SUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS
|
|
- Oswin Underwood
- 5 years ago
- Views:
Transcription
1 SUPPLEMENTARY TOPIC 3 ENERGY AND CHEMICAL REACTIONS Rearranging atoms. In a chemical reaction, bonds between atoms in one or more molecules (reactants) break and new bonds are formed with other atoms to produce different molecules (products). These reactions can only occur if the molecules involved collide with sufficient energy to allow the bonds to break, a process which always requires energy input. When the new bonds form as a result of the collision, energy is released. Overall, there may be a nett release of energy (EXOTHERMIC reaction) or there may be a nett requirement for energy to be supplied (ENDOTHERMIC reaction). The heat supplied by burning gas is an example of an exothermic reaction, while the production of the metal iron from its ore, iron oxide, is endothermic, the heat energy required being supplied in a blast furnace. During chemical reactions, although bonds are broken and new bonds are formed, the same atoms remain in the same quantities after the reaction as there were before. It is a fundamental law of chemistry that atoms are not created or destroyed during chemical change. For this reason, whenever a balanced chemical equation is written for a reaction, all atoms which appear on the reactants side must also appear on the products side of that equation. The following equation shows the formation of water from its elements, and includes structural formulas to emphasise the bonds broken and formed. H H + O=O + H H H O H + H O H This would of course usually be written as 2H 2 + O 2 2H 2 O. Energy changes. All molecules have energy stored in their chemical bonds. Some of this energy can be released (mostly as heat) when they react to form molecules which have less energy than the reactants, the reaction being classed as EXOTHERMIC. Alternatively, in an ENDOTHERMIC reaction, additional energy is supplied to the reactants so that the products finish up with more energy stored in their chemical bonds than the reactants had originally. The total energy stored in a collection of molecules is called the ENTHALPY of that substance (H), and for the overall reaction, the difference (enthalpy of products enthalpy of reactants) is the energy released or taken up. This enthalpy difference is given the symbol ÄH. The enthalpy change for a chemical reaction can be measured experimentally by observing the temperature change (increase or decrease) when the reaction is carried out in a thermally insulated ST3-1
2 ST3-2 container basically similar to a thermos flask. CALORIMETER. Such a container is called a As an example, the burning of carbon in oxygen releases 394 kj for each mole of carbon (12.01 g) used. This is represented by the THERMODYNAMIC EQUATION which shows the enthalpy change as well as the reactants and products and their physical states. C(s) + O 2 (g) CO 2 (g) The sign indicates the energy is released. For an endothermic reaction, a + sign is used for ÄH. ÄH = 394 kj/mol Thus for the electrolysis of water, an endothermic process, the corresponding thermodynamic equation is H 2 O(l) H 2 (g) + ½O 2 (g) ÄH = +285 kj/mol This reaction can be reversed by burning hydrogen in oxygen to produce water as a vapour which then condenses to form liquid water. The energy released by this exothermic reaction is numerically exactly the same as the energy supplied (per mole of water) in the electrolysis reaction, but with the sign reversed. Thus the process could be represented by the following thermodynamic equation H 2 (g) + ½O 2 (g) H 2 O(l) ÄH = 285 kj/mol Consider another example - the burning of methane, the main component of natural gas, to form gaseous water and carbon dioxide. This exothermic reaction releases 889 kj from each mole of methane used so the thermodynamic equation for the reaction is CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) ÄH = 889 kj/mol Energy units. There are various units used to express an amount of energy. In science, the normal unit used is the joule, abbreviated as J. Note that energy and work units are identical as these two are interchangeable - energy is expended doing work or work can be harnessed to produce energy. The use of kj per mole in the above thermodynamic equations can be somewhat confusing until one realises that the per mole part merely indicates that all quantities are expressed in moles. The actual numbers of moles of each constituent is given by the stoichiometric coefficients as written in the equation. It is customary to write the per mole as mol 1 " using the exponential notation. Thus while ÄH for the reaction equation H 2 (g) + ½O 2 (g) H 2 O(l) ÄH = 285 kj mol 1 shows that 285 kj is released for the formation of 1 mole of H 2 O,
3 ÄH for the reaction equation ST3-3 2H 2 (g) + O 2 (g) 2H 2 O(l) ÄH = 570 kj mol 1 shows that 2 ( 285) = 570 kj is released for the formation of 2 moles of H 2 O. Consequently a ÄH value for a reaction must be accompanied by the equation to which it refers. Check your understanding of this section. (a) Write a thermodynamic equation for the combustion of methane (natural gas). A typical household uses 100 megajoules each quarter on average. Calculate what mass of methane this would correspond to having been burnt. (1 megajoule = 10 6 joules) (b) Given H 2 (g) + Cl 2 (g) 2HCl(g) ÄH = 184 kj mol 1, calculate ÄH for the reaction 1 / 2 H 2 (g) + 1 / 2 Cl 2 (g) HCl(g). Activation energy: why you need a match to light the gas? Consider the reaction of hydrogen with oxygen again. A mixture of these two gases in a balloon remains indefinitely without reacting. However, application of a small amount of energy such as from a spark or a match causes the reaction to proceed instantaneously to completion, releasing the 285 kj of energy for every mole (2.0 g) of H 2 reacting. [This is the fuel mixture that was used in the Space Shuttle.] The reaction could not start without the heat supplied by the match because there is an "energy barrier" between the reactants and products. Recall that energy is always needed to break bonds, and that before any energy can be obtained through the formation of new bonds, at least some of the old bonds must be broken. This energy barrier is called the ACTIVATION ENERGY of the reaction. Apparently, in the original mixture, not enough of the hydrogen and oxygen molecules have sufficient energy when they collide for reaction to occur no matter how long one waits. By supplying the additional energy from the match to relatively few molecules, they are then able to react and in the process release energy to the remaining molecules, thereby providing the activation energy for all the remaining molecules to react, as the reaction is exothermic. This can be illustrated on an energy diagram as shown.
4 ST3-4 Check your understanding of this section. The process of charging a car battery involves some electrolysis of the sulfuric acid / water mixture in the battery. Why should one not use a match to inspect the electrolyte level in the battery? Catalysts. Catalysts are substances which, when present, reduce the activation energy for a given reaction by providing a different, lower-energy pathway, thereby causing the reaction to proceed faster. Catalysts are not consumed in the reaction, and do not give a greater final yield of products - they only make the reaction faster, thereby increasing the yield obtained in a given time. The following diagram represents the enthalpy change for a reaction with and without a catalyst present. There are many different types of catalysts. Some are simply metals which have a suitable surface on which to promote a particular reaction - eg platinum gauze can catalyse the reaction between hydrogen and oxygen. All modern motor cars have a canister containing metal catalysts in their exhaust systems to catalyse the reaction of unburnt hydrocarbons to carbon dioxide and water. The catalyst used would become "poisoned" if any lead came in contact with it, and this was the original reason why unleaded fuel was introduced, although later concern about lead levels in blood may cause one to believe that this was the reason. As replacement canisters of catalyst for cars cost about $500, it was most important not to ever allow leaded fuel to enter the petrol tank of a car requiring unleaded fuel. The elimination of leaded fuel has removed this risk.
5 ST3-5 Many industrial processes would not be feasible without the use of catalysts which allow greater yields in a given amount of time and/or allow a lower temperature to be used, thereby saving on fuel costs. The Haber synthesis, a method whereby nitrogen and hydrogen are combined to form ammonia, is responsible for about half of the nitrogen fixed on earth. This synthesis would not be feasible without the catalyst used in the industrial process. The search is currently under way to find catalysts that can lead to the commercial production of hydrogen economically enough to become a fuel for motor vehicles. Energy content of some common fuels. The following illustration shows the energy supplied by complete combustion of some common fuels. The units used are kilojoules per gram of the fuel. The chemical energy released from the fuel can be harnessed for other purposes - e.g. to do work such as in an internal combustion engine or to generate electricity which in turn can be used to do work via an electric motor. Note that the process of conversion of the original energy from the fuel into useful work is seldom even 50 % efficient. Energy and living systems. The same laws governing energy and work apply equally well to living systems (in vivo) as they do to chemical changes in test tubes (in vitro). Apart from nuclear energy, earth is ultimately dependent on energy from the sun in the form of electromagnetic radiation (EMR) in the infra-red, visible and ultra-violet frequencies. The energy carried by EMR is converted to chemical energy stored in the bonds of CARBOHYDRATES by plants through the process of PHOTOSYNTHESIS, in particular via formation of the monosaccharide called GLUCOSE as shown in the following equation. 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) ÄH = kj mol 1
6 ST3-6 Glucose and other simple carbohydrates are combined to form polymers called POLYSACCHARIDES, such as CELLULOSE and STARCH. n C 6 H 12 O 6 (C 6 H 10 O 5 ) n where n is > 1000 Cellulose provides structural strength for plant cells and starch provides a reserve store of glucose for energy requirements. The energy stored in the chemical bonds of oil, coal and natural gas represents reserves of solar energy from millions of years past, laid down at a time when the climate favoured prolific plant growth. Objectives of this Topic. After studying this Topic, you should have achieved the following goals: 1. Recognise that energy is stored in chemical bonds. 2. Know that when chemical reactions occur, energy is required to break bonds and is released when new bonds form, and that there will be an overall energy change equal to the difference between the energy stored in the bonds of the products and reactants. 3. Know that both endothermic and exothermic reactions require some energy input to initiate them - called the activation energy for that reaction. 4. Understand that the energy change for a reaction proceeding one way is identical, but of opposite sign, to the energy change for the same reaction in reverse. 5. Be able to write a thermodynamic equation and interpret the ÄH data associated with it. 6. Understand the role of catalysts in lowering the activation energy barrier by providing an alternative pathway for the reaction. 7. Know that energy can be obtained from fuels and foods substances which undergo exothermic reactions and that the energy released can in part be made to do work or support living systems.
7 XVI - 7 SUMMARY. Chemical reactions involve the breaking of existing bonds in the reactants and the forming of new bonds in the products. These changes are accompanied by energy changes - exothermic if there is a nett release of energy and endothermic if there is a nett gain of energy by the components of the reaction. The total energy stored in a collection of molecules is called its enthalpy and is given the symbol H. When a reaction occurs, the total energy change is represented as ÄH. If the reaction is exothermic, the enthalpy change is given a negative sign while if the reaction is endothermic, absorbing energy, the enthalpy change is given a positive sign. The energy change for a reaction going in the forward direction has the same magnitude as that for the reaction going in the reverse direction. An equation which shows the reactants and their physical states as well as the accompanying enthalpy change is called a thermodynamic equation. Reacting molecules must collide with enough energy to break bonds (always an endothermic process) before any energy can be obtained from the formation of new bonds (always exothermic). Consequently every reaction always has an activation energy requirement which must be supplied before the reaction can proceed. This activation energy barrier can be lowered by substances called catalysts which provide an alternative reaction pathway. They are not consumed in the reaction but merely allow it to proceed much more rapidly. Energy derivable from fuel and foods can be used to do work or to allow living systems to function. Recommended follow up chemcal modules: Section: General Chemistry Module: Chemical Energy and Calorimetry Topics covered: Chemical energy; calorimetry; enthalpy; Hess's law; bond enthalpies. TUTORIAL QUESTIONS - SUPPLEMENTARY TOPIC What is meant by the terms "exothermic reaction" and "endothermic reaction"? Give two examples of each.
8 ST What is the reason why chemical reactions are usually accompanied by gain or loss of heat? 3. Why is it that a reaction which is exothermic such as the combustion of hydrogen gas still requires heat to be supplied before it starts? 4. Utilisation of glucose as a food releases 2807 kj of energy per mole of glucose. Where did the energy to make glucose originate? What happens to the energy released when glucose is utilised? 5. Explain the role of a catalyst. What are the characteristics of catalysts? 6. The Haber synthesis of ammonia produces half of all the nitrogen that is fixed on earth. This reaction combines nitrogen gas and hydrogen gas at high pressure and temperature using a catalyst to achieve large yields economically. Given that for the reaction N 2 (g) + 3H 2 (g) 2NH 3 (g) ÄH = 91.8 kj mol 1 calculate the amount of energy released in the production of 100 g of ammonia.
9 ST3-9 ANSWERS TO TUTORIAL SUPPLEMENTARY TOPIC Exothermic reactions are those that liberate heat while endothermic reactions absorb heat as a result of the reaction occurring. Burning fuels such as methane (natural gas) or petrol are exothermic. Endothermic reactions include the smelting of metal ores such as iron oxide to form the metal. Another example is the formation of carbohydrates by plants using solar energy to provide the required energy. 2. There is usually a difference between the energy stored in the bonds of the reactants and the products. This energy difference is made apparent by the gain or loss of heat during the reaction. 3. To initiate reactions requires some energy to be supplied because the first step involves the breaking of bonds in the reactants, a process that always needs energy input. Once even a small number of bonds have been broken, the energy released from the formation of new bonds may sustain the reaction so continued heating may not be required. For example, a mixture of hydrogen and oxygen gases will not combine unless a spark or similar small amount of heat is supplied and then the mixture explodes instantaneously. The energy required to make a reaction proceed is called its activation energy. 4. The chemical energy stored in the bonds of glucose originated as energy from the sun. Glucose undergoes a series of reactions in cells of the body, ultimately being transformed into water and carbon dioxide and releasing energy in the process. The energy released is used to drive chemical reactions required for processes involved in the metabolism within living cells. 5. Catalysts are substances that enable the activation energy of a reaction to be lowered by using a different pathway between the reactants and the products. Catalysts are not consumed in the reaction and do not increase the yield but speed it up, allowing more product to be obtained in a shorter time and often with the need for less heat to be supplied because the activation energy is smaller. 6. The thermodynamic equation for the reaction, N 2 (g) + 3H 2 (g) 2NH 3 (g) ÄH = 91.8 kj mol 1 shows that the production of 2 moles of ammonia releases 91.8 kj of energy. Molar mass of NH 3 = g mol 1 2 moles of NH 3 has a mass = = g and releases 91.8 kj of energy. production of 100 g of NH 3 releases / kj = 269 kj of energy.
1.4 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 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 informationChemical reactions. C2- Topic 5
Chemical reactions C2- Topic 5 What is a chemical reaction? A chemical reaction is a change that takes place when one or more substances (called reactants) form one or more new substances (called products)
More information5 Energy from chemicals
5 Energy from chemicals Content 5.1 Enthalpy 5.2 Hydrogen fuel cell Learning Outcomes Candidates should be able to: (a) (b) (c) (d) (e) describe the meaning of enthalpy change in terms of exothermic (H
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 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 informationChemistry 101 Chapter 10 Energy
Chemistry 101 Chapter 10 Energy Energy: the ability to do work or produce heat. Kinetic energy (KE): is the energy of motion. Any object that is moving has kinetic energy. Several forms of kinetic energy
More informationQuantitative Relationships in Chemical Reactions Chapter 7
Quantitative Relationships in Chemical Reactions Chapter 7 The burning of charcoal releases heat (thermal energy) that grills our food. But the combustion of charcoal and fossil fuels also releases CO
More informationChapter 8 Thermochemistry: Chemical Energy
Chapter 8 Thermochemistry: Chemical Energy 國防醫學院生化學科王明芳老師 2011-11-8 & 2011-11-15 Chapter 8/1 Energy and Its Conservation Conservation of Energy Law: Energy cannot be created or destroyed; it can only be
More informationSCIENCE 9 CONCEPT 4 CHEMICAL REACTIONS
SCIENCE 9 CONCEPT 4 CHEMICAL REACTIONS VOCABULARY TERMS CONCEPT 4 Chemical reaction Reactants Products Exothermic Endothermic Combustion Corrosion Cellular respiration Conservation of mass Closed systems
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 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 informationQ1. (a) State what is meant by the term activation energy of a reaction. (1)
Q1. (a) State what is meant by the term activation energy of a reaction. (c) State in general terms how a catalyst increases the rate of a chemical reaction. The curve below shows the Maxwell Boltzmann
More information3.2 Alkanes. Refining crude oil. N Goalby chemrevise.org 40 C 110 C 180 C. 250 C fuel oil 300 C 340 C. Fractional Distillation: Industrially
3.2 Alkanes Refining crude oil Fractional Distillation: Industrially Petroleum is a mixture consisting mainly of alkane hydrocarbons Petroleum fraction: mixture of hydrocarbons with a similar chain length
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 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 information(g) 2NH 3. (g) ΔH = 92 kj mol 1
1 The uses of catalysts have great economic and environmental importance For example, catalysts are used in ammonia production and in catalytic converters (a) Nitrogen and hydrogen react together in the
More informationF322: Chains, Energy and Resources Enthalpy Changes
F322: Chains, Energy and Resources 2.3.1 Enthalpy Changes 1. Some reactions of 2 O 2 are exothermic. Use ideas about the enthalpy changes that take place during bond breaking and bond making to explain
More informationChemistry Slide 1 of 33
Chemistry 17.2 1 of 33 17.2 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
More informationName AP CHEM / / Collected AP Exam Essay Answers for Chapter 16
Name AP CHEM / / Collected AP Exam Essay Answers for Chapter 16 1980 - #7 (a) State the physical significance of entropy. Entropy (S) is a measure of randomness or disorder in a system. (b) From each of
More informationLesmahagow High School CfE Higher Chemistry. Chemical Changes & Structure Controlling the Rate
Lesmahagow High School CfE Higher Chemistry Chemical Changes & Structure Controlling the Rate E a Page 1 of 18 Learning Outcomes Controlling the Rate Circle a face to show how much understanding you have
More informationTHERMODYNAMICS. Energy can be neither created nor destroyed but it can be converted from one form to another.
Chemical Energetics 1 TERMODYNAMICS First Law Energy can be neither created nor destroyed but it can be converted from one form to another. all chemical reactions are accompanied by some form of 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 informationSection 1 - Thermochemistry
Reaction Energy Section 1 - Thermochemistry Virtually every chemical reaction is accompanied by a change in energy. Chemical reactions usually absorb or release energy as heat. You learned in Chapter 12
More informationGeneral Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University. Module 4: Chemical Thermodynamics
General Chemistry I Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University Module 4: Chemical Thermodynamics Zeroth Law of Thermodynamics. First Law of Thermodynamics (state quantities:
More informationUnit 7 Kinetics and Thermodynamics
17.1 The Flow of Energy Heat and Work Unit 7 Kinetics and Thermodynamics I. Energy Transformations A. Temperature 1. A measure of the average kinetic energy of the particles in a sample of matter B. Heat
More informationReaction Rates & Equilibrium. What determines how fast a reaction takes place? What determines the extent of a reaction?
Reaction Rates & Equilibrium What determines how fast a reaction takes place? What determines the extent of a reaction? Reactants Products 1 Reaction Rates Vary TNT exploding. A car rusting. Dead plants
More informationName: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each
Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O
More informationAP* Thermodynamics Free Response Questions page 1. Essay Questions
AP* Thermodynamics Free Response Questions page 1 Essay Questions 1991 The reaction represented above is a reversible reaction. BCl 3 (g) + NH 3 (g) Cl 3 BNH 3 (s) (a) Predict the sign of the entropy change,
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 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 informationAccelerated Chemistry Study Guide Chapter 12, sections 1 and 2: Heat in Chemical Reactions
Accelerated Chemistry Study Guide Chapter 12, sections 1 and 2: Heat in Chemical Reactions Terms, definitions, topics Joule, calorie (Re-read p 57-58) Thermochemistry Exothermic reaction Endothermic reaction
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 informationQ1. Methane and oxygen react together to produce carbon dioxide and water.
Q1. Methane and oxygen react together to produce carbon dioxide and water. The methane gas will not burn in oxygen until a flame is applied, but once lit it continues to burn. (a) Explain why energy must
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 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 informationAP Chemistry Chapter 16 Assignment. Part I Multiple Choice
Page 1 of 7 AP Chemistry Chapter 16 Assignment Part I Multiple Choice 1984 47. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(l) H = 889.1 kj H f H 2 O(l) = 285.8 kj mol 1 H f CO 2 (g) = 393.3 kj mol 1 What is
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 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 informationEnthalpy Chapter 5.3-4,7
Enthalpy Chapter 5.3-4,7 heat transfer in (endothermic), +q heat transfer out (exothermic), -q SYSTEM E = q + w w transfer in (+w) w transfer out (-w) Internal Energy at Constant Volume E = E K + E P ΔE
More informationNote: 1 calorie = 4.2 Joules
Enthalpy Changes All substances contain chemical energy, called enthalpy. Like any kind of energy it is measured in Joules (previously energy was measured in Calories). When reactions happen, energy is
More informationEnthalpy changes
2.3.1. Enthalpy changes In an exothermic change energy is transferred from the system (chemicals) to the surroundings. The have less energy than the If an enthalpy change occurs then energy is transferred
More informationChapter Objectives. Chapter 9 Energy and Chemistry. Chapter Objectives. Energy Use and the World Economy. Energy Use and the World Economy
Chapter Objectives Larry Brown Tom Holme www.cengage.com/chemistry/brown Chapter 9 Energy and Chemistry Explain the economic importance of conversions between different forms of energy and the inevitability
More information(02) WMP/Jun10/CHEM2
Energetics 2 Section A Answer all the questions in the spaces provided. 1 An equation for the equilibrium reaction between hydrogen, iodine and hydrogen iodide is shown below. H 2 (g) + I 2 (g) 2HI(g)
More informationcopper carbonate copper oxide carbon dioxide Is the reaction exothermic or endothermic? Use ideas about bonds to explain why.
Endothermic and Exothermic reaction Worksheet Name date period 1 Exothermic and endothermic reactions Decide whether each of these reactions is exothermic or endothermic: a) When two chemicals mix their
More informationEquilibrium. What is equilibrium? Hebden Unit 2 (page 37 69) Dynamic Equilibrium
Equilibrium What is equilibrium? Hebden Unit (page 37 69) Dynamic Equilibrium Hebden Unit (page 37 69) Experiments show that most reactions, when carried out in a closed system, do NOT undergo complete
More informationName: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each
Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O
More informationEnergy Changes in Chemical Reactions
Unit 3 Energetics Unit 3-1 Section 3.1 Energy Changes in Chemical Reactions ( 1 ) Conservation of energy An object which is capable of doing work is said to possess energy. There are many forms of energy:
More information5.7 Quantity Relationships in Chemical Reactions (Stoichiometry)
5.7 Quantity Relationships in Chemical Reactions (Stoichiometry) We have previously learned that atoms combine in simple whole number ratios to form compounds. However, to perform a chemical reaction,
More informationEnergetics. These processes involve energy exchanges between the reacting system and its surroundings.
Energetics Chemical reactions involve: the breaking of bonds between atoms the making of new bonds between atoms These processes involve energy exchanges between the reacting system and its surroundings.
More informationThe reactions we have dealt with so far in chemistry are considered irreversible.
1. Equilibrium Students: model static and dynamic equilibrium and analyse the differences between open and closed systems investigate the relationship between collision theory and reaction rate in order
More informationGummy Bear Demonstration:
Name: Unit 8: Chemical Kinetics Date: Regents Chemistry Aim: _ Do Now: a) Using your glossary, define chemical kinetics: b) Sort the phrases on the SmartBoard into the two columns below. Endothermic Rxns
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 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 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 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 informationWhat does rate of reaction mean?
Junior Science What does rate of reaction mean? It is not how much of a product is made, but instead how quickly a reaction takes place. The speed of a reaction is called the rate of the reaction. What
More informationMgO. progress of reaction
Enthalpy Changes Enthalpy is chemical energy, given the symbol H. We are interested in enthalpy changes resulting from the transfer of energy between chemical substances (the system) and the surroundings
More information(a) Reaction rates (i) Following the course of a reaction Reactions can be followed by measuring changes in concentration, mass and volume of
(a) Reaction rates (i) Following the course of a reaction Reactions can be followed by measuring changes in concentration, mass and volume of reactants or products. g Measuring a change in mass Measuring
More informationChemical changes. All exothermic reactions release heat energy to the surroundings. Heat given out. Products. Progress of reaction
Chemical changes 6.1 Energetics of a reaction All chemical reactions involve an energy change. Energy is taken in or given out in the form of heat. So the reactions are divided into 2 groups Exothermic
More informationReaction Rates & Equilibrium. What determines how fast a reaction takes place? What determines the extent of a reaction?
Reaction Rates & Equilibrium What determines how fast a reaction takes place? What determines the extent of a reaction? Reactants Products 1 Reaction Rates Vary TNT exploding. A car rusting. Dead plants
More informationDefine the term enthalpy change of formation of a compound
1. Alkanes are important hydrocarbons since they are used as fuels in homes and in industry. It is important that the enthalpy changes involved in alkane reactions are known. Define the term enthalpy change
More information3.2.1 Energetics. Enthalpy Change. 263 minutes. 259 marks. Page 1 of 41
..1 Energetics Enthalpy Change 6 minutes 59 marks Page 1 of 41 Q1. (a) Define the term standard molar enthalpy of formation, ΔH f. (b) State Hess s law. (c) Propanone, CO, burns in oxygen as shown by the
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 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 information(b) Describe, and explain, what would happen to the position of the NO 2 /N 2 O 4 equilibrium if the following changes are made
1. Nitrogen dioxide, NO 2, and dinitrogen tetroxide, N 2 O 4, take part in the following equilibrium. 2NO 2 (g) N 2 O 4 (g) ΔH = 58 kj mol 1 (a) State le Chatelier s principle. (b) Describe, and explain,
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 information1. Enthalpy changes of reaction can be determined indirectly from average bond enthalpies and standard enthalpy changes.
1. Enthalpy changes of reaction can be determined indirectly from average bond enthalpies and standard enthalpy changes. The table below shows the values of some average bond enthalpies. bond average bond
More informationWhat is energy??? The ability to do work or produce heat. Potential Energy (PE) energy due to position or composition
Chapter 10: Energy What is energy??? The ability to do work or produce heat. Potential Energy (PE) energy due to position or composition Kinetic Energy (KE) energy due to motion Law of Conservation of
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 informationThe following gas laws describes an ideal gas, where
Alief ISD Chemistry STAAR Review Reporting Category 4: Gases and Thermochemistry C.9.A Describe and calculate the relations between volume, pressure, number of moles, and temperature for an ideal gas as
More informationUnit 3, Lesson 02: Enthalpy Changes in Chemical Reactions
Unit 3, Lesson 02: Enthalpy Changes in Chemical Reactions Chemical Potential Energy refers to the energy that is stored within an atom or molecule because of electrostatic attraction and repulsion between
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 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 information7.1 Describing Reactions
Chapter 7 Chemical Reactions 7.1 Describing Reactions Chemical Equations Equation states what a reaction starts with, and what it ends with. Reactants the starting materials that undergo change. (On the
More informationAS Paper 1 and 2 Kc and Equilibria
AS Paper 1 and 2 Kc and Equilibria Q1.When one mole of ammonia is heated to a given temperature, 50 per cent of the compound dissociates and the following equilibrium is established. NH 3(g) ½ N 2 (g)
More informationTopic 2.1 ENERGETICS. Measuring and Calculating Enthalpy Changes Mean Bond Dissociation Enthalpies Hess Law
Topic 2.1 ENERGETICS Measuring and Calculating Enthalpy Changes Mean Bond Dissociation Enthalpies ess Law 1. Exothermic and endothermic reactions ENTALPY CANGES When a chemical reaction takes place, the
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 informationCHEMISTRY LEVEL 4C (CHM415115)
CHEMISTRY LEVEL 4C (CHM415115) THERMOCHEMISTRY & ENERGY CHANGES THEORY SUMMARY & REVISION QUESTIONS Tasmanian TCE Chemistry Revision Guides by Jak Denny are licensed under a Creative Commons Attribution-NonCommercial-NoDerivatives
More informationStandard enthalpies and standard Gibbs energies of formation 4. Calculating enthalpy changes and Gibbs energy changes for reactions 5
Chemical Reactions as Sources of Energy Part 1: Thermodynamics Contents Standard enthalpies and standard Gibbs energies of formation 4 Calculating enthalpy changes and Gibbs energy changes for reactions
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 informationThermochemistry-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 informationALE 1. Chemical Kinetics: Rates of Chemical Reactions
Name Chem 163 Section: Team Number: ALE 1. Chemical Kinetics: Rates of Chemical Reactions (Reference: Sections 16.1 16.2 + parts of 16.5 16.6 Silberberg 5 th edition) How do the surface area, concentration
More information2-4 Chemical Reactions and Enzymes
2-4 Chemical Reactions and Enzymes Living things, as you have seen, are made up of chemical compounds-some simple and some complex. But chemistry isn t just what life is made of-chemistry is also what
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 informationUNIT ONE BOOKLET 6. Thermodynamic
DUNCANRIG SECONDARY ADVANCED HIGHER CHEMISTRY UNIT ONE BOOKLET 6 Thermodynamic Can we predict if a reaction will occur? What determines whether a reaction will be feasible or not? This is a question that
More informationModule 5: Combustion Technology. Lecture 32: Fundamentals of thermochemistry
1 P age Module 5: Combustion Technology Lecture 32: Fundamentals of thermochemistry 2 P age Keywords : Heat of formation, enthalpy change, stoichiometric coefficients, exothermic reaction. Thermochemistry
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 informationUnderstanding Equations
Chemical Reactions Chemical reaction: a process of chemically changing both the physical and chemical properties of a substance to a new substance with different physical and chemical properties. Video
More informationF322: Chains, Energy and Resources Rates and Equilibria
F322: Chains, Energy and Resources 2.3.2 Rates and Equilibria 1. Dilute aqueous hydrogen peroxide, H 2 O 2 (aq), is used to sterilise contact lenses. Dilute H 2 O 2 (aq) slowly decomposes at room temperature
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 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 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 information2. If the volume of a container holding a gas is reduced, what will happen to the presure within the container?
1. Which gas law states that the volume of a fixed mass of a gas is directly proportional to its Kelvin temperature if the pressure is kept constant? A. Boyle s law B. Charles law C. Dalton s law D. Gay-Lussac
More informationEnergy Changes, Reaction Rates and Equilibrium. Thermodynamics: study of energy, work and heat. Kinetic energy: energy of motion
Energy Changes, Reaction Rates and Equilibrium Thermodynamics: study of energy, work and heat Kinetic energy: energy of motion Potential energy: energy of position, stored energy Chemical reactions involve
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 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 informationUNIT 4 INTRODUCTION TO PHYSICAL CHEMISTRY
UNIT 4 INTRODUCTION TO PHYSICAL CHEMISTRY Student Version www.swotrevision.com www.chemguide.co.uk www.khanacademy.org Contents a) Energy Changes b) Rates of Reaction c) Equilibrium Key words: enthalpy,
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 information