energy transfer, in the form of heat, that accompanies chemical and physical processes. Chemical

More information

AGK s Fall 2006 Chem 111 Exam 2 Review Sheet

AGK s Fall 2006 Chem 111 Exam 2 Review Sheet AGK s Fall 2006 Chem 111 Exam 2 Review Sheet *NOTE: This list is fairly comprehensive but designed only as a study aid. You are responsible for all material covered in class and in assigned readings. While

More information

3. When the external pressure is kpa torr, water will boil at what temperature? a C b C c. 100 C d. 18 C

3. When the external pressure is kpa torr, water will boil at what temperature? a C b C c. 100 C d. 18 C Chemistry EOC Review 5: Physical Behavior of Matter 1. Which gas is monatomic at STP? a. chlorine b. fluorine c. neon d. nitrogen 2. What Kelvin temperature is equal to 25 C? a. 248 K b. 298 K c. 100 K

More information

Thermochemistry Chapter 8

Thermochemistry Chapter 8 Thermochemistry Chapter 8 Thermochemistry First law of thermochemistry: Internal energy of an isolated system is constant; energy cannot be created or destroyed; however, energy can be converted to different

More information

CHEMISTRY 109 #25 - REVIEW

CHEMISTRY 109 #25 - REVIEW CHEMISTRY 109 Help Sheet #25 - REVIEW Chapter 4 (Part I); Sections 4.1-4.6; Ch. 9, Section 9.4a-9.4c (pg 387) ** Review the appropriate topics for your lecture section ** Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc

More information

(a) graph Y versus X (b) graph Y versus 1/X

(a) graph Y versus X (b) graph Y versus 1/X HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below

More information

PLEASE DO NOT MARK ON THE EXAM. ALL ANSWERS SHOULD BE INDICATED ON THE ANSWER SHEET. c) SeF 4

PLEASE DO NOT MARK ON THE EXAM. ALL ANSWERS SHOULD BE INDICATED ON THE ANSWER SHEET. c) SeF 4 Chem 130 EXAM 4 Fall 99 PLEASE DO NOT MARK ON THE EXAM. ALL ANSWERS SHOULD BE INDICATED ON THE ANSWER SHEET QUESTIONS 1-5 MAY HAVE MORE THAN ONE POSSIBLE ANSWER CIRCLE ALL CORRECT RESPONSES TO EACH QUESTION

More information

Energy Relationships in Chemical Reactions

Energy Relationships in Chemical Reactions Energy Relationships in Chemical Reactions What is heat? What is a state function? What is enthalpy? Is enthalpy a state function? What does this mean? How can we calculate this? How are the methods the

More information

Chemistry Grade : 11 Term-3/Final Exam Revision Sheet

Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Exam Date: Tuesday 12/6/2018 CCS:Chem.6a,6b,6c,6d,6e,6f,7a,7b,7d,7c,7e,7f,1g Chapter(12):Solutions Sections:1,2,3 Textbook pages 378 to 408 Chapter(16):Reaction

More information

Chem Midterm 3 April 23, 2009

Chem Midterm 3 April 23, 2009 Chem. 101 - Midterm 3 April 3, 009 Name All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units and for the incorrect number of significant figures. Only

More information

2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container?

2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container? 1. Which gas law states that the volume of a fixed mass of a gas is directly proportional to its Kelvin temperature if the pressure is kept constant? A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac

More information

2. What is a measure of the average kinetic energy of particles? (A) heat capacity (B) molar enthalpy (C) specific heat (D) temperature

2. What is a measure of the average kinetic energy of particles? (A) heat capacity (B) molar enthalpy (C) specific heat (D) temperature Thermochemistry #1 Chemistry 3202 Name: 1. Classify the following systems as open or closed a) glass of cold water b) a gel filled freezer pack c) a burning candle d) a fluorescent lightbulb e) hot water

More information

LECTURE 4 Variation of enthalpy with temperature

LECTURE 4 Variation of enthalpy with temperature LECTURE 4 Variation of enthalpy with temperature So far, we can only work at 25 C. Like c v we define a constant pressure heat capacity, c p, as the amount of heat energy needed to raise the temperature

More information

Name: Class: Date: ID: A

Name: Class: Date: ID: A Name: Class: _ Date: _ CH11 1. Order the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest. A) dipole-dipole, London dispersion, ionic, and

More information

Thermochemistry-Part 1

Thermochemistry-Part 1 Brad Collins Thermochemistry-Part 1 Chapter 7 Thermochemistry Thermodynamics: The study of energy Thermochemistry: The study of energy in chemical reactions Energy: The capacity to do work Work = force

More information

CHM2045 Exam 3 Review Fall 2015

CHM2045 Exam 3 Review Fall 2015 The steps to solving any chemistry problem 1) Read Question 2) Re-read Question 3) Write down everything you are given 4) Write down what you are trying to find CHM2045 Exam 3 Review 1) Write out the following

More information

Chemistry 212 Fall 2017 Exam III - A

Chemistry 212 Fall 2017 Exam III - A Chemistry 212 Fall 2017 Exam III - A Name MULTIPLE CHOICE. (1 point each) Choose the one alternative that best completes the statement or answers the question. 1) An important step in the synthesis of

More information

10 States of Matter. Aubrey High School AP Chemistry. Period Date / / 10.2 Problems - Liquids and Gases

10 States of Matter. Aubrey High School AP Chemistry. Period Date / / 10.2 Problems - Liquids and Gases Aubrey High School AP Chemistry 10 States of Matter 1. Use the following table to answer these questions. Vapor Pressures of Various Liquids Temp. ( C) Ethyl alcohol Benzene Methyl salicylate Water Carbon

More information

= (25.0 g)(0.137 J/g C)[61.2 C - (-31.4 C)] = 317 J (= kj)

= (25.0 g)(0.137 J/g C)[61.2 C - (-31.4 C)] = 317 J (= kj) CHEM 101A ARMSTRONG SOLUTIONS TO TOPIC D PROBLEMS 1) For all problems involving energy, you may give your answer in either joules or kilojoules, unless the problem specifies a unit. (In general, though,

More information

g of CO 2 gas is at a temperature of 45 o C and a pressure of 125 kpa. What is the volume of the container? 11 L

g of CO 2 gas is at a temperature of 45 o C and a pressure of 125 kpa. What is the volume of the container? 11 L Name period AP Chemistry Unit 5 answers 1. A fixed quantity of gas at 23⁰C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is

More information

Hood River Valley High

Hood River Valley High Chemistry Hood River Valley High Name: Period: Unit 7 States of Matter and the Behavior of Gases Unit Goals- As you work through this unit, you should be able to: 1. Describe, at the molecular level, the

More information

Chemistry B11 Chapter 6 Gases, Liquids, and Solids

Chemistry B11 Chapter 6 Gases, Liquids, and Solids Chapter 6 Gases, Liquids, and Solids States of matter: the physical state of matter depends on a balance between the kinetic energy of particles, which tends to keep them apart, and the attractive forces

More information

CHEMISTRY 102B Hour Exam II. Dr. D. DeCoste T.A.

CHEMISTRY 102B Hour Exam II. Dr. D. DeCoste T.A. CHEMISTRY 10B Hour Exam II March 19, 015 Dr. D. DeCoste Name Signature T.A. This exam contains questions on 9 numbered pages. Check now to make sure you have a complete exam. You have one hour and thirty

More information

6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.

6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl. CH141 Practice Problems/Practice Final Exam Page 1 of 12 Name: 1. What is the SO 4 2- concentration of a solution prepared by dissolving 3.00 g of Na 2 SO 4 in 1.00 L of water? 2. What is the hybridization

More information

DO NOT OPEN UNTIL INSTRUCTED TO DO SO. CHEM 110 Dr. McCorkle Exam #3. While you wait, please complete the following information:

DO NOT OPEN UNTIL INSTRUCTED TO DO SO. CHEM 110 Dr. McCorkle Exam #3. While you wait, please complete the following information: DO NOT OPEN UNTIL INSTRUCTED TO DO SO CHEM 110 Dr. McCorkle Exam #3 While you wait, please complete the following information: Name: Student ID: Turn off cellphones and stow them away. No headphones, mp3

More information

Thermochemistry HW. PSI Chemistry

Thermochemistry HW. PSI Chemistry Thermochemistry HW PSI Chemistry Name Energy 1) Objects can possess energy as: (a) endothermic energy (b) potential energy A) a only B) b only C) c only D) a and c E) b and c (c) kinetic energy 2) The

More information

CHAPTER 10 LIQUID & SOLIDS

CHAPTER 10 LIQUID & SOLIDS Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 10 LIQUID & SOLIDS Day Plans for the day Assignment(s) for the

More information

Gases. Chapter 5. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Gases. Chapter 5. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Gases Chapter 5 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Elements that exist as gases at 25 0 C and 1 atmosphere 2 3 Physical Characteristics of Gases

More information

Chemistry 145 Exam number 2 name 10/8/98 # A.(64) Circle the best response. Record answers on the attached answer sheet.

Chemistry 145 Exam number 2 name 10/8/98 # A.(64) Circle the best response. Record answers on the attached answer sheet. Chemistry 145 Exam number 2 name 10/8/98 # A.(64) Circle the best response. Record answers on the attached answer sheet. 1. Which is NOT a unit for expressing pressure? a) Pascal b) lb/cm 3 c) torr d)

More information

Name: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry

Name: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical

More information

Phase Change DIagram

Phase Change DIagram States of Matter Phase Change DIagram Phase Change Temperature remains during a phase change. Water phase changes Phase Diagram What is a phase diagram? (phase diagram for water) Normal melting point:

More information

Name May 2, 2012 Physical Behavior of Matter and Bonding Review

Name May 2, 2012 Physical Behavior of Matter and Bonding Review Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool

More information

Question 2 Identify the phase transition that occurs when CO 2 solid turns to CO 2 gas as it is heated.

Question 2 Identify the phase transition that occurs when CO 2 solid turns to CO 2 gas as it is heated. For answers, send email to: admin@tutor-homework.com. Include file name: Chemistry_Worksheet_0039 Price: $4 (c) 2012 www.tutor-homework.com: Tutoring, homework help, help with online classes. Chapter 11

More information

Chapter 3. Thermochemistry: Energy Flow and Chemical Change. 5.1 Forms of Energy and Their Interconversion

Chapter 3. Thermochemistry: Energy Flow and Chemical Change. 5.1 Forms of Energy and Their Interconversion Chapter 3 Thermochemistry: Energy Flow and Chemical Change 5.1 Forms of Energy and Their Interconversion 5.2 Enthalpy: Chemical Change at Constant Pressure 5.3 Calorimetry: Measuring the Heat of a Chemical

More information

MUNISH KAKAR's INSTITUE OF CHEMISTRY

MUNISH KAKAR's INSTITUE OF CHEMISTRY ENTHALPY CHANGE & HESS's LAW ( WS #4 ) Q1. H and E for the reaction, S(s) + 3 O(g) SO3(g) are related as: (a) H = E 0.5 RT (b) H = E 1.5RT (c) H = E + RT (d) H = E + 1.5 RT Q. The enthalpy of solution

More information