Study Guide Chapter 5
|
|
- Nelson Reynolds
- 5 years ago
- Views:
Transcription
1 Directions: Answer the following 1. When writing a complete ionic equation, a. what types of substances should be shown as dissociated/ionized? soluble ionic compounds, acids, bases b. What types of substances should not be shown as dissociated/ionized? most molecular, insoluble ionic 2. How does electrical potential energy change between particles of like charge as the distance between them increases? As the distance between particles increases, the repulsive force (potential energy) decreases. How does electrical potential energy change between particles of opposing charge as the distance between them increases? As the distance between particles increases, the attractive force (potential energy) decreases. 3. Differentiate between an open, closed and isolated thermodynamic system. Isolated system: no exchange of heat, work, or matter with the surroundings; Closed system: exchange of heat and work, but not matter with the surroundings; Open system: exchange of heat, work and matter with the surroundings. Directions: Fill in the table for each of the variables. definition meaning if positive meaning if negative ΔE Change in internal energy (E f -E i ) The system is gaining energy from the environment from work or heat. The system is releasing energy to the environment from work or heat. w Work Work is being done on the system, so internal energy increases. Work is being done by the system, so internal energy decreases. q Heat Heat is being gained by the system, so internal energy increases. Heat is being lost by the system, so internal energy decreases. ΔH Change in enthalpy (H f -H i ) Enthalpy increasing products are higher in enthalpy than reactants. Enthalpy decreasing products are lower in enthalpy than reactants ΔT Change in temperature (T f -T i ) Temperature increasing. Temperature decreasing ΔV Change in volume (V f -V i ) Volume increasing. Volume decreasing 4. Describe what is happening in system where q = -51 kj and w = +25 kj. Heat is being released by the system (q is negative) and work is being done on the system (w is positive) 5. Describe what is happening in system where q = +321 kj and w = +132 kj. Heat is being added by the system (q is positive) and work is being done on the system (w is positive) 6. Define a state function. A property that depends only on the condition or "state" of the system, and not on the path used to obtain the current conditions. Energy, enthalpy, temperature, volume, pressure, and temperature are examples of state functions; heat and work are examples of non-state functions. 7. What is pressure-volume (PV) work? Pressure-volume work (or PV work) occurs when the volume V of a system changes. PV work is often measured in units of litre-atmospheres where 1L atm = J. 8. In the formula, w = -PΔV, why is PΔV a negative value? because this formula describes work at a constant pressure, if ΔV is negative (volume is shrinking) work is being done on the system (squeezing the gas) and w must be positive the negative sign makes the w value positive; if the gas is expanding it is doing work on the environment (volume is increasing) and ΔV would be positive the negative sign would make the w value negative 9. In what types of reactions would PV work require special attention? Reactions in which gas is produced or consumed, thereby changing the pressure of the system
2 10. What are the conditions of the enthalpy statement ΔH o = -117 kj? 1 atm and 25 o C 11. Why is the enthalpy of formation of an element in its standard state equal to zero? The standard enthalpy of formation of a substance is defined as the enthalpy change when 1 mol of the substance is formed from the most stable form of its elements in their standard states at a pressure of 1 atm and a temperature of 25 C. All elements in their standard states (for example, oxygen in the form of O 2,C in the form of graphite, H 2, I2, F2) have a standard enthalpy of formation of zero, because there is no change involved when they are formed from themselves. 12. Describe an endothermic reaction in terms of the reactants and products. The energy necessary to break the reactants is greater than the energy released by the products in their formation. 13. Describe an exothermic reaction in terms of the reactants and products. The energy released in the formation of the products is greater than the energy necessary to break the reactants. 14. Why is the sign of ΔH for a reaction reversed when the reaction direction is reversed? The amount of energy involved in the formation of a substance is equal but opposite in sign to the energy required to decompose the susbstance. 15. How are heat capacity and specific heat related? Different? Heat capacity and specific heat are both measures of how much energy is required to raise the temperature of a substance by 1 o C (or 1K). Specific heat applies to 1 gram of the substance as opposed to the the entire sample of the substance. 16. Why does ΔH = q for most reactions carried out in a calorimeter? ΔH = q for the conditions that a chemist usually works with: a constant pressure environment, and the system does no other work and has no other work done on it than the work of expansion. 17. How are coffee-cup calorimetry and bomb calorimetry alike? Different? Both types of calorimetry are used to determine heat flow resulting from a change to a system. They capitalize on the known heat capacity of a substance that absorbs or releases heat in the case of coffee cup calorimetry, that substance is usually water; in a bomb calorimeter, the substance is the bomb and surrounding water. Bomb calorimetry is constant volume meaning no PV work can be done since the volume of the bomb cannot change. Coffee cup calorimetry is constant pressure meaning the pressure is held constant (this is usually used when reactions are carried out in solution). 18. Why does the formula for calculating heat flow in a bomb calorimeter not include mass? In bomb calorimetry the heat capacity of the bomb is determined experimentally in order to calibrate it. The mass of the bomb is constant and incorporated into the heat capacity C cal. 19. In the bomb calorimetry formula, q = -C cal ΔT, why is C cal ΔT a negative value? The q value represents the heat of the reaction. When the temperature of the bomb increases, the ΔT is positive, and the q value must be negative as the bomb has heated due to energy being released by the reaction. The negative sign accomplishes the q rxn = -q sur that is used in coffee cup calorimetry. 20. Describe Hess Law. The total enthalpy of a reaction is independent of the reaction pathway. This means that if a reaction is carried out in a series of steps, the enthalpy change (DH) for the overall reaction will be equal to the sum of the enthalpy changes for the individual steps. 21. Define enthalpy of formation. change in enthalpy involved in forming 1 mole of a substance from its constituent elements 22. The symbol ΔH o f means standard enthalpy of formation (heat of formation at standard conditions, 1atm & 25 o C) 23. Why does standard enthalpy of formation equal zero for pure elements in their most stable form? It requires no energy to form an element in its most stable elemental form. This is sort of its natural resting position as an element.
3 Directions: Calculate each of the following in the space provided. 24. If atm L of work are done on a ml volume of gas at a constant pressure of 2.20 atm, what is the new volume of gas? w = -P V w = 357. atm L P = 2.20 atm V = w/-p = 357 atm L / atm = -162 L ( ml) V f = V i + V = 64.00mL + ( ml) = Oops. You get a negative volume of gas. This one won t work the way it is written. How about this instead: If atm L of work are done on a ml volume of gas at a constant pressure of 2.20 atm, what is the new volume of gas? w = -P V w = atm L P = 2.20 atm V = w/-p = atm L / atm = L (-16.2 ml) V f = V i + V = 64.00mL + (-16.2 ml) = 47.8 ml The volume decreases because work in being done on the volume of gas. 25. Compute the enthalpy change for the production of 17.1 g of Fe 2 O 3 using the following unbalanced equation. FeO(s) + O 2 (g) Fe 2 O 3 (s) ; H o = kj 4FeO(s) + O 2 (g) 2Fe 2 O 3 (s) ; H o = kj 17.1g? kj 17.1 g Fe 2 O 3 1 mol Fe 2 O kj g Fe 2 O 3 2 mol Fe 2 O 3 = kj 26. A 46.2-g sample of copper is heated to 95.4 C and then placed in a calorimeter containing 70.0 g water at 19.6 C. After the metal cools, the final temperature of metal and water is 21.8 C. Calculate the specific heat capacity of copper, assuming that all the heat lost by the copper is gained by the water. q = mc T First calculate the energy transferred to the water using the values for the water: q w =? m w = 70.0 g c w = J/(g o C) T i(w) = 19.6 o C T f(w) = 21.8 o C T w = 21.8 o C 19.6 o C = 2.2 o C q w = 70.0 g J/(g o C) 2.2 o C = J q m = -q w (because the water gained the energy directly and only from the metal) Calculate the specific heat of the metal using values for the metal: q m = J m m = 46.2 g c w =? T i(m) = 95.4 o C T f(m) = 21.8 o C T w = 21.8 o C 95.4 o C = o C c = q m /(m m T m ) = J / (46.2 g o C) = J/(g o C) 27. A g sample quinone (C 6 H 4 O 2 ) is burned in a bomb calorimeter that has a heat capacity of 1.56 kj/ C. The temperature of the calorimeter increases by 3.2 C. Calculate the energy of combustion of quinone in joules per gram and per mole. q rxn = -C cal ΔT
4 q rxn =? C cal = 1.56 kj/ C ΔT = 3.2 C q rxn = -(1.56 kj/ C 3.2 C) = -5.0 kj Convert kj to J: -5.0 kj = -5.0 x 10 3 J Finding q rxn per gram: -5.0 x 10 3 J / g = J/g Converting q rxn per gram to q rxn per mole: kj g C 6 H 4 O 2 g 1 mol C 6 H 4 O 2 = -2.7 x 10 6 J / mol 28. Find the H for the reaction below, given the following reactions and subsequent H values: HCl(g) + NaNO 2 (s) HNO 2 (l) + NaCl(s) ½ reverse 2 NaCl(s) + H 2 O(l) 2 HCl(g) + Na 2 O(s) ΔH = 507 kj ½ reverse NO(g) + NO 2 (g) + Na 2 O(s) 2 NaNO 2 (s) ΔH = 427 kj ½ forward NO(g) + NO 2 (g) N 2 O(g) + O 2 (g) ΔH = 43 kj ½ reverse 2 HNO 2 (l) N 2 O(g) + O 2 (g) + H 2O(l) ΔH = 34 kj HCl(g) + ½ Na 2 O(s) NaCl(s) + ½ H 2 O(l) NaNO 2 (s) ½ NO(g) + ½ NO 2 (g) + ½ Na 2 O(s) ½ NO(g) + ½ NO 2 (g) ½ N 2 O(g) + ½ O 2 (g) ½ N 2 O(g) + ½ O 2 (g) + ½ H 2 O(l) HNO 2 (l) ΔH = kj ΔH = kj ΔH = kj ΔH = - 17 kj ΔH rxn -78 kj Directions: Using a table of enthalpies of formation (like the one on page 184), calculate the following: 29. The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is: Calculate ΔH for this reaction. 3Al(s) + 3NH 4 ClO 4 (s) Al 2 O 3 (s) + AlCl 3 (s) + 3NO(g) + 6H 2 O(g) H o = [sum of enthalpies of products] [sum of enthalpies of reactants] H o = [H f (Al 2 O 3 (s)) + H f (AlCl 3 (s)) + 3 H f (NO(g)) + 6 H f (H 2 O(g))] [3 H f (NH 4 ClO 4 (s))] Using values from the worksheet 05.7: H o = [ kj kj + 3(90.4 kj) + 6( kj)] [3(-295 kj)] = kj 30. Consider the reaction: 2ClF 3 (g) + 2NH 3 (g) N 2 (g) + 6HF(g) + Cl 2 (g); ΔH = 1196 kj Calculate ΔH o f for ClF 3 (g). H o = [sum of enthalpies of products] [sum of enthalpies of reactants] H o = [6 H f (HF(g))] [2 H f (ClF 3 (g)) + 2 H f (NH 3 (g))] ΔH = kj Using values from the worksheet 05.7:
5 Let x stand in for H f (ClF 3 (g)) (We re supposed to be using ΔH to find a missing enthalpy of formation.) kj = [6( kj)] [2x + 2(-46.2 kj)] (Watch distributing the - here, especially on the 2(-46.2 kj) ) kj = kj 2x kj, solve for x x = -162 kj H o f(clf 3 ) = -162 kj
CHEM 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 informationThermochemistry is the study of the relationships between chemical reactions and energy changes involving heat.
CHEM134- F18 Dr. Al- Qaisi Chapter 06: Thermodynamics Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat. Energy is anything that has the capacity
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 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 informationThe Nature of Energy. Chapter Six: Kinetic vs. Potential Energy. Energy and Work. Temperature vs. Heat
The Nature of Energy Chapter Six: THERMOCHEMISTRY Thermodynamics is the study of energy and its transformations. Thermochemistry is the study of the relationship between chemical reactions and energy changes
More informationChapter 6 Review. Part 1: Change in Internal Energy
Chapter 6 Review This is my own personal review, this should not be the only thing used to study. You should also study using notes, PowerPoint, homework, ect. I have not seen the exam, so I cannot say
More informationEnthalpy and Internal Energy
Enthalpy and Internal Energy H or ΔH is used to symbolize enthalpy. The mathematical expression of the First Law of Thermodynamics is: ΔE = q + w, where ΔE is the change in internal energy, q is heat and
More informationEnthalpies 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 informationLearning Check. How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C?
Learning Check q = c * m * ΔT How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C? (c water =4.184 J/ C g, c iron =0.450 J/ C g) q Fe = 0.450
More informationFirst Law of Thermodynamics
Energy Energy: ability to do work or produce heat. Types of energy 1) Potential energy - energy possessed by objects due to position or arrangement of particles. Forms of potential energy - electrical,
More informationChemistry: The Central Science. Chapter 5: Thermochemistry
Chemistry: The Central Science Chapter 5: Thermochemistry Study of energy and its transformations is called thermodynamics Portion of thermodynamics that involves the relationships between chemical and
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 informationThermodynamics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Thermodynamics Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Thermodynamics is the scientific study of the interconversion of heat and other kinds of energy.
More information33. a. Heat is absorbed from the water (it gets colder) as KBr dissolves, so this is an endothermic process.
31. This is an endothermic reaction so heat must be absorbed in order to convert reactants into products. The high temperature environment of internal combustion engines provides the heat. 33. a. Heat
More informationChapter 6 Energy and Chemical Change. Brady and Senese 5th Edition
Chapter 6 Energy and Chemical Change Brady and Senese 5th Edition Index 6.1 An object has energy if it is capable of doing work 6.2 Internal energy is the total energy of an object s molecules 6.3 Heat
More informationLaw of conservation of energy: energy cannot be created or destroyed, only transferred One object to another One type of energy to another
ch6blank Page 1 Chapter 6: Thermochemistry Thermochemistry: study of the relationships between chemistry and energy Energy: capacity to do work Work:result of a force acting over a certain distance, one
More informationCh 6. Energy and Chemical Change. Brady & Senese, 5th Ed.
Ch 6. Energy and Chemical Change Brady & Senese, 5th Ed. Energy Is The Ability To Do Work Energy is the ability to do work (move mass over a distance) or transfer heat Types: kinetic and potential kinetic:
More informationThermochemistry 14.notebook. November 24, Thermochemistry. Energy the capacity to do work or produce heat. translational.
Thermochemistry Energy the capacity to do work or produce heat POTENTIAL ENERGY KINETIC ENERGY (energy of motion) "stored" bond energy TEMPERATURE and HEAT vibrational rotational translational a measure
More informationEnergy, Heat and Chemical Change
Energy, Heat and Chemical Change Chemistry 35 Fall 2000 Thermochemistry A part of Thermodynamics dealing with energy changes associated with physical and chemical reactions Why do we care? -will a reaction
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 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 informationThermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation
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 of motion:
More informationChapter 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 informationThermochemistry Notes
Name: Thermochemistry Notes I. Thermochemistry deals with the changes in energy that accompany a chemical reaction. Energy is measured in a quantity called enthalpy, represented as H. The change in energy
More informationChapter 6: Thermochemistry
Chapter 6: Thermochemistry 1. Light the Furnace: The Nature of Energy and Its Transformations a. Thermochemistry is the study of the relationships between chemistry and energy i. This means that we will
More information= (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 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 informationQuantities in Chemical Reactions
Quantities in Chemical Reactions 6-1 6.1 The Meaning of a Balanced Equation C 3 H 8(g) + 5 O 2(g) 3 CO 2(g) + 4 H 2 O (g) The balanced equation tells us: 1 molecule of propane reacts with 5 molecules of
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 informationChapter 6. Thermochemistry
Chapter 6. Thermochemistry 1 1. Terms to Know: thermodynamics thermochemistry energy kinetic energy potential energy heat heat vs. temperature work work of expanding gases work of expanding gases under
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 informationChapter 6 Thermochemistry
Chapter 6 Thermochemistry Thermochemistry Thermochemistry is a part of Thermodynamics dealing with energy changes associated with physical and chemical reactions Why do we care? - Will a reaction proceed
More informationSlide 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 informationThermochemistry: 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 informationChapter 8. Thermochemistry
Chapter 8 Thermochemistry Copyright 2001 by Harcourt, Inc. All rights reserved. Requests for permission to make copies of any part of the work should be mailed to the following address: Permissions Department,
More informationThermochemistry AP Chemistry Lecture Outline
Thermochemistry AP Chemistry Lecture Outline Name: thermodynamics: the study of energy and its transformations -- thermochemistry: the subdiscipline involving chemical reactions and energy changes Energy
More informationCHEM J-11 June /01(a)
CHEM1001 2014-J-11 June 2014 22/01(a) Combustion of 15.0 g of coal provided sufficient heat to increase the temperature of 7.5 kg of water from 286 K to 298 K. Calculate the amount of heat (in kj) absorbed
More informationAdditional Calculations: 10. How many joules are required to change the temperature of 80.0 g of water from 23.3 C to 38.8 C?
Additional Calculations: 10. How many joules are required to change the temperature of 80.0 g of water from 23.3 C to 38.8 C? q = m C T 80 g (4.18 J/gC)(38.8-23.3C) = 5183 J 11. A piece of metal weighing
More informationQuantities in Chemical Reactions
Quantities in Chemical Reactions 6-1 6.1 The Meaning of a Balanced Equation C 3 H 8(g) + 5 O 2(g) 3 CO 2(g) + 4 H 2 O (g) The balanced equation tells us: 1 molecule of propane reacts with 5 molecules of
More informationCh 9 Practice Problems
Ch 9 Practice Problems 1. One mole of an ideal gas is expanded from a volume of 1.50 L to a volume of 10.18 L against a constant external pressure of 1.03 atm. Calculate the work. (1 L atm = 101.3 J) A)
More informationCh. 17 Thermochemistry
Ch. 17 Thermochemistry 17.1 The Flow of Energy Energy Transformations Thermochemistry: study of energy changes in chemical reactions and changes in state Chemical potential energy: energy stored in bonds
More informationChapter 5 - Thermochemistry
Chapter 5 - Thermochemistry Study of energy changes that accompany chemical rx s. I) Nature of Energy Energy / Capacity to do work Mechanical Work w = F x d Heat energy - energy used to cause the temperature
More informationChapter 5 Thermochemistry. 許富銀 ( Hsu Fu-Yin)
Chapter 5 Thermochemistry 許富銀 ( Hsu Fu-Yin) 1 Thermodynamics The study of energy and its transformations is known as thermodynamics The relationships between chemical reactions and energy changes that
More informationAP* Chemistry THERMOCHEMISTRY
AP* Chemistry THERMOCHEMISTRY Terms for you to learn that will make this unit understandable: Energy (E) the ability to do work or produce heat ; the sum of all potential and kinetic energy in a system
More informationThermodynamics I. Prep Session
Thermodynamics I Prep Session Dr. John I. Gelder Department of Chemistry Oklahoma State University Stillwater, OK 74078 john.gelder@okstate.edu http://intro.chem.okstate.edu 12/5/09 1 Thermo I Prep Session
More informationAP CHEMISTRY. Unit 5 Thermochemistry. Jeff Venables Northwestern High School
AP CHEMISTRY Unit 5 Thermochemistry Jeff Venables Northwestern High School Kinetic Energy and Potential Energy Kinetic energy - the energy of motion: Ek = 1 mv 2 Potential energy - the energy an object
More informationChapter 5. Thermochemistry
Chapter 5 Thermochemistry Energy Thermodynamics Study of the relationship between heat, work, and other forms of energy Thermochemistry A branch of thermodynamics Focuses on the study of heat given off
More informationAP* Chapter 6. Thermochemistry
AP* Chapter 6 Thermochemistry Section 6.1 The Nature of Energy Energy Capacity to do work or to produce heat. Law of conservation of energy energy can be converted from one form to another but can be neither
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 informationmeasure ΔT in water to get q = q surroundings and use q system = q surroundings
example using water: Calculate the amount of energy required to heat 95.0 g of water from 22.5 C to 95.5 C. q = s m ΔT ( C (4.184 J g 1 C 1 ) (95.0 g) (73.0 = = 2.90 x 10 4 J or 29.0 kj Constant Pressure
More information5.1 Exothermic and endothermic reactions
Topic 5: Energetics 5.1 Exothermic and endothermic reactions Chemical reactions involve the breaking and making of bonds. Breaking bonds requires energy,whereas energy is given out when new bonds are formed.
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 informationChapter 6 Thermochemistry 許富銀
Chapter 6 Thermochemistry 許富銀 6.1 Chemical Hand Warmers Thermochemistry: the study of the relationships between chemistry and energy Hand warmers use the oxidation of iron as the exothermic reaction: Nature
More informationCHEMISTRY. Chapter 5 Thermochemistry
CHEMISTRY The Central Science 8 th Edition Chapter 5 Thermochemistry Dr. Kozet YAPSAKLI The Nature of Energy Kinetic and Potential Energy Potential energy can be converted into kinetic energy. E p = mgh
More informationChapter 6. Thermochemistry
Chapter 6 Thermochemistry Section 5.6 The Kinetic Molecular Theory of Gases http://www.scuc.txed.net/webpages/dmackey/files /chap06notes.pdf ..\..\..\..\..\..\Videos\AP Videos\Thermochemistry\AP
More informationThermochemistry: 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 informationChapter 6: Thermochemistry
Chapter 6: Thermochemistry Section 6.1: Introduction to Thermochemistry Thermochemistry refers to the study of heat flow or heat energy in a chemical reaction. In a study of Thermochemistry the chemical
More informationThermochemistry: Part of Thermodynamics
Thermochemistry: Part of Thermodynamics Dr. Vickie M. Williamson @vmwilliamson Student Version 1 Chemical Thermodynamics! Thermodynamics: study of the energy changes associated with physical and chemical
More informationTHERMOCHEMISTRY & DEFINITIONS
THERMOCHEMISTRY & DEFINITIONS Thermochemistry is the study of the study of relationships between chemistry and energy. All chemical changes and many physical changes involve exchange of energy with the
More informationObservations of Container. Hot Same Size. Hot Same Size. Hot Same Size. Observations of Container. Cold Expanded. Cold Expanded.
Chapter 9: Phenomena Phenomena: Below is data from three different reactions carried out with three different amounts of reactants. All reactants were carried out in expandable/contractable containers
More informationCHAPTER 16 REVIEW. Reaction Energy. SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 16 REVIEW Reaction Energy SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. For elements in their standard state, the value of H 0 f is 0. 2. The formation and decomposition
More informationChapter 6. Thermochemistry. Chapter 6. Chapter 6 Thermochemistry. Chapter 6 Thermochemistry Matter vs Energy 2/16/2016
Chapter 6 Thermochemistry Chapter 6 Chapter 6 Thermochemistry 6.1 Chemical Hand Warmers 6.2 The Nature of Energy: Key Definitions 6.3 The First Law of Thermodynamics: There is no Free Lunch 6.4 6.5 Measuring
More informationJune Which is a closed system? (A) burning candle (B) halogen lightbulb (C) hot water in a sink (D) ripening banana
June 2005 28. Which is a closed system? burning candle halogen lightbulb hot water in a sink ripening banana 29. Which involves the greatest energy change? chemical reaction nuclear reaction phase change
More informationThermochemistry. Questions to ponder. Because 4/20/14. an ice-cube? an ice-cube? Part 2: Calorimetry. But I KNOW. Q=mc T, but T=0
Thermochemistry Part 2: Calorimetry p p If you leave your keys and your chemistry book sitting in the sun on a hot summer day, which one is hotter? Why is there a difference in temperature between the
More information6.5 Hess s Law of Heat Summation. 2 Chapter 6: First Law. Slide 6-2
1/3/11 Thermochemistry: Energy Flow and Chemical Change Chapter 6 6.1 Forms of Energy and Their Interconversion 6.2 Enthalpy: Heats of Reaction and Chemical Change Thermochemistry: Energy Flow and Chemical
More information1. State in your own terms what is the first law of thermodynamics, a closed system, an isolated system, surroundings, heat, work, and energy.
Worksheet 1 1. State in your own terms what is the first law of thermodynamics, a closed system, an isolated system, surroundings, heat, work, and energy. The first law of thermodynamics is the conservation
More informationName: Class: Date: ID: A
Name: Class: _ Date: _ ID: A Chpter 17 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of these phase changes is an endothermic process? a.
More informationCHEMISTRY - TRO 4E CH.6 - THERMOCHEMISTRY.
!! www.clutchprep.com CONCEPT: ENERGY CHANGES AND ENERGY CONSERVATION is the branch of physical science concerned with heat and its transformations to and from other forms of energy. is the branch of chemistry
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 informationChapter 5: Thermochemistry
Chapter 5: Thermochemistry 1. Thermodynamics 2. Energy 3. Specific Heat 4. Enthalpy 5. Enthalpies of Reactions 6. Hess s Law 7. State Functions 8. Standard Enthalpies of Formation 9. Determining Enthalpies
More information10/23/10. Thermodynamics and Kinetics. Chemical Hand Warmers
10/23/10 CHAPTER 6 Thermochemistry 6-1 Chemical Hand Warmers Most hand warmers work by using the heat released from the slow oxidation of iron 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) The amount your hand temperature
More informationTypes of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy
Unit 7: Energy Outline Types of Energy Calorimetry q = mc T Thermochemical Equations Hess s Law Spontaneity, Entropy, Gibb s Free energy Energy Energy is the ability to do work or produce heat. The energy
More informationCHEMISTRY 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 information47 people in recitation yesterday. Expect quizzes there and in class.
Announcements 47 people in recitation yesterday. Expect quizzes there and in class. Chapter 6 Problems: 6.9, 6.11, 6.13(except c), 6.19, 6.23, 6.34, 6.38, 6.42, 6.51, 6.53, 6.54, 6.57, 6.64, 6.66, 6.69,
More informationChapter 5: Thermochemistry. Molecular Kinetic Energy -Translational energy E k, translational = 1/2mv 2 -Rotational energy 5.
Chapter 5: Thermochemistry 1. Thermodynamics 2. Energy 3. Specific Heat 4. Enthalpy 5. Enthalpies of Reactions 6. Hess s Law 7. State Functions 8. Standard Enthalpies of Formation 9. Determining Enthalpies
More informationThermochemistry Ch. 8
Definitions I. Energy (E): capacity to do work. II. Heat (q): transfer of energy from a body at a high temp. to a body at a low temp. III. Reaction perspectives: A. System: the focus. B. Surroundings:
More informationMeasuring and Expressing Enthalpy Changes. Copyright Pearson Prentice Hall. Measuring and Expressing Enthalpy Changes. Calorimetry
Measuring and Expressing Enthalpy Changes A burning match releases heat to its surroundings in all directions. How much heat does this exothermic reaction release? You will learn to measure heat flow in
More informationBrown, LeMay Ch 5 AP Chemistry Monta Vista High School
Brown, LeMay Ch 5 AP Chemistry Monta Vista High School 1 From Greek therme (heat); study of energy changes in chemical reactions Energy: capacity do work or transfer heat Joules (J), kilo joules (kj) or
More informationENTHALPY, INTERNAL ENERGY, AND CHEMICAL REACTIONS: AN OUTLINE FOR CHEM 101A
ENTHALPY, INTERNAL ENERGY, AND CHEMICAL REACTIONS: AN OUTLINE FOR CHEM 101A PART 1: KEY TERMS AND SYMBOLS IN THERMOCHEMISTRY System and surroundings When we talk about any kind of change, such as a chemical
More informationEnergy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy
THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:
More informationThermochemistry: 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 informationI. Chemical Reactions that Involve Heat
Unit 12 Energy I. Chemical Reactions that Involve Heat Thermochemistry: study of changes in heat in chemical reactions. Endothermic: absorbs heat; temp. goes down Exothermic: releases heat; temp. goes
More informationName 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 information8.6 The Thermodynamic Standard State
8.6 The Thermodynamic Standard State The value of H reported for a reaction depends on the number of moles of reactants...or how much matter is contained in the system C 3 H 8 (g) + 5O 2 (g) > 3CO 2 (g)
More informationChapter 5 Thermochemistry
Chapter 5 Thermochemistry Section 17.1 The Flow of Energy Heat and Work OBJECTIVES: Explain how energy, heat, and work are related. 2 Section 17.1 The Flow of Energy Heat and Work OBJECTIVES: Classify
More informationEnergy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy
THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:
More informationChapter 5 Thermochemistry
Chapter 5 Thermochemistry Energy -Very much a chemistry topic Every chemical change has an accompanying change of. Combustion of fossil fuels The discharging a battery Metabolism of foods If we are to
More informationChapter 6. Energy Thermodynamics
Chapter 6 Energy Thermodynamics 1 Energy is... The ability to do work. Conserved. made of heat and work. a state function. independent of the path, or how you get from point A to B. Work is a force acting
More informationExothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (l) + energy
Exothermic process is any process that gives off heat transfers thermal energy from the system to the surroundings. H 2 O (g) H 2 O (l) + energy Endothermic process is any process in which heat has to
More informationThermochemistry 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 informationChemistry. Friday, March 30 th Monday, April 9 th, 2018
Chemistry Friday, March 30 th Monday, April 9 th, 2018 Do-Now: BrainPOP: Heat 1. Write down today s FLT 2. Distinguish between exothermic and endothermic processes. 3. What is the specific heat of water?
More informationCh. 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 informationEnergy 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 informations Traditionally, we use the calorie as a unit of energy. The nutritional Calorie, Cal = 1000 cal. Kinetic Energy and Potential Energy
AP Chemistry: Thermochemistry Lecture Outline 5.1 The Nature of Energy Thermodynamics is the study of energy and its transformations. Thermochemistry is the study of the relationships between chemical
More informationEnthalpy of Formation of Ammonium Chloride Version 6.2.5
Enthalpy of Formation of Ammonium Chloride Version 6.2.5 Michael J. Vitarelli Jr. Department of Chemistry and Chemical Biology Rutgers University, 60 Taylor Road, Piscataway, NJ 08854 I. INTRODUCTION Enthalpy
More informationChemistry 123: Physical and Organic Chemistry Topic 2: Thermochemistry
Topic 2: Introduction, Topic 2: Thermochemistry Text: Chapter 7 and 19 (~ 3 weeks) 2.0 Introduction, terminology and scope 2.1 Enthalapy and Energy Change in a chemical process; 1st law of Thermodynamics
More informationChemistry Chapter 16. Reaction Energy
Chemistry Reaction Energy Section 16.1.I Thermochemistry Objectives Define temperature and state the units in which it is measured. Define heat and state its units. Perform specific-heat calculations.
More informationLecture Presentation. Chapter 5. Thermochemistry Pearson Education, Inc.
Lecture Presentation Chapter 5 Energy Energy is the ability to do work or transfer heat. Energy used to cause an object that has mass to move is called work. Energy used to cause the temperature of an
More informationName SUNY Chemistry Practice Test: Chapter 5
Name SUNY Chemistry Practice Test: Chapter 5 Multiple Choice 1. 1... 3. 3. 4. 4. 5. 6. 7. 8. 9. 10. 11. 1. 13. 14. 15. 16. 17. 18. 19. 0. 1 1) Calculate the kinetic energy in joules of an automobile weighing
More informationChapter 8 Thermochemistry
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 8 Thermochemistry Edward J. Neth University of Connecticut Outline 1. Principles of heat flow 2. Measurement
More information