Chapter 5 THERMO. THERMO chemistry. 5.4 Enthalpy of Reactions 5.5 Calorimetry 5.6 Hess s Law 5.7 Enthalpies of Formation
|
|
- Jeffry Sharp
- 6 years ago
- Views:
Transcription
1 Chapter 5 THERMO THERMO chemistry 5.4 Enthalpy of Reactions 5.5 Calorimetry 5.6 Hess s Law 5.7 Enthalpies of Formation
2 Chemical Equations 1 st WRITE the Chemical Equation 2 nd BALANCE the Chemical Equation 3 rd INTERPRET the Chemical Equation Now when Interpreting Chemical Equations must also include ENERGY
3 Involved in Chemical Processes Physical Process H 2 O(gas) H 2 O(liquid) + HEAT or Chemical Process CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O + HEAT
4 Chemical reactions can RELEASE when they occur CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O + HEAT or Chemical reactions can ABSORB when they occur 2 C (s) + 2 H 2 (g) + HEAT C 2 H 4 (g)
5 predict whether heat is absorbed endothermic or released exothermic by the system for : (1) An ice cube melts (2) butane is burned
6 Exo thermic and Endo thermic Processes thermic: transfers heat TO THE surroundings An exothermic process feels HOT thermic: absorbs heat FROM THE surroundings An endothermic process feels cold
7 Two (2) Ways to express heat 1. Heat can be expressed as q - or - 2. Expressed as H called Enthalpy - or - H Change in
8 Table 5.1 Sign Convention EXO thermic Heat is transferred FROM SYSTEM to the surroundings: q > 0 ; H < 0 ENDO thermic Heat is transferred FROM SURROUNDINGS to the system: q < 0 ; H > 0
9
10 System & Surroundings I. SYSTEM the portion of the universe that is singled out for study II. SURROUNDINGS everything outside the system III. CONSERVATION OF ENERGY
11 Open, Closed, & Isolated Systems
12 HEAT LOST = HEAT GAIN Something is gaining Heat While Something else looses Heat. IF YOU KNOW ONE OF THESE {Heat Lost - or - Heat Gained} THEN YOU KNOW
13 THERMO chemistry Two parts I. EXPERIMENTAL II. MATHEMATICAL
14 Energy Changes Involved With Part 1. PHYSICAL Changes a) Phase Changes b) WITHIN a Phase Part 2. CHEMICAL Changes
15 Part 1a Energy Changes Involved Physical Changes PHASE Changes Gas Liquid Solid
16
17
18 Energy Expressed In Terms of q for a Change Of State H 2 O (solid) H 2 O (liq) - Energy H 2 O(solid) H 2 O(liq) kj/mole The Sign Means Heat is Needed
19 Energy Can Also Be Expressed As A CHANGE In ENTHALPY ( H) H 2 O (solid) H 2 O (liq) - Energy H 2 O (solid) H 2 O (liq) H = kj/mole The Sign Means Heat is Needed!!!! NOTE THE SIGN CHANGE!!!!
20
21 Example 1: How much energy is needed to melt [ H 2 O (solid) H 2 O (liq) +/- Heat ] 18 grams of H 2 O at 0 o C? [The Heat of fusion of H 2 O = KJ / mole] 18 grams of water = 1.0 mole of water therefore need KJ of heat
22 Example 2: What quantity of Heat is required to vaporize 18 grams of H 2 O at 100 o C? H 2 O (liq) H 2 O (gas) +/- Heat [The Heat of vaporization = KJ / mole ] 18 grams of water = 1.0 mole of water therefore need KJ of heat
23 Part 1b [NO CHANGE IN PHASE] Energy Change WITHIN A State Gas Gas Liquid Liquid Solid Solid
24 Specific Heat Specific Heat- The heat required to raise the temperature of 1 gm of a substance by 1 o C EVERY SUBSTANCE HAS ITS OWN UNIQUE SPECIFIC HEAT (SH) For Water :S.H. = 4.18 JOULES (Grams) ( T)
25 UNIQUE SPECIFIC HEAT
26
27 Specific heat = quantity of heat transferred (grams of substance) x (temperature change)
28 How much heat energy is required to heat one pound of water from 25 o C (room temp) to its boiling point (100 o C)? LET THE UNITS SOLVE THE PROBLEM. Energy = (Specific Heat)x(grams)x(change in Temp) For Water :S.H. = 4.18 JOULES (Grams) ( T)
29 Energy required to heat one pound of water from 25 to 100 o C? Joules = Joules 4.18 C g ( ( ) o 454g (75 ) )( T ) Heat Energy = 142,329 Joules How many Significant Figures? Therefore answer is?????? Joules
30 Large beds of rocks are used in some solar-heated homes to store heat Calculate the quantity of heat absorbed by 50.0 kg of granite if the temperature increases by 12.0 C [The specific heat of granite is 0.79 J/g-K]
31 How much heat is absorbed by 50.0 kg of cement if the temperature increases 12.0 C [The specific heat of cement is 0.88 J/g-K] Let UNITS solve the problem Joules = (Specific Heat)x(grams)x(change in Temp) Joules = (0.88 J / g-k)(50.0x10 3 g)(12.0 C) Joules =
32 How much heat is absorbed by 50.0 kg of Rocks J Cement J Water J What statement can be made about specific heat in terms of substances absorbing or releasing heat?
33 Heat Flow Heat spontaneously flows from a hot object to a cold one until the temperature of the two objects are the same
34 Every substance has its own unique specific heat Use that information to identify an unknown 1. Put into a Styrofoam cup ¾ full of water a piece of hot metal 2. Measure temperature change of water
35 A 2.61 gram block of metal was heated to o C and put into an insulated cup containing g of water. The water temperature rose from to o C
36 When the Hot Metal is dropped into the cup of water HEAT Flows from the metal to the water Heat Lost by Metal = Heat Gain by Water Heat spontaneously flows from a hot object to a cold one until the temperature of the two objects are the same
37 Metal: 2.61 grams ; initial temp = 100 o C Water: grams; initial temp = o C final temp = C 1. What was the final temperature of the Metal? 2. How much energy did the water gain? 3. How much energy did the Metal lose? 4. What is the specific heat of Metal?
38 Joules Heat GAIN by Water Joules = 4.18 C g ( ( ) o 28.0g ( ) )( T ) = 173 Joules {Heat Gained by Water equals Heat LOST by Metal Metal LOST 173 Joules FOR THE METAL: 173 Joules = S.H x (2.61 g) x ( )
39 SpecificHeat = ( 173Joules 2.61g )( ) =???? WHAT WAS THE UNKNOWN METAL?
40 Review of Part 1 Energy Changes Involved With PHYSICAL Changes a) Phase Changes b) WITHIN a Phase
41 How much Energy required to heat 1.0 gram of ice at 10 o C to steam at 110 o C Ice Ice Liq Liq Gas Gas -10 o C 0 o C 0 o C 100 o C 100 o C 110 o C What information do you need to work this problem
42 Data Required for problem Heat of fusion = kj / mole Heat of vaporization = kj / mole Specific heat: Ice J / g - K Liq J / g K Steam J / g - K
43 Energy required to heat 1.0 gram of ice at 10 o C to ice at 0 o C? Heat required to melt 1.0 gram of ice? Heat required to heat 1.0 gram of water at 0 o C to water at 100 o C? Heat required to vaporize 1.0 grams of H 2 O? Heat required to heat 1.0 gram of steam at 100 o C to steam at 110 o C?
44 How much Energy required to heat 1.0 gram of ice at 10 o C to steam at 110 o C Add all the numbers 21 J kj J kj + 18 J How many significant figures in answer?
45
46 Part 2 CHEMICAL REACTIONS Reactants Products +/-ENERGY
47 Chemical reactions can release or absorb heat Energy is stored in Chemical BONDS It TAKES Energy To BREAK Bonds Energy Is RELEASED When A Bond Is Formed
48 Enthalpies of Reaction For a reaction: H = H final H initial = H products H reactants
49 HEAT OF REACTION CH O 2 CO H 2 O + HEAT The PLUS Sign Means Heat Is Given Off OR CH O 2 CO H 2 O H = - # The MINUS Sign Means Heat Is Given Off
50 DETERMINATION of HEATS of REACTIONS 1. THE DIRECT METHOD EXPERIMENTAL Use A Calorimeter 2. THE INDIRECT METHOD MATHEMATICAL Use HESS S Law
51 1. The Direct Method EXPERIMENTAL Go to Lab and Use A Calorimeter HEAT LOST = HEAT GAINED
52 Two (2) types of CALORIMETERS 1. OPEN { to the atmosphere and 2. CLOSED {to the atmosphere
53 OPEN CALORIMETER Also called a CONSTANT PRESSURE CALORIMETER Styrofoam cup
54 100 ml of 0.5 M HCl added to 100 ml of 0.5 M NaOH
55 Data Collected from experiment Volume of M NaOH(aq) = 1.00 x 10 2 ml Volume of M HCl(aq) = 1.00 x 10 2 ml Initial Temperature = o C Final Temperature = o C
56 Detemine the heat of the reaction PER MOLE (the Heat of neutralization) What GIVES OFF THE HEAT? The reaction! 1 HCl(aq) + 1 NaOH (aq) H 2 O + NaCl (aq) + HEAT What ABSORBS THE HEAT? The solution
57 How do you determine the Heat of the reaction? From the HEAT GAINED by the SOLUTION Joules = (Specific Heat) x (grams) x (Temp Change) of the solution from density from experiment
58 Number of GRAMS =? 100 ml HCl (aq) ml NaOH (aq) ml of each = ml total 2. Relationship between weight & volume? 3. DENSITY of solution 4. If Density = 1.00 g / ml 5. Have grams of solution
59 Let UNITS solve the problem Joules = (Specific Heat) x (grams) x (change in T) change in Temp =? grams = 200 grams of solution Specific Heat = Joules 4.18 gram x temp change Joules = (Specific Heat) x (grams) x (change in T) Joules = (4.184)(200)(3.42) =
60 Joules = (4.184)(200)(3.42) = kj 1 HCl(aq) + 1 NaOH (aq) H 2 O + NaCl (aq) + Heat kj of heat given off when 1.00 x 10 2 ml of M HCl (aq) is mixed with 1.00 x 10 2 ml of M NaOH (aq) How much heat given off per mole of water formed?
61 heat of neutralization per mole? How many moles of water formed? 1.00 x 10 2 ml of both M of HCl(aq) & NaOH Moles = Molarity x Volume = H + (aq) OH - (aq) 0.05 H 2 O kj 1.00 H + (aq) OH - (aq) 1.00 H 2 O +
62 Calorimeter [Used For Gas Reactions] CONSTANT VOLUME CALORIMETER It is called a BOMB CALORIMETER Because the Chemical Reaction Occurs in a CLOSED Container
63 See Text Fig 5.19 Page 186
64 Chemical Reaction takes place in Bomb HEAT IS GIVEN off by Reaction (SYSTEM) HEAT IS ABSORBED by SURROUNDINGS Surroundings are 1. WATER In Calorimeter 2. Everything else {thermometer, stirrer, metal bomb itself, etc
65 Example grams Of Mg Was Burned In a Constant Volume Calorimeter Write & Balance the COMBUSTION Reaction Mg + O MgO + HEAT 2 Heat Lost by = Heat Gain by Chemical 1. Water + Reaction 2. Calorimeter
66 Data Collected from experiment The Calorimeter had a Heat Capacity = 1769 J/ 0 C Calorimeter Contained 3.00x10 2 ml of Water Initial Temperature = 22.5 o C Final Temperature = 42.4 o C
67 1. Heat Gain by Water = S. H. x grams x Temp q water = (4.184 x 300 x 19.9 ) 2. Heat Gain by Calorimeter = Heat Cap x Temp Change q Calorimeter = (1769 x 19.9 ) Total Heat Gained = Water + Calorimeter
68 = (1769 x 19.9 ) + (4.184 x 300 x 19.9 ) = (35,203.1) + (24,978.48) Joules = Joules for grams of Mg HEAT LOST = HEAT GAIN How do you convert from grams to moles?
69 Record Data Record results in Tabular Form
70 Heats of Combustion (- H) per mole in kj at 25 o C HC 2 H 3 O 2 (aq) { Acetic Acid (aq) CH 4 (g) { Methane C 2 H 6 (g) C 6 H 6 (liq) C 6 H 12 (liq) Sucrose (s)
71 Enthalpy is an EXTENSIVE property ( H is directly proportional to amount): CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(liq) H = kj 2 CH 4 (g) + 4 O 2 (g) 2 CO 2 (g) + 4 H 2 O(liq) H = kj Phase (solid, liquid, gas) is Important CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(gas) H = kj 4 CH 4 (g) + 8 O 2 (g) 4 CO 2 (g) + 8 H 2 O(g) H = kj Note the state of water
72 Next, DETERMINATION OF HEATS OF REACTIONS Using 2. THE INDIRECT METHOD MATHEMATICAL Use Of HESS S Law
73 I. COMBUSTION of hydrocarbons CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) II. FORMATION Reactions e.g., CH 4 (Methane) C(s) + 2 H 2 (g) CH 4 (g)
74 Standard State The Standard State of a substance is the state the pure substance is in at atmospheric pressure ( 1 atm) and 25 o C The standard state of carbon is graphite and not diamond The standard state of hydrogen is H 2 not H
75 STANDARD ENTHALPIES OF FORMATION For example H 2 O (liq) is formed from its elements as they exist in nature H 2 (gas) + ½ O 2 (gas) H 2 O (liq) H = kj
76
77 STANDARD ENTHALPIES OF FORMATION THE STANDARD ENTHALPY OF FORMATION ( H f ) OF ANY ELEMENT IN ITS MOST STABLE FORM IS ZERO (BY DEFINATION)
78 HESS S LAW ENTHALPY CHANGES ARE ADDITIVE
79 Example 1 Calculate [using Hess Law] the heat of reaction for CO(g) + ½ O 2 (g) CO 2 (g) What DATA Do You Need From Table?
80 H f From Table WRITE AND BALANCE REACTIONS Formation of CO (g) is : 1. C (s) + ½ O 2 (g) CO(g) H = kj Formation of CO 2 (g) is : 2. C (s) + O 2 (g) CO 2 (g) H = kj
81 Want CO (g) + ½ O 2 (g) CO 2 (g) 1. C (s) + ½ O 2 (g) CO(g) H = kj REWRITE Eq 1 1b. CO (g) C (s) + ½ O 2 (g) H = kj also 2. C (s) + O 2 (g) CO 2 (g) H = kj
82 CO (g) C (s) + ½ O 2 (g) H = kj C (s) + O 2 (g) CO 2 (g) H = kj Add Equations To Get Reaction Wanted: CO (g) + ½ O 2 (g) CO 2 (g) Add H s To Get : H = kj kj =
83 Example 2 Find the Enthalpy of Formation of C 3 H 8 (g) Given Enthalpy of combustion of C 3 H 8 (g) = kj Enthalpy of formation of CO 2 (g) = kj Enthalpy of formation of H 2 O(g) = kj
84 Write and balance the following reactions Combustion of one mole of C 3 H 8 (g) Formation of one mole of CO 2 (g) Formation of one mole of H 2 O(g) Formation of one mole of C 3 H 8 (g) 3 C (s) +4 H 2 (g) C 3 H 8 (g) H =???
85 Example 3 Find the Enthalpy of Formation of C 3 H 8 (g) From Enthalpy of combustion of C 3 H 8 (g) = kj Enthalpy of formation of CO 2 (g) = kj Enthalpy of formation of H 2 O(g) = kj answer 3 C (s) +4 H 2 (g) C 3 H 8 (g) H = kj
86 Example 4 Find the Heat of Vaporization of Water From the following HEATS of COMBUSTION C 3 H 8 (g) + 5O 2 (g) 3CO 2 + 4H 2 O(g) C 3 H 8 (g) + 5O 2 (g) 3CO 2 + 4H 2 O(l) H = kj H = kJ NOTE: These reactions have Nothing to do with the vaporization of water
87 Want H for H 2 O (liquid) H 2 O (gas) C 3 H 8 (g) + 5O 2 (g) 3CO 2 + 4H 2 O(g) C 3 H 8 (g) + 5O 2 (g) 3CO 2 + 4H 2 O(l) H = kj H = kJ Rewrite last equation to get 3CO 2 + 4H 2 O(l) C 3 H 8 (g) + 5O 2 (g) H = kj WHY?
88 Want H for H 2 O (liquid) H 2 O (gas) C 3 H 8 (g) + 5O 2 (g) 3CO 2 + 4H 2 O(g) H = kj 3CO 2 + 4H 2 O(l) C 3 H 8 (g) + 5O 2 (g) H = kj Add Equations getting 4 H 2 O (liquid) 4 H 2 O (gas) H = kj H 2 O (liquid) H 2 O (gas) H =
89 Given the data N 2 (g) + O 2 (g) 2 NO(g) H = kj 2 NO(g) + O 2 (g) 2 NO 2 (g) H = kj 2 N 2 O(g) 2N 2 (g) + O 2 (g) H = kj Use Hess s law to calculate H For the reaction N 2 O(g) + NO 2 (g) 3 NO(g)
90 Example 4 Find H for N 2 O(g) + NO 2 (g) 3NO(g) Given N 2 (g) + O 2 (g) 2 NO(g) H = kj 2 NO(g) + O 2 (g) 2 NO 2 (g) H = kj 2 N 2 O(g) 2N 2 (g) + O 2 (g) H = kj Add The Following Equations N 2 (g) + O 2 (g) 2 NO(g) H = kj NO 2 (g) NO(g) + ½ O 2 (g) H = ½ [ kj] N 2 O(g) N 2 (g) + ½ O 2 (g) H = ½ [ kj]
91 Energy From Foods
92 Energy in our bodies comes from fats and carbohydrates (mostly) Carbohydrates converted into glucose, then: C 6 H 12 O O 2 6 CO H 2 O H = kj Fats: contain more energy; are not water soluble, so are good for energy storage. 2 C 57 H 110 O O CO H 2 O H = - 75,520 kj
93 Which releases the greatest amount of energy per gram upon metabolism (a) carbohydrates (b) proteins (c) fats
94 Energy From Fuels
95 Which releases the greatest amount of energy per gram upon combustion (a) Methane (b) gasoline (c) hydrogen
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 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 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 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 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 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 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 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 informationGravity is a force which keeps us stuck to the earth. The Electrostatic force attracts electrons to protons in an atom.
Energy Relations in Chemistry: Thermochemistry The Nature of Energy Sugar you eat is "combusted" by your body to produce CO 2 and H 2 O. During this process energy is also released. This energy is used
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 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 17 Thermochemistry
CHAPTER 17 Thermochemistry Thermochemistry The study of the heat changes that occur during chemical reactions and physical changes of state. Chemical Change: new substances created during chemical reaction
More informationName: 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 informationChapter 11. Thermochemistry. 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages
Chapter 11 Thermochemistry 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages 293-94 The Flow of energy - heat Thermochemistry concerned with the heat changes that occur
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 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 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 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 informationTopic 05 Energetics : Heat Change. IB Chemistry T05D01
Topic 05 Energetics 5.1-5.2: Heat Change IB Chemistry T05D01 5.1 Exothermic and endothermic reactions - 1 hour 5.1.1 Define the terms exothermic reaction, endothermic reaction and standard enthalpy change
More informationI. The Nature of Energy A. Energy
I. The Nature of Energy A. Energy is the ability to do work or produce heat. It exists in 2 forms: 1. Potential energy is energy due to the composition or position of an object. 2. Kinetic energy is energy
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 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 informationEnergy and Chemical Change
Energy and Chemical Change Reviewing Vocabulary Match the definition in Column A with the term in Column B. h e d p c f a r m t j i s l u k n q g o Column A 1. The ability to do work or produce heat 2.
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 informationThe 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 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 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 informationChapter 17 Thermochemistry
Chapter 17 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 informationName: General Chemistry Chapter 11 Thermochemistry- Heat and Chemical Change
Name: General Chemistry Chapter 11 Thermochemistry- Heat and Chemical Change Notepack 1 Section 11.1: The Flow of Energy Heat (Pages 293 299) 1. Define the following terms: a. Thermochemistry b. Energy
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 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 informationThermodynamics- Chapter 19 Schedule and Notes
Thermodynamics- Chapter 19 Schedule and Notes Date Topics Video cast DUE Assignment during class time One Review of thermodynamics ONE and TWO Review of thermo Wksheet Two 19.1-4; state function THREE
More 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 informationTHE 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 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 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 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 informationEnergetics. Topic
Energetics Topic 5.1 5.2 Topic 5.1 Exothermic and Endothermic Reactions?? total energy of the universe is a constant if a system loses energy, it must be gained by the surroundings, and vice versa Enthalpy
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 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 and Chemical Change
Energy and Chemical Change Section 16.1 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 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 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 informationUnit 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 information1.4 Enthalpy. What is chemical energy?
1.4 Enthalpy What is chemical energy? Chemical energy is a form of potential energy which is stored in chemical bonds. Chemical bonds are the attractive forces that bind atoms together. As a reaction takes
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 informationThermochemistry. Energy (and Thermochemistry) World of Chemistry Chapter 10. Energy. Energy
Thermochemistry Thermodynamics is the science of the relationship between heat and other forms of energy. (and Thermochemistry) World of Chemistry Chapter 10 is defined as the ability to do work or produce
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 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 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 informationSaturday Study Session 1 3 rd Class Student Handout Thermochemistry
Saturday Study Session 1 3 rd Class Student Handout Thermochemistry Multiple Choice Identify the choice that best completes the statement or answers the question. 1. C 2 H 4 (g) + 3 O 2 (g) 2 CO 2 (g)
More information2. Calculate the heat change in joules when 45.2 g of steam at C condenses to water at the same temperature.!
Chem L3 Worksheet:Thermochemistry: Chapter 11 Page 1 Water Heating Cooling curve Problems ( Stairstep ): pp. 292-325, 549-556 1. How much heat is released when 65.0 g of steam cools from 150.0 C to 130.0
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 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 informationLecture Presentation. Chapter 5. Thermochemistry. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 5 Thermochemistry John D. Bookstaver St. Charles Community College Cottleville, MO Thermochemistry Thermodynamics is the study of energy and its transformations. Thermochemistry
More informationSlide 2 / 118. Thermochemistry
Slide 1 / 118 Slide 2 / 118 Thermochemistry Slide 3 / 118 Table of Contents The Nature of Energy State Functions** Click on the topic to go to that section Enthalpy Measuring Enthalpy Changes: Calorimetry
More informationEnergy Transformations
Thermochemistry Energy Transformations Thermochemistry - concerned with heat changes that occur during chemical reactions Energy - capacity for doing work or supplying heat weightless, odorless, tasteless
More informationSample Exercise 5.1 Describing and Calculating Energy Changes
Sample Exercise 5.1 Describing and Calculating Energy Changes A bowler lifts a 5.4-kg (12-lb) bowling ball from ground level to a height of 1.6 m (5.2 feet) and then drops the ball back to the ground.
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 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 informationName 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 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 informationChapter 6. Thermochemistry
Chapter 6 Thermochemistry This chapter develops for the student the concepts of thermochemistry. Upon completion of Chapter 6, the student should be able to: 1. Define and explain the following terms:
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 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 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 informationCHAPTER 17: THERMOCHEMISTRY. Mrs. Brayfield
CHAPTER 17: THERMOCHEMISTRY Mrs. Brayfield REVIEW What is the law of conservation of energy? It states that energy cannot be created or destroyed So the energy of any process is the same THERMOCHEMISTRY
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 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 informationMr Chiasson Advanced Chemistry 12 / Chemistry 12 1 Unit B: Thermochemical Changes
Mr Chiasson Advanced Chemistry 12 / Chemistry 12 1 Unit B: Thermochemical Changes Students will be expected to: Compare the molar enthalpies of several combustion reactions involving organic compounds.
More informationLecture 0503 Calorimetry and Hess s Law
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Lecture 0503 Calorimetry and Hess s Law John D. Bookstaver St. Charles Community College Cottleville,
More informationENERGY AND ENERGETICS PART ONE Keeping Track of Energy During a Chemical Reaction
ENERGY AND ENERGETICS PART ONE Keeping Track of Energy During a Chemical Reaction ADEng. PROGRAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore
More informationI. Energy A. Terms and Definitions B. Energy Transfer as Heat C. Energy Transfer as Work D. Internal Energy
Chapter 7 1 Thermochemistry is HOT! I. Energy A. Terms and Definitions B. Energy Transfer as Heat C. Energy Transfer as Work D. Internal Energy II. Chemistry and Energy A. Enthalpy and Enthalpies of Reaction
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 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 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 informationChapter 15 Energy and Chemical Change
Chapter 15 Energy and Chemical Change Chemical reactions usually absorb or release energy. Section 1: Energy Section 2: Heat Section 3: Thermochemical Equations Section 4: Calculating Enthalpy Change Section
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 information11B, 11E Temperature and heat are related but not identical.
Thermochemistry Key Terms thermochemistry heat thermochemical equation calorimeter specific heat molar enthalpy of formation temperature enthalpy change enthalpy of combustion joule enthalpy of reaction
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 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 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 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. 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 informationClass 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 information0. Graphite is thermodynamically less stable that diamond under standard conditions. 1. True 2. False
0. Graphite is thermodynamically less stable that diamond under standard conditions. 1. True 2. False 1. Which statement would be the best interpretation of the First Law of Thermodynamics? 1. The total
More 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 informationGilbert Kirss Foster. Chapter 9. Thermochemistry. Energy Changes in Chemical Reactions
Gilbert Kirss Foster Chapter 9 Thermochemistry Energy Changes in Chemical Reactions Chapter Outline 9.1 Energy as a Reactant or Product 9.2 Transferring Heat and Doing Work 9.3 Enthalpy and Enthalpy Changes
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 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 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 information5/14/14. How can you measure the amount of heat released when a match burns?
CHEMISTRY & YOU Chapter 7 Thermochemistry How can you measure the amount of heat released when a match burns? 7. The Flow of Energy 7.3 Heat in Changes of State 7.4 Calculating Heats of Reaction Remember:
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 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 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 informationEnergy Changes in Reactions p
Energy Changes in Reactions p.126 210 Heat vs. temperature: Heat is a form of energy, it is transferred from one system to another Temperature is an indication of the intensity of heat, it measures the
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 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 information17.2 Thermochemical Equations
17.2. Thermochemical Equations www.ck12.org 17.2 Thermochemical Equations Lesson Objectives Define enthalpy, and know the conditions under which the enthalpy change in a reaction is equal to the heat absorbed
More informationSection 9: Thermodynamics and Energy
Section 9: Thermodynamics and Energy The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 9.01 Law of Conservation of Energy Chemistry (11)(A)
More information