Lecture Notes C: Thermodynamics I (cont)
|
|
- Dwain Hubert Richardson
- 6 years ago
- Views:
Transcription
1 Lecture Notes C: Thermodynamics I (cont) How big would an asteroid have to be to evaporate the photic zone of Earth s oceans. The photic zone is the first 200m of the ocean, and is the depth which gets sufficient sunlight to support photosynthetic life. Typical speed of an asteroid = 20 km/s Surface area of water on the earth = x 10 6 km 2 Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 1 of 10
2 1) Standard states Sea level acts as a standard state sea level ocean altitude A altitude B altitude difference between A and B is difference between altitudes relative to sea level Chemical Standard States: gas: 1 atm and 25 o C. substance in aqueous solution: 1M concentration element or compound: most stable form at 1 atm and 25 o C (O 2, H 2, graphite (C) etc.) 2) Heats of formation (or Enthalpy s of formation) Enthalpy change associated with creating one mole of a chemical substance from the elements in their standard states, H 2 (g) + O 2 (g) H 2 O (l) H o = kj H f o ( H 2 O(l) ) = kj/mole The heat of formation of FeCO 3 (s) is kj/mole. Write the corresponding reaction and give its reaction enthalpy. 3) Calculating reaction enthalpies from heats of formation. Elements in standard states products reactants Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 2 of 10
3 For a general reaction: aa + bb cc + dd Using the data in the appendix of the textbook, calculate the enthalpy of combustion for methanol vapor (CH 3 OH (g) ). Assume the combustion produces CO 2 (g) and H 2 O (g). H f o (CH 3 OH (g) ) = kj/mol ; H f o ( CO 2 (g) ) = kj/mol ; H f o ( H 2 O (g) ) = kj/mol C (graphite) 2 O 2 (g) 2 H 2 (g) CH 3 OH(g) 3/2 O 2 (g) CO 2 (g) 2 H 2 O (g) Concept Which of the following is correct? a) H f o (CS 2 (l)) = kj/mol ; H f o (CS 2 (g)) = kj/mol b) H f o (CS 2 (l)) = kj/mol ; H f o (CS 2 (g)) = kj/mol Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 3 of 10
4 Concept State whether each of the following is obviously incorrect: 1) H o f (N 2 (g) at 25 o C ) = kj/mole a) obviously incorrect b) could be ok 2) H o f (C 2 H 4 (g) at 25 o C) = kj/mole a) obviously incorrect b) could be ok 3) H o f (Si (g) at 25 o C ) = kj/mole a) obviously incorrect b) could be ok 4) H o f (As (g) at 25 o C ) = kj/mole a) obviously incorrect b) could be ok Hydrogen (perhaps produced by solar energy) would be an ideal alternative to fossil fuels, since it does not produce pollutants or green house gases when burned. The problem is that it is a gas, and hard to store and transport. What volume of hydrogen gas at 1.00 atm and 25 o C would be required to produce an amount of energy equivalent to that produced by the combustion of a gallon of octane (C 8 H 18 ) to form CO 2 (g) and H 2 O(l)? H f o (C 8 H 18 ) = kj/mol H f o (CO 2 (g)) = kj/mol H f o (H 2 O (l) ) = kj/mol Density of C 8 H 18 at 25 o C is g/m Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 4 of 10
5 The Bombardier Beetle defends itself by spraying nearly boiling water on its predators. It has two glands on the tip of its abdomen. Each gland has two compartments. The inner compartment holds an aqueous solution of hydroquinone and hydrogen peroxide. The outer compartment holds a mixture of enzymes that catalyze the following reaction: C 6 H 4 (OH) 2 (aq) + H 2 O 2 (aq) C 6 H 4 O 2 (aq) + 2 H 2 O (l) hydroquinone hydrogen peroxide quinone When threatened, the beetle squeezes some fluid from the inner compartment into the outer compartment, and sprays the mixture (which is near its boiling point) onto the predator. The thermodynamic properties are: H f o (H 2 O (l) ) = kj/mol ; H f o (H 2 O 2(aq) ) = kj/mol C 6 H 4 (OH) 2 (aq) ---> C 6 H 4 O 2 (aq) + H 2 (g) H= 177kJ Suppose the concentration of the hydroquinone solution is 2.0M and the concentration of the H 2 O 2 solution is 2.0M. What is the temperature of the solution after mixing 1ml of the hydroquinone solution with 1ml of the H 2 O 2 solution? Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 5 of 10
6 Concept Suppose the concentration of H 2 O 2 is 2.5M, and that of hydroquinone is 2.0M. What happens to the final temperature of the solution? a) same as above b) higher than above c) lower than above Suppose the bug mixes 0.5ml of the hydroquinone solution with 0.5ml of H 2 O 2. What happens to the final temperature of the solution? a) same as above b) higher than above c) lower than above Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 6 of 10
7 4) Bond enthalpy CH 4 (g) ---> CH 3(g) + H (g) H o = 438kJ C 2 H 6 (g) ---> C 2 H 5(g) + H (g) H o = 410kJ CHCl 3 (g) --> CCl 3(g) + H (g) H o = 380kJ CHBr 3 (g) --> CBr 3(g) + H (g) H o = 377kJ Average Bond Enthalpies in kj/mole (Table 7.3) Molar Enthalpy of Atomization H- C- C= C N- N= N O- O= H C N O S F Cl Br I Estimate H for the following reaction, using the bond enthalpy s listed above. Compare this to that obtained from the table at the end of the book. H 2 CCH 2 + H 2 --> H 3 CCH 3 Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 7 of 10
8 5) Molar Enthalpy of Atomization (element in standard state) (single, gas-phase atom) H Gas-phase atoms provides a convenient reference when using bond enthalpies to estimate the heat of formation of a molecule. Estimate the heat of formation of H 2 CCH 2 using the atomization energies and bond enthalpy s in the table. Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 8 of 10
9 6) Clarification: Sign of H and conventions for H f o vs. bond enthalpies Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 9 of 10
10 7) Enthalpies of Formation versus Bond Enthalpies 2CO (g) + O 2 (g) 2CO 2 (g) H f o (kj/mol) Molar Enthalpy of Vaporization: C = 716.7kJ, O = 249.2kJ Bond Enthalpies: CO triple bond: 1080kJ O=O : 498kJ C=O : 728kJ from table (really 804 in CO 2 ) Lecture Notes C: Thermodynamics I (cont) Distributed on: Monday, January 22, 2001 Page 10 of 10
Lecture Notes C: Thermodynamics I (cont)
Lecture Notes C: Thermodynamics I (cont) 1) The tools of thermochemistry (from page 2 of Lecture Notes B) How do we measure and quantify heat given off or absorbed by a reaction (lecture notes B)? Definition
More informationb. 2.8 x 10-3 M min -1 d. 1.5 x 10-3 M min -1 Answer C
Chem 30 Name Exam 3 November 8, 207 00 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and significant
More informationExam 3, Ch 7, 19 November 7, Points
Chem 120 Name Exam 3, Ch 7, 19 November 7, 2008 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More informationWhen activation energy is added to the reactants, a so-called activated complex is formed.
SESSION 12: ENERGY & CHEMICAL CHANGE Key Concepts In this session we will focus on summarising what you need to know about: Activation energy and activation complex Energy profile of a reaction Enthalpy
More informationEnergy 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 informationLecture Notes B: Thermodynamics I (cont)
Lecture Notes B: Thermodynamics I (cont) 1) Energy flow in chemical systems: Overview and outline General approach In the heat transfer problems of Lecture Notes A: Iron poker in water q iron = -q water
More information10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics
Chapter 10 Thermochemistry 10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics OFB Chap. 10 1 Chapter 10 Thermochemistry Heat
More information10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics
Chapter 10 Thermochemistry 10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics OFB Chap. 10 1 OFB Chap. 10 2 Thermite Reaction
More informationEntropy. Spontaneity. Entropy. Entropy mol of N 2 at 1 atm or 1 mol of N 2 at atm. process a process that occurs without intervention
Entropy Spontaneity process a process that occurs without intervention can be fast or slow Entropy (s) the measure of molecular randomness or disorder Think of entropy as the amount of chaos Entropy Predict
More informationChem 75 February, 2017 Practice Exam 2
As before, here is last year s Exam 2 in two forms: just the questions, and then the questions followed by their solutions. 1. (2 + 6 + 8 points) At high temperature, aluminum nitride, AlN(s), decomposes
More informationUNIVERSITY 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 informationCHEM 1105 S10 March 11 & 14, 2014
CHEM 1105 S10 March 11 & 14, 2014 Today s topics: Thermochemistry (Chapter 6) Basic definitions Calorimetry Enthalpy Thermochemical equations Calculating heats of reaction Hess s Law Energy and Heat Some
More informationPractice 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 informationFirst Law of Thermodynamics: energy cannot be created or destroyed.
1 CHEMICAL THERMODYNAMICS ANSWERS energy = anything that has the capacity to do work work = force acting over a distance Energy (E) = Work = Force x Distance First Law of Thermodynamics: energy cannot
More informationUnit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit.
Unit 5: Spontaneity of Reaction You need to bring your textbooks everyday of this unit. THE LAWS OF THERMODYNAMICS 1 st Law of Thermodynamics Energy is conserved ΔE = q + w 2 nd Law of Thermodynamics A
More informationChapter 8 Thermochemistry: Chemical Energy
Chapter 8 Thermochemistry: Chemical Energy 國防醫學院生化學科王明芳老師 2011-11-8 & 2011-11-15 Chapter 8/1 Energy and Its Conservation Conservation of Energy Law: Energy cannot be created or destroyed; it can only be
More informationUNIVERSITY 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 informationTo calculate heat (q) for a given temperature change: heat (q) = (specific heat) (mass) ( T) where T = T f T i
Use your textbook or other resources available to answer the following questions General Information: Thermochemistry Phase Change A change in the physical form/state but not a change in the chemical identity
More informationChapter 16. Thermodynamics. Thermochemistry Review. Calculating H o rxn. Predicting sign for H o rxn. Creative Commons License
Chapter 16 Thermodynamics GCC CHM152 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution License 4.0. ChemWiki (CC
More informationCHEM 101 Fall 08 Exam III(a)
CHEM 101 Fall 08 Exam III(a) On the answer sheet (scantron) write you name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on your
More informationHomework 11 - Second Law & Free Energy
HW11 - Second Law & Free Energy Started: Nov 1 at 9:0am Quiz Instructions Homework 11 - Second Law & Free Energy Question 1 In order for an endothermic reaction to be spontaneous, endothermic reactions
More informationSection 3.0. The 1 st Law of Thermodynamics. (CHANG text Chapter 4) 3.1. Revisiting Heat Capacities Definitions and Concepts
Section 3.0. The 1 st Law of Thermodynamics (CHANG text Chapter 4) 3.1. Revisiting Heat Capacities 3.2. Definitions and Concepts 3.3. The First Law of THERMODYNAMICS 3.4. Enthalpy 3.5. Adiabatic Expansion
More informationCHEMISTRY 202 Hour Exam III. Dr. D. DeCoste T.A. 21 (16 pts.) 22 (21 pts.) 23 (23 pts.) Total (120 pts)
CHEMISTRY 202 Hour Exam III December 1, 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 23 questions on 12 numbered pages. Check now to make sure you have a complete exam. You have two hours
More informationHigher Chemistry Principles to Production October Revision
igher Chemistry Principles to Production October Revision You should use your class notes, Evans2Chemweb and Scholar to help. Show your working for each question. Sections covered so far; Principles to
More informationExam 1. Name: Recitation Section Lenny.: 6:30 7:30 (circle one): Greg.: 6:30 7:30 Student Number: Nic.: 6:30 7:30
Exam 1 Name: Recitation Section Lenny.: 6:30 7:30 (circle one): Greg.: 6:30 7:30 Student Number: Nic.: 6:30 7:30 Please show your work and either circle your answers or put your answers in the boxes provided.
More informationThermochemistry. Chapter 6. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Thermochemistry Chapter 6 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Energy is the capacity to do work. Radiant energy comes from the sun and is earth s
More informationChapter 19 Chemical Thermodynamics
Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H
More informationUnit 13: Rates and Equilibrium- Guided Notes
Name: Period: What is a Chemical Reaction and how do they occur? Unit 13: Rates and Equilibrium- Guided Notes A chemical reaction is a process that involves of atoms Law of Conservation of : Mass is neither
More informationWarm up. 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]?
Warm up 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]? 4) What is the concentration of H 2 SO 4 if 30.1 ml
More informationChapter 6 Problems: 9, 19, 24, 25, 26, 27, 31-33, 37, 39, 43, 45, 47, 48, 53, 55, 57, 59, 65, 67, 73, 78-82, 85, 89, 93
Chapter 6 Problems: 9, 19, 24, 25, 26, 27, 31-33, 37, 39, 43, 45, 47, 48, 53, 55, 57, 59, 65, 67, 73, 78-82, 85, 89, 93 Chapter 6 Thermochemistry The study of chemical reactions and the energy changes
More informationEquilibrium. Dynamic Equilibrium, Position of Equilibrium, Liquid-Vapor Equilibrium, Equilibrium Law January 2015
Equilibrium Dynamic Equilibrium, Position of Equilibrium, Liquid-Vapor Equilibrium, Equilibrium Law January 2015 Equilibrium Review What is equilibrium? Features of equilibrium the rate of the forward
More informationThermodynamics- 1) Hess's law states that 1) The standard enthalpy of an overall reaction is the sum of the enthalpy changes in individual reaction. ) Enthalpy of formation of compound is same as the enthalpy
More informationFACULTY 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 informationLesmahagow High School
Lesmahagow High School Higher Chemistry Enthalpy - Tutorial Questions Energy Changes Tutorial Questions 1 1. A pupil found the enthalpy of combustion of propan-1-ol using the following apparatus: a. In
More information2013, 2011, 2009, 2008 AP
Lecture 15 Thermodynamics I Heat vs. Temperature Enthalpy and Work Endothermic and Exothermic Reactions Average Bond Enthalpy Thermodynamics The relationship between chemical reactions and heat. What causes
More informationChemistry 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 informationChapter 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 informationChapter 6. Heat Flow
Chapter 6 Thermochemistry Heat Flow Heat (q): energy transferred from body at high T to body at low T Two definitions: System: part of universe we are interested in Surrounding: the rest of the universe
More informationUse the data in the table to calculate the standard enthalpy of formation of liquid methylbenzene, C 7 H 8. Substance C(s) H 2 (g) C 7 H 8 (l)
Q1.(a) Define the term standard enthalpy of formation, H f ο (3) (b) Use the data in the table to calculate the standard enthalpy of formation of liquid methylbenzene, C 7 H 8 Substance C(s) H 2 (g) C
More informationCHM 2046 Test 2 Review: Chapter 12, Chapter 13, & Chapter 14
Chapter 12: 1. In an 80.0 L home aquarium, the total pressure is 1 atm and the mole fraction of nitrogen is 0.78. Henry s law constant for N 2 in water at 25 is 6.1 x 10 4. What mass of nitrogen is dissolved
More informationENERGY (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 informationLecture 2. Review of Basic Concepts
Lecture 2 Review of Basic Concepts Thermochemistry Enthalpy H heat content H Changes with all physical and chemical changes H Standard enthalpy (25 C, 1 atm) (H=O for all elements in their standard forms
More informationLecture Presentation. Chapter 6. Thermochemistry. Sherril Soman Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 6 Thermochemistry Sherril Soman Grand Valley State University Chemical Hand Warmers Most hand warmers work by using the heat released from the slow oxidation of iron 4 Fe(s)
More informationThermodynamics: Entropy, Free Energy, and Equilibrium
Chapter 16 Thermodynamics: Entropy, Free Energy, and Equilibrium spontaneous nonspontaneous In this chapter we will determine the direction of a chemical reaction and calculate equilibrium constant using
More information17.4 Calculating Heats Essential Understanding Heats of reaction can be calculated when it is difficult or
17.4 Calculating Heats of Reaction Essential Understanding Heats of reaction can be calculated when it is difficult or impossible to measure them directly. Lesson Summary Hess s Law Hess s law provides
More informationFACULTY OF SCIENCE MID-TERM EXAMINATION CHEMISTRY 120 GENERAL CHEMISTRY MIDTERM 1. Examiners: Prof. B. Siwick Prof. I. Butler Dr. A.
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
More informationThermochemistry Chapter 4
Thermochemistry Chapter 4 Thermochemistry is the study of energy changes that occur during chemical reactions Focus is on heat and matter transfer between the system and the surroundings Energy The ability
More informationClass XI Chapter 6 Thermodynamics Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii)
More informationGeneral Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University. Module 4: Chemical Thermodynamics
General Chemistry I Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University Module 4: Chemical Thermodynamics Zeroth Law of Thermodynamics. First Law of Thermodynamics (state quantities:
More informationChapter 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 information4 Energetics Exam-style questions. AQA Chemistry
1 Amended from AQA Chemistry Unit 2 Chemistry in Action CHEM2 January 2011 (Question 9) a A student carried out a laboratory experiment to determine the enthalpy change when a sample of butan-1-ol was
More informationChapter 8. Thermochemistry 강의개요. 8.1 Principles of Heat Flow. 2) Magnitude of Heat Flow. 1) State Properties. Basic concepts : study of heat flow
강의개요 Basic concepts : study of heat flow Chapter 8 Thermochemistry Calorimetry : experimental measurement of the magnitude and direction of heat flow Thermochemical Equations Copyright 2005 연세대학교이학계열일반화학및실험
More informationChapter 5. Thermochemistry
Chapter 5 Thermochemistry Dr. A. Al-Saadi 1 Preview Introduction to thermochemistry: Potential energy and kinetic energy. Chemical energy. Internal energy, work and heat. Exothermic vs. endothermic reactions.
More informationPractice Questions Placement Exam for Entry into Chemistry 120
Practice Questions Placement Exam for Entry into Chemistry 120 Potentially Useful Information Avogadro's number = 6.0221420 10 23 h = 6.6260688 10 34 J s c = 2.9979246 10 8 m/s 1amu = 1.6605387 10 27 kg
More informationHeat energy change revision questions
Name: Heat energy change revision questions Date: Time: Total marks available: 63 Total marks achieved: Q1. A student uses this apparatus to find the increase in temperature of water when methanol, CH
More informationAP Chapter 6: Thermochemistry Name
AP Chapter 6: Thermochemistry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 6: Thermochemistry 2 Warm-Ups (Show your work for credit)
More informationEnergy is the capacity to do work
1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More informationCHEMISTRY 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 informationChapter 5 THERMO. THERMO chemistry. 5.4 Enthalpy of Reactions 5.5 Calorimetry 5.6 Hess s Law 5.7 Enthalpies of Formation
Chapter 5 THERMO THERMO chemistry 5.4 Enthalpy of Reactions 5.5 Calorimetry 5.6 Hess s Law 5.7 Enthalpies of Formation Chemical Equations 1 st WRITE the Chemical Equation 2 nd BALANCE the Chemical Equation
More informationMULTIPLE CHOICE PORTION:
AP Chemistry Fall Semester Practice Exam 4 MULTIPLE CHOICE PORTION: Write the letter for the correct answer to the following questions on the provided answer sheet. Each multiple choice question is worth
More informationChapter 6 Thermochemistry
Chapter 6 Thermochemistry Contents and Concepts Understanding Heats of Reaction The first part of the chapter lays the groundwork for understanding what we mean by heats of reaction. 1. Energy and Its
More informationMost hand warmers work by using the heat released from the slow oxidation of iron: The amount your hand temperature rises depends on several factors:
Lecture Presentation Chapter 6 Thermochemistry Chemical Hand Warmers Most hand warmers work by using the heat released from the slow oxidation of iron: Exothermic reaction 4 Fe(s) + 3 O 2 (g) 2 Fe 2 O
More information5.) One mole of an ideal gas expands isothermally against a constant pressure of 1 atmosphere. Which of the following inequalities is true?
Part 1: Multiple Choice. (4 pts each, 44 pts total) Instructions: Bubble in the correct answer on your Scantron form AND circle the answer on your exam. Each question has one correct answer. 1.) The answer
More informationIntroduction to Thermochemistry. Thermochemistry Unit. Definition. Terminology. Terminology. Terminology 07/04/2016. Chemistry 30
Thermochemistry Unit Introduction to Thermochemistry Chemistry 30 Definition Thermochemistry is the branch of chemistry concerned with the heat produced and used in chemical reactions. Most of thermochemistry
More informationEquilibrium. What is equilibrium? Hebden Unit 2 (page 37 69) Dynamic Equilibrium
Equilibrium What is equilibrium? Hebden Unit (page 37 69) Dynamic Equilibrium Hebden Unit (page 37 69) Experiments show that most reactions, when carried out in a closed system, do NOT undergo complete
More informationA) 93 C B) 54 C C) 75 C D) 86 C E) 134 C. Sec# 1-4 Grade# 60. Q2. Which one of the following is an example of a physical change?
Q1. The melting and boiling points in a newly devised thermometer are 0 X and 100 X which are equivalent to 45 C and 115 C respectively in Celsius scale. What is a temperature reading of 86 X in C in this
More information15.1 The Concept of Equilibrium
Lecture Presentation Chapter 15 Chemical Yonsei University 15.1 The Concept of N 2 O 4 (g) 2NO 2 (g) 2 Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. The
More informationMultiple Choice 2 POINTS EACH Select the choice that best answers the question. Mark it clearly on your answer sheet.
Chemistry 45.5 100 Points Take Home Exam 1 2009-10 Name: Student ID: Form A Multiple Choice 2 POINTS EACH Select the choice that best answers the question. Mark it clearly on your answer sheet. 1. Likes
More informationEXTRA HOMEWORK 5A 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 is determined with
More informationThermochemistry. 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 informationName Class Date. As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings.
Name Class Date Thermochemistry 17.1 The Flow of Energy As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings. Process Cause Effect endothermic
More informationFinal Exam Review-Honors Name Period
Final Exam Review-Honors Name Period This is not a fully comprehensive review packet. This packet is especially lacking practice of explanation type questions!!! You should study all previous review sheets
More informationChapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics
Chapter 8 Thermochemistry: Chemical Energy Chapter 8 1 Chemical Thermodynamics Chemical Thermodynamics is the study of the energetics of a chemical reaction. Thermodynamics deals with the absorption or
More informationCP Chapter 17 Thermochemistry
CP Chapter 17 Thermochemistry Thermochemistry Thermochemistry is the study of energy that occur during chemical reactions and phase changes (changes of state) The Nature of Energy Energy is the ability
More informationChapter Eighteen. Thermodynamics
Chapter Eighteen Thermodynamics 1 Thermodynamics Study of energy changes during observed processes Purpose: To predict spontaneity of a process Spontaneity: Will process go without assistance? Depends
More informationAS Paper 1 and 2 Energetics
AS Paper 1 and 2 Energetics Q1.Nitric acid is produced industrially from ammonia, air and water using the following sequence of reactions: 4NH 3 (g) + 5O 2(g) 4NO(g) + 6H 2O(g) H = 909 kj mol 1 (2) 2NO(g)
More informationElectrochemistry: Oxidation numbers. EIT Review F2006 Dr. J.A. Mack. Electrochemistry: Oxidation numbers
EIT Review F2006 Dr. J.A. Mack Electrochemistry: Oxidation numbers In the compound potassium bromate (KBrO 3 ), the oxidation number of bromine (Br) is? www.csus.edu/indiv/m/mackj/ Part 2 38 39 +1 +2 Oxidation
More informationThermodynamics - Energy Relationships in Chemical Reactions:
Thermodynamics - Energy Relationships in Chemical Reactions: energy - The capacity to do work. Types of Energy: radiant-energy from the sun. potential-energy due to an objects position. chemical-energy
More informationChem 1A Dr. White Fall 2015 Exam 3 Practice Problems
Exam 3 Practice Problems 1. The face centered cubic cell of copper has an edge length of 0.362 nm. Calculate the density of copper (g/cm 3 ). 2. Consider the following ionic substances and arrange them
More informationCHAPTER 12: Thermodynamics Why Chemical Reactions Happen
CHAPTER 12: Thermodynamics Why Chemical Reactions Happen Useful energy is being "degraded" in the form of unusable heat, light, etc. A tiny fraction of the sun's energy is used to produce complicated,
More informationHomework 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(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 informationContents and Concepts
Contents and Concepts 1. First Law of Thermodynamics Spontaneous Processes and Entropy A spontaneous process is one that occurs by itself. As we will see, the entropy of the system increases in a spontaneous
More informationContents and Concepts
Contents and Concepts 1. First Law of Thermodynamics Spontaneous Processes and Entropy A spontaneous process is one that occurs by itself. As we will see, the entropy of the system increases in a spontaneous
More information6. 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 informationExam 4 and Final Exam Review
Exam 4 and Final Exam Review General Chemistry I Material Exam 4: Wednesday, Dec 12 th 5:30 6:30 PM Bolton 150 Chapters 1-19 44 multiple choice questions Final Exam: Wednesday, Dec 19 th 3:00-5:00 PM Bolton
More informationName Date Class THERMOCHEMISTRY
Name Date Class 17 THERMOCHEMISTRY SECTION 17.1 THE FLOW OF ENERGY HEAT AND WORK (pages 505 510) This section explains the relationship between energy and heat, and distinguishes between heat capacity
More informationLecture Outline. 5.1 The Nature of Energy. Kinetic Energy and Potential Energy. 1 mv
Chapter 5. Thermochemistry Common Student Misconceptions Students confuse power and energy. Students confuse heat with temperature. Students fail to note that the first law of thermodynamics is the law
More information= = 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 informationChapter 5 Practice Multiple Choice & Free
Name Response 1. A system has an increase in internal energy, E, of 40 kj. If 20 kj of work, w, is done on the system, what is the heat change, q? a) +60 kj d) -20 kj b) +40 kj e) -60 kj c) +20 kj 2. Which
More information(02) WMP/Jun10/CHEM2
Energetics 2 Section A Answer all the questions in the spaces provided. 1 An equation for the equilibrium reaction between hydrogen, iodine and hydrogen iodide is shown below. H 2 (g) + I 2 (g) 2HI(g)
More informationEnergy and Chemical Change
Energy and Chemical Change Section 15.1 Energy In your textbook, read about the nature of energy. In the space at the left, write true if the statement is true; if the statement is false, change the italicized
More informationS = k log W 11/8/2016 CHEM Thermodynamics. Change in Entropy, S. Entropy, S. Entropy, S S = S 2 -S 1. Entropy is the measure of dispersal.
Entropy is the measure of dispersal. The natural spontaneous direction of any process is toward greater dispersal of matter and of energy. Dispersal of matter: Thermodynamics We analyze the constraints
More informationA) 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 informationThermochemistry. Chapter 6. Dec 19 8:52 AM. Thermochemistry. Energy: The capacity to do work or to produce heat
Chapter 6 Dec 19 8:52 AM Intro vocabulary Energy: The capacity to do work or to produce heat Potential Energy: Energy due to position or composition (distance and strength of bonds) Kinetic Energy: Energy
More informationThe Equilibrium State. Chapter 13 - Chemical Equilibrium. The Equilibrium State. Equilibrium is Dynamic! 5/29/2012
Chapter 13 - Chemical Equilibrium The Equilibrium State Not all chemical reactions go to completion; instead they attain a state of equilibrium. When you hear equilibrium, what do you think of? Example:
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
More informationEnergy & Chemistry. Internal Energy (E) Energy and Chemistry. Potential Energy. Kinetic Energy. Energy and Chemical Reactions: Thermochemistry or
Page III-5-1 / Chapter Five Lecture Notes Energy & Chemistry Energy and Chemical Reactions: Thermochemistry or Thermodynamics Chapter Five Burning peanuts supplies sufficient energy to boil a cup of water
More information2) C 2 H 2 (g) + 2 H 2 (g) ---> C 2 H 6 (g) Information about the substances
Thermochemistry 1) 2 C 4 H 10 (g) + 13 O 2 (g) ------> 8 CO 2 (g) + 10 H 2 O(l) The reaction represented above is spontaneous at 25 C. Assume that all reactants and products are in their standard states.
More informationEntropy, Free Energy, and Equilibrium
Entropy, Free Energy, and Equilibrium Chapter 17 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs
More information