10/23/10. Thermodynamics and Kinetics. Chemical Hand Warmers

Size: px
Start display at page:

Download "10/23/10. Thermodynamics and Kinetics. Chemical Hand Warmers"

Transcription

1 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 rises depends on several factors the size of the hand warmer the size of your glove, etc. mainly, the amount of heat released by the reaction 6-2 Thermodynamics and Kinetics SiO2 --x--> Si + O2 Diamond ---> graphite Rusting is slow 6-3 1

2 Chemistry & Energy 6-4 Chemistry and Energy H 2 /O 2 Fuel Cell 6-5 Thermodynamics is the study of heat and its transformations. Thermochemistry is a branch of thermodynamics that deals with the heat involved with chemical and physical changes. Fundamental premise When energy is transferred from one object to another, it appears as work and/or as heat. For our work we must define a system to study; everything else then becomes the surroundings. The system is composed of particles with their own internal energies (E or U). Therefore the system has an internal energy. When a change occurs, the internal energy changes

3 A chemical system and its surroundings. the surroundings the system 6-7 Figure 6.1 Energy diagrams for the transfer of internal energy (E) between a system and its surroundings. E tot = E pot + E kinetic ΔE = E final - E initial = E products - E reactants 6-8 Figure 6.2 Energy and Work 6-9 3

4 Forms of Energy Electrical kinetic energy associated with the flow of electrical charge Heat or thermal energy kinetic energy associated with molecular motion Light or radiant energy kinetic energy associated with energy transitions in an atom Nuclear potential energy in the nucleus of atoms Chemical potential energy due to the structure of the atoms, the attachment between atoms, the atoms positions relative to each other in the molecule, or the molecules, relative positions in the structure Manifestations of Energy Example of Work Heat transfers from surroundings to system in endothermic process

5 Molecular Picture of Process CO 2 (s, -78 o C) ---> CO 2 (g, -78 o C) A regular array of molecules in a solid -----> gas phase molecules. Gas molecules have higher kinetic energy Table 6.1 The Sign Conventions* for q, w and ΔE q + w = ΔE depends on sizes of q and w depends on sizes of q and w - * For q: + means system gains heat; - means system loses heat. * For w: + means word done on system; - means work done by system Units of Energy The amount of kinetic energy an object has is directly proportional to its mass and velocity KE = ½mv

6 Units of Energy 6-16 State Functions Two different paths for the energy change of a system Figure 6.6 State Function You can travel either of two trails to reach the top of the mountain. One is long and winding, the other is shorter but steep. Regardless of which trail you take, when you reach the top you will be 10,000 ft above the base. The distance from the base to the peak of the mountain is a state function. It depends only on the difference in elevation between the base and the peak, not on how you arrive there!

7 Pressure-volume work. Figure Specific Heat Capacity and Measurement of Heats of Reactions Specific heat capacity = heat lost or gained by substance (J) (mass, g)(t change, K) q = C spc x mass x ΔT 6-20 Table 6.2 Specific Heat Capacities of Some Elements, Compounds, and Materials (at 298 K) Substance Specific Heat Capacity (J/g*K) Substance Specific Heat Capacity (J/g*K) Elements aluminum, Al graphite,c iron, Fe copper, Cu gold, Au Solid materials wood cement glass granite steel Compounds water, H 2 O(l) ethyl alcohol, C 2 H 5 OH(l) ethylene glycol, (CH 2 OH) 2 (l) carbon tetrachloride, CCl 4 (l)

8 Finding the Quantity of Heat from Specific Heat Capacity PROBLEM: q = C spc x mass x ΔT 6-22 Coffee-cup calorimeter. -q sys = -q H2O -(C s x mass s x ΔT s = -(C H2O x mass H2O x ΔT H2O ) C s = C H2O x mass H2O x ΔT H2O mass s x ΔT H2O 6-23 Figure 6.9 Enthalpy w

9 The Meaning of Enthalpy w = - PΔV H = E + PV where H is enthalpy ΔH = ΔE + PΔV q p = ΔE + PΔV = ΔH ΔH ΔE in 1. Reactions that do not involve gases. 2. Reactions in which the number of moles of gas does not change. 3. Reactions in which the number of moles of gas does change but q is >>> PΔV Enthalpy diagrams for exothermic and endothermic processes. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) H 2 O(s) H 2 O(l) CH 4 + 2O 2 H initial H 2 O(l) H final Enthalpy, H Enthalpy, H ΔH < 0 heat out ΔH > 0 heat in CO 2 + 2H 2 O H final H 2 O(s) H initial A Exothermic process B Endothermic process 6-26 Figure 6.8 Some Important Types of Enthalpy Change heat of combustion (ΔH comb ) C 4 H 10 (l) + 13/2O 2 (g) 4CO 2 (g) + 5H 2 O(g) heat of formation (ΔH f ) K(s) + 1/2Br 2 (l) KBr(s) heat of fusion (ΔH fus ) NaCl(s) NaCl(l) heat of vaporization (ΔH vap ) C 6 H 6 (l) C 6 H 6 (g)

10 Enthalpy of Reaction The enthalpy change in a chemical reaction is an extensive property the more reactants you use, the larger the enthalpy change By convention, we calculate the enthalpy change for the number of moles of reactants in the reaction as written C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g) ΔH = 2044 kj Relationships Involving ΔH rxn When reaction is multiplied by a factor, ΔH rxn is multiplied by that factor because ΔH rxn is extensive C(s) + O 2 (g) CO 2 (g) ΔH = kj 2 C(s) + 2 O 2 (g) 2 CO 2 (g) ΔH = 2( kj) = kj If a reaction is reversed, then the sign of ΔH is changed CO 2 (g) C(s) + O 2 (g) ΔH = kj Sample Problem 6.4 Determining the Heat of a Reaction PROBLEM: 50.0 ml of M NaOH is placed in a coffee-cup calorimeter at o C and carefully add 25.0 ml of M HCl, also at o C. After stirring, the final temperature is o C. Calculate q soln (in J) and ΔH rxn (in kj/mol). d = 1.00 g/ml and c = J/g*K PLAN: SOLUTION: Use volumes and density to find the mass of the water. Calculate the moles of NaOH and HCl. Write balanced equations and determine the limiting reactant. Calculate q soln using the mass, c, and ΔT and finally dividing by of water gives the heat per mole. Mass( ) ml x 1.00 g/ml= 75.0 g of water ΔT = ( ) o C = 2.21 o C = 2.21 K HCl(aq) + NaOH(aq) H + (aq) + OH - (aq) H 2 O(l) NaCl(aq) + H 2 O(l) NaOH M x L = mol OH - HCl M x L = mol H + HCl is the limiting reactant, so mol H 2 O q = mass x specific heat x ΔT = 75.0 g x J/g*K x 2.21 K = 693 J (693 J/ mol H 2 O)(kJ/10 3 J) = 55.4 kj/ mol H 2 O formed 10

11 Heating/Cooling Curve for Water" Isothermal Titration Calorimetry

12 Figure 6.11 Summary of the relationship between amount (mol) of substance and the heat (kj) transferred during a reaction Sample Problem 6.6 Using the Heat of Reaction (ΔH rxn ) to Find Amounts PROBLEM: The major source of aluminum in the world is bauxite (mostly aluminum oxide). Its thermal decomposition can be represented by Al 2 O 3 (s) 2Al(s) + 3/2O 2 (g) ΔH rxn = 1676 kj If aluminum is produced this way, how many grams of aluminum can form when 1.000x10 3 kj of heat is transferred? PLAN: heat (kj) 1676 kj = 2 mol Al mol of Al x M g of Al SOLUTION: 1.000x10 3 kj x 2 mol Al 1676 kj g Al 1 mol Al = g Al 6-35 Hess's Law The enthalpy change of an overall process is the sum of the enthalpy changes of its individual steps. 1/2 O 2 (g) + C(s) CO(g) CO(g) + 1/2 O 2 (g) CO 2 (g) O 2 (g) + C(s) CO 2 (g) net reaction

13 Hess's Law S(s) + 3/2 O 2 (g) ΔH 3 = kj ΔH 1 = kj S(s) + O 2 (g) SO 2 (g) 2SO 2 (g) + O 2 (g) 1/2 (ΔH 2 = kj ) 1/2 ( 2SO 2 (g) + O 2 (g) 2SO 3 (g) ) SO 3 (g) 6-37 S(s) + 3/2 O 2 (g) SO 3 (g) Practice Hess s Law Given the following information: Cu(s) + Cl 2 (g) CuCl 2 (s) ΔH = 206 kj 2 Cu(s) + Cl 2 (g) 2 CuCl(s) ΔH = 36 kj Calculate the ΔH for the reaction below: Cu(s) + CuCl 2 (s) 2 CuCl(s) ΔH =? kj Sample Problem 6.7 Using Hess s Law to Calculate an Unknown ΔH PROBLEM: PLAN: SOLUTION: 6-39 Two gaseous pollutants that form in auto exhaust are CO and NO. An environmental chemist is studying ways to convert them to less harmful gases through the following equation: CO(g) + NO(g) CO 2 (g) + 1/2N 2 (g) ΔH =? Given the following information, calculate the unknown ΔH: Equation A: CO(g) + 1/2O 2 (g) Equation B: N 2 (g) + O 2 (g) CO 2 (g) ΔH A = kj 2NO(g) ΔH B = kj Equations A and B have to be manipulated by reversal and/or multiplication by factors in order to sum to the first, or target, equation. Multiply Equation B by 1/2 and reverse it. CO(g) + 1/2O 2 (g) NO(g) CO(g) + NO(g) CO 2 (g) 1/2N 2 (g) + 1/2O 2 (g) CO 2 (g) + 1/2N 2 (g) ΔH A = kj ½ ΔH B = ½ ( kj) = kj ΔH rxn = kj 13

14 Standard Conditions The standard state is the state of a material at a defined set of conditions pure gas at exactly 1 atm pressure pure solid or liquid in its most stable form at exactly 1 atm pressure and temperature of interest usually 25 C substance in a solution with concentration 1 M The standard enthalpy change, ΔH, is the enthalpy change when all reactants and products are in their standard states The standard enthalpy of formation, ΔH f, is the enthalpy change for the reaction forming 1 mole of a pure compound from its constituent elements the elements must be in their standard states the ΔH f for a pure element in its standard state = 0 kj/mol by definition Table 6.3 Selected Standard Heats of Formation at 25 o C (298K) 6-41 Formula Calcium Ca(s) CaO(s) CaCO 3 (s) Carbon C(graphite) C(diamond) CO(g) CO 2 (g) CH 4 (g) CH 3 OH(l) HCN(g) CS s (l) Chlorine Cl(g) ΔH 0 f (kj/mol) Formula Cl 2 (g) HCl(g) Hydrogen H(g) H 2 (g) Nitrogen N 2 (g) NH 3 (g) NO(g) Oxygen O 2 (g) O 3 (g) H 2 O(g) H 2 O(l) ΔH 0 f (kj/mol) Formula ΔH 0 f (kj/mol) Silver Ag(s) AgCl(s) Sodium Na(s) Na(g) NaCl(s) Sulfur S 8 (rhombic) 0 S 8 (monoclinic) 0.3 SO 2 (g) SO 3 (g) Formation Reactions Reactions of elements in their standard state to form 1 mole of a pure compound if you are not sure what the standard state of an element is, find the form in Appendix IIB that has a ΔH f = 0 because the definition requires 1 mole of compound be made, the coefficients of the reactants may be fractions

15 Writing Formation Reactions Write the Formation Reaction for CO(g) The formation reaction is the reaction between the elements in the compound, which are C and O C + O CO(g) The elements must be in their standard state there are several forms of solid C, but the one with ΔH f = 0 is graphite oxygen s standard state is the diatomic gas C(s, graphite) + O 2 (g) CO(g) The equation must be balanced, but the coefficient of the product compound must be 1 use whatever coefficient in front of the reactants is necessary to make the atoms on both sides equal without changing the product coefficient C(s, graphite) + 43 ½ O 2 (g) CO(g) 6-43 Sample Problem 6.8 Writing Formation Equations PROBLEM: PLAN: SOLUTION: Write balanced equations for the formation of 1 mol of the following compounds from their elements in their standard states and include ΔH 0 f. (a) Silver chloride, AgCl, a solid at standard conditions. (b) Calcium carbonate, CaCO 3, a solid at standard conditions. (c) Hydrogen cyanide, HCN, a gas at standard conditions. Use the table of heats of formation for values. (a) Ag(s) + 1/2Cl 2 (g) AgCl(s) (b) Ca(s) + C(graphite) + 3/2O 2 (g) (c) 1/2H 2 (g) + C(graphite) + 1/2N 2 (g) CaCO 3 (s) HCN(g) ΔH o f = kj ΔH o f = kj ΔH o f = 135 kj 6-44 Calculating Standard Enthalpy Change for a Reaction Any reaction can be written as the sum of formation reactions (or the reverse of formation reactions) for the reactants and products The ΔH for the reaction is then the sum of the ΔH f for the component reactions ΔH reaction = Σ n ΔH f (products) Σ n ΔH f (reactants) Σ means sum n is the coefficient of the reaction

16 Example: Calculate the enthalpy change in the reaction 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O(l) 1. Write formation reactions for each compound and determine the ΔH f for each 2 C(s, gr) + H 2 (g) C 2 H 2 (g) ΔH f = kj/mol C(s, gr) + O 2 (g) CO 2 (g) ΔH f = kj/mol H 2 (g) + ½ O 2 (g) H 2 O(l) ΔH f = kj/mol Example of ΔH o rxn from ΔH o f TiCl 4 (l) + 2H 2 O(g) TiO 2 (s) + 4HCl(g) TiCl4(l) Ti(s) + 2Cl 2 (g) -ΔH o f[ticl 4 (l)] 2H2O(g) 2H2(g) + O2(g) -2ΔH o f[h 2 O(g)] Ti(s) + O2(g) TiO 2 (s) ΔH o f[ti2o2(s)] 2H2(g) + 2Cl2(g) 4HCl(g) 4ΔH o f[hcl(g)] TiCl 4 (l) + 2H 2 O(g) TiO 2 (s) + 4HCl(g) net reaction 6-47 Figure 6.12 The general process for determining ΔH o rxn from ΔHo f values. Elements Enthalpy, H Reactants decomposition -ΔH o f formation ΔH o f H initial ΔH o rxn Products H final ΔH o rxn = Σ mδho f(products) - Σ nδho f(reactants)

17 Sample Problem 6.9 Formation PROBLEM: Nitric acid, whose worldwide annual production is about 8 billion kilograms, is used to make many products, including fertilizer, dyes, and explosives. The first step in the industrial production process is the oxidation of ammonia: 4NH 3 (g) + 5O 2 (g) Calculating the Heat of Reaction from Heats of Calculate ΔH o rxn from ΔHo f values. 4NO(g) + 6H 2 O(g) PLAN: Look up the ΔH o f values and use Hess s Law to find ΔH rxn. SOLUTION: ΔH rxn = Σ mδh o f (products) - Σ nδho f (reactants) ΔH rxn = [4(ΔH o f NO(g) + 6(ΔHo f H 2 O(g)] - [4(ΔHo f NH 3 (g) + 5(ΔHo f O 2 (g)] = (4 mol)(90.3 kj/mol) + (6 mol)( kj/mol) - [(4 mol)(-45.9 kj/mol) + (5 mol)(0 kj/mol)] ΔH rxn = -906 kj

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

6.5 Hess s Law of Heat Summation. 2 Chapter 6: First Law. Slide 6-2

6.5 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 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

Definitions and Basic Concepts

Definitions and Basic Concepts Chemical Thermodynamics: Energy Changes in Chemical Systems Conversion of energy from one form to another Transfer of energy from one place to another Why do we care about Thermodynamics? Practical applications:

More information

Learning 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. 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 information

Chapter 6 Thermochemistry: Energy Flow and Chemical Change

Chapter 6 Thermochemistry: Energy Flow and Chemical Change Chapter 6 Thermochemistry: Energy Flow and Chemical Change 6.1 Forms of Energy and Their Interconversion 6.2 Enthalpy: Heats of Reaction and Chemical Change 6.3 Calorimetry: Laboratory Measurement of Heats

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

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

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

33. a. Heat is absorbed from the water (it gets colder) as KBr dissolves, so this is an endothermic process.

33. 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 information

Thermodynamics I. Prep Session

Thermodynamics 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 information

Chapter 6 Energy and Chemical Change. Brady and Senese 5th Edition

Chapter 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 information

Thermochemistry: Part of Thermodynamics

Thermochemistry: 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 information

1 A reaction that is spontaneous.

1 A reaction that is spontaneous. Slide 1 / 55 1 A reaction that is spontaneous. A B C D E is very rapid will proceed without outside intervention is also spontaneous in the reverse direction has an equilibrium position that lies far to

More information

Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat.

Thermochemistry 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 information

Chapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics

Chapter 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 information

Thermochemistry Chapter 4

Thermochemistry 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 information

Enthalpy and Internal Energy

Enthalpy 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 information

Lecture Presentation. Chapter 6. Thermochemistry. Sherril Soman Grand Valley State University Pearson Education, Inc.

Lecture 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 information

Chapter 5. Thermochemistry

Chapter 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 information

CHEMISTRY - TRO 4E CH.6 - THERMOCHEMISTRY.

CHEMISTRY - 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 information

_ + Units of Energy. Energy in Thermochemistry. Thermochemistry. Energy flow between system and surroundings. 100º C heat 50º C

_ + Units of Energy. Energy in Thermochemistry. Thermochemistry. Energy flow between system and surroundings. 100º C heat 50º C Units of Energy Like we saw with pressure, many different units are used throughout the world for energy. SI unit for energy 1kg m 1J = 2 s 2 Joule (J) calorie (cal) erg (erg) electron volts (ev) British

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

Most hand warmers work by using the heat released from the slow oxidation of iron: The amount your hand temperature rises depends on several factors:

Most 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 information

Thermochemistry deals with the heat involved in chemical and physical changes. 2 H2(g) + O2(g) 2 H2O(g) + energy. Two types of energy

Thermochemistry deals with the heat involved in chemical and physical changes. 2 H2(g) + O2(g) 2 H2O(g) + energy. Two types of energy All course materials, including lectures, class notes, quizzes, exams, handouts, presentations, and other materials provided to students or this course are protected intellectual property. As such, the

More information

10/1/ st Law of Thermodynamics (Law of Conservation of Energy) & Hess s Law. Learning Targets

10/1/ st Law of Thermodynamics (Law of Conservation of Energy) & Hess s Law. Learning Targets 1 st Law of Thermodynamics (Law of Conservation of Energy) & Hess s Law 1 Learning Targets LT 5.02: I can relate temperature to the motions of particles and average kinetic energy. LT 5.03: I can generate

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

Chapter 6. Thermochemistry: Energy Flow and Chemical Change

Chapter 6. Thermochemistry: Energy Flow and Chemical Change Chapter 6 Thermochemistry: Energy Flow and Chemical Change Thermochemistry involves the monitoring of energy transformations that occur with a chemical reaction. CH4(g) + 2 O2 ==> CO2 + 2 H2O + HEAT Reaction

More information

Ch 6. Energy and Chemical Change. Brady & Senese, 5th Ed.

Ch 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 information

Thermochemical Equations

Thermochemical Equations Assignment There are two correct answers for #9 on the exam choice b and c. If you have one of these and it is marked wrong--submit your exam and get 6 points. Thermochemical Equations 1. The stoichiometric

More information

Chapter 8. Thermochemistry 강의개요. 8.1 Principles of Heat Flow. 2) Magnitude of Heat Flow. 1) State Properties. Basic concepts : study of heat flow

Chapter 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 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

Thermochemistry Notes

Thermochemistry 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 information

Chapter 6. Thermochemistry

Chapter 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 information

Selected Questions on Chapter 5 Thermochemistry

Selected Questions on Chapter 5 Thermochemistry Selected Questions on Chapter 5 Thermochemistry Circle the correct answer: 1) At what velocity (m/s) must a 20.0 g object be moving in order to possess a kinetic energy of 1.00 J? A) 1.00 B) 100 10 2 C)

More information

Thermodynamics. 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 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 information

Chapter 6 Thermochemistry

Chapter 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 information

First Law of Thermodynamics: energy cannot be created or destroyed.

First 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 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

47 people in recitation yesterday. Expect quizzes there and in class.

47 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 information

Thermochemistry. Chapter 6. Dec 19 8:52 AM. Thermochemistry. Energy: The capacity to do work or to produce heat

Thermochemistry. 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 information

Name Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS

Name Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS SOLUTIONS Practice Problems In your notebook, solve the following problems. SECTION 16.1 PROPERTIES OF SOLUTIONS 1. The solubility of CO 2 in water at 1.22 atm is 0.54 g/l. What is the solubility of carbon

More information

Chemical Thermodynamics. Chemical Thermodynamics. Changes of State. Chemical Thermodynamics. State Functions. State Functions 11/25/13

Chemical Thermodynamics. Chemical Thermodynamics. Changes of State. Chemical Thermodynamics. State Functions. State Functions 11/25/13 Chemical Thermodynamics n Thermodynamics is the study of the energetics and order of a system. n A system is the thing we want to study it can be a chemical reaction, a solution, an automobile, or the

More information

AP Chapter 6: Thermochemistry Name

AP 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 information

Chapter 11 Thermochemistry Heat and Chemical Change

Chapter 11 Thermochemistry Heat and Chemical Change Chemistry/ PEP Name: Date: Chapter 11 Thermochemistry Heat and Chemical Change Chapter 11:1 35, 57, 60, 61, 71 Section 11.1 The Flow of Energy - Heat 1. When 435 of heat is added to 3.4 g of olive oil

More information

Chemical Thermodynamics

Chemical Thermodynamics Quiz A 42.8 ml solution of ammonia (NH 3 ) is titrated with a solution of 0.9713 M hydrochloric acid. The initial reading on the buret containing the HCl was 47.13 ml and the final reading when the endpoint

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

Law of conservation of energy: energy cannot be created or destroyed, only transferred One object to another One type of energy to another

Law 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 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

THE ENERGY OF THE UNIVERSE IS CONSTANT.

THE ENERGY OF THE UNIVERSE IS CONSTANT. Chapter 6 Thermochemistry.notebook Chapter 6: Thermochemistry Jan 29 1:37 PM 6.1 The Nature of Energy Thermodynamics: The study of energy and its interconversions Energy: the capacity to do work or to

More information

Chemistry 30: Thermochemistry. Practice Problems

Chemistry 30: Thermochemistry. Practice Problems Name: Period: Chemistry 30: Thermochemistry Practice Problems Date: Heat and Temperature 1. Pretend you are doing a scientific study on the planet Earth. a. Name three things in the system you are studying.

More information

Chemistry 400: General Chemistry Miller Exam II November 4, 2015 Approximately 150 points

Chemistry 400: General Chemistry Miller Exam II November 4, 2015 Approximately 150 points Chemistry 400: General Chemistry Name: Miller Exam II November 4, 2015 Approximately 150 points Please answer each of the following questions to the best of your ability. If you wish to receive partial

More information

Lecture outline: Chapter 5

Lecture outline: Chapter 5 Lecture outline: Chapter 5 1. The nature of energy Thermochemistryh 2. First law of thermodynamics 3. Enthalpies of reaction 4. Hess law 5. Enthalpies of formation 1 Chemical Reactivity (1) Does a chemical

More information

CHEM 1105 S10 March 11 & 14, 2014

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 information

Chapter 5 Practice Multiple Choice & Free

Chapter 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

The Nature of Energy. Chapter Six: Kinetic vs. Potential Energy. Energy and Work. Temperature vs. Heat

The 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 information

Study Guide Chapter 5

Study Guide Chapter 5 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

More information

Chapter 6. Thermochemistry

Chapter 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 information

Thermochemistry: Energy Flow and Chemical Reactions

Thermochemistry: Energy Flow and Chemical Reactions Thermochemistry: Energy Flow and Chemical Reactions Enthalpy of Formation formation = f = enthalpy associated with the formation of a compound from its constituent elements Examples of formation equations:

More information

Energy. Different types of energy exist (heat, potential, kinetic, chemical, nuclear etc.)

Energy. Different types of energy exist (heat, potential, kinetic, chemical, nuclear etc.) Change in Energy Energy Different types of energy exist (heat, potential, kinetic, chemical, nuclear etc.) Heat - the energy transferred between objects that are at different temperatures. Unit of heat

More information

Observations of Container. Hot Same Size. Hot Same Size. Hot Same Size. Observations of Container. Cold Expanded. Cold Expanded.

Observations 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 information

Chapter 8 Thermochemistry: Chemical Energy

Chapter 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 information

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

Thermochemistry. 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 information

THERMOCHEMISTRY & DEFINITIONS

THERMOCHEMISTRY & 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 information

Homework 11 - Second Law & Free Energy

Homework 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 information

Chapter 5 Thermochemistry

Chapter 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 information

Thermochemistry 14.notebook. November 24, Thermochemistry. Energy the capacity to do work or produce heat. translational.

Thermochemistry 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 information

Unit 7 Thermochemistry Chemistry 020, R. R. Martin

Unit 7 Thermochemistry Chemistry 020, R. R. Martin Unit 7 Thermochemistry Chemistry 020, R. R. Martin 1. Thermochemistry Heat is a form of energy - which may take many forms: - Kinetic energy due to motion, ½ mv 2 - Potential energy due to position - Electrical

More information

Chapter 6. Heat Flow

Chapter 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 information

(for tutoring, homework help, or help with online classes) 1.

(for tutoring, homework help, or help with online classes) 1. www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. 2. Consider the following processes used to produce energy. Which does not predominantly use potential energy? 1. Fossil

More information

Chapter 5 Thermochemistry. 許富銀 ( Hsu Fu-Yin)

Chapter 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 information

June Which is a closed system? (A) burning candle (B) halogen lightbulb (C) hot water in a sink (D) ripening banana

June 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 information

Chapter 8. Thermochemistry

Chapter 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 information

The Nature of Energy Energy is the ability to do work or produce Heat, q or Q, is ; flows due to temperature differences (always to )

The Nature of Energy Energy is the ability to do work or produce Heat, q or Q, is ; flows due to temperature differences (always to ) CP Chapter 17 Thermochemistry 2014-2015 Thermochemistry Thermochemistry is the study of energy that occur during chemical and physical changes (changes of state) The Nature of Energy Energy is the ability

More information

Brown, LeMay Ch 5 AP Chemistry Monta Vista High School

Brown, 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 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

Solution: 1) Energy lost by the hot water: q = m C p ΔT. q = (72.55 g) (4.184 J/g 1 C 1 ) (24.3 C) q = J. 2) Energy gained by the cold water:

Solution: 1) Energy lost by the hot water: q = m C p ΔT. q = (72.55 g) (4.184 J/g 1 C 1 ) (24.3 C) q = J. 2) Energy gained by the cold water: A calorimeter is to be calibrated: 72.55 g of water at 71.6 C added to a calorimeter containing 58.85 g of water at 22.4 C. After stirring and waiting for the system to equilibrate, the final temperature

More information

Chapter 5: Thermochemistry. Molecular Kinetic Energy -Translational energy E k, translational = 1/2mv 2 -Rotational energy 5.

Chapter 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 information

05_T03. TABLE 5.3 Standard Enthalpies of Formation, H f, at 298 K. Hydrogen iodide HI(g) Silver chloride AgCl(s) Methanol

05_T03. TABLE 5.3 Standard Enthalpies of Formation, H f, at 298 K. Hydrogen iodide HI(g) Silver chloride AgCl(s) Methanol TABLE 5.3 Standard Enthalpies of Formation, H f, at 298 K H f H f Substance Formula ( kj/mol ) Substance Formula ( kj/mol ) Acetylene C 2 H 2 (g) 226.7 Hydrogen chloride HCl(g) -92.30 Ammonia NH 3 (g)

More information

Midterm Examination 2

Midterm Examination 2 CH 221 General Chemistry Spring 2012 Name: Midterm Examination 2 Useful Information is located on the last two pages of the Exam. Multiple Choice Questions A carton of Morton's Iodized Salt, NaCl with

More information

Chapter 5 Thermochemistry

Chapter 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 information

Chemistry: The Central Science. Chapter 5: Thermochemistry

Chemistry: 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 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

Chapter 6 Thermochemistry

Chapter 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 information

Workbook 5. Chem 1A Dr. White 1

Workbook 5. Chem 1A Dr. White 1 Chem 1A Dr. White 1 Workbook 5 5-1: Dalton s Law, KMT, Effusion/Diffusion/Real Gases 1. What is the total pressure and the partial pressure of each gas (in atm) in a mixture of 3.2 g of O 2, 1.6 g of CH

More information

Energy & Chemistry. Internal Energy (E) Energy and Chemistry. Potential Energy. Kinetic Energy. Energy and Chemical Reactions: Thermochemistry or

Energy & 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 information

1) Calculate the kinetic energy in J of an electron moving at m / s. The mass of an electron is g.

1) Calculate the kinetic energy in J of an electron moving at m / s. The mass of an electron is g. Multiple-Choice and Bimodal Questions 6 1) Calculate the kinetic energy in J of an electron moving at 6.00 m / s. The mass of 28 an electron is 9.11 g. A) 4.98 48 B) 3.28 14 C) 1.64 17 D) 2.49 48 E) 6.56

More information

Name SUNY Chemistry Practice Test: Chapter 5

Name 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 information

Chemistry Chapter 16. Reaction Energy

Chemistry 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 information

Chapter 5 - Thermochemistry

Chapter 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 information

Introduction to Thermochemistry. Thermochemistry Unit. Definition. Terminology. Terminology. Terminology 07/04/2016. Chemistry 30

Introduction 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 information

AP CHEMISTRY NOTES 4-1 THERMOCHEMISTRY: ENTHALPY AND ENTROPY

AP CHEMISTRY NOTES 4-1 THERMOCHEMISTRY: ENTHALPY AND ENTROPY AP CHEMISTRY NOTES 4-1 THERMOCHEMISTRY: ENTHALPY AND ENTROPY Reaction Rate how fast a chemical reaction occurs Collision Theory In order for a chemical reaction to occur, the following conditions must

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

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

THERMOCHEMISTRY CHAPTER 11

THERMOCHEMISTRY CHAPTER 11 THERMOCHEMISTRY CHAPTER 11 ENERGY AND HEAT nthermochemistry: The study of the energy changes that accompany chemical reactions and changes in the physical states of matter. ENERGY AND HEAT nwork: Energy

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 5: Thermochemistry

Chapter 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 information

Thermochemistry. Energy and Chemical Change

Thermochemistry. Energy and Chemical Change Thermochemistry Energy and Chemical Change Energy Energy can change for and flow, but it is always conserved. The Nature of Energy Energy the ability to do work or produce heat Potential energy Kinetic

More information

If neither volume nor pressure of the system changes, w = 0 and ΔE = q = ΔH. The change in internal energy is equal to the change in enthalpy.

If neither volume nor pressure of the system changes, w = 0 and ΔE = q = ΔH. The change in internal energy is equal to the change in enthalpy. 5 Thermochemistry Visualizing Concepts 5.1 The book s potential energy is due to the opposition of gravity by an object of mass m at a distance d above the surface of the earth. Kinetic energy is due to

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