temperature begins to change noticeably. Feedback D. Incorrect. Putting an object on a hot plate will always cause the temperature to increase.
|
|
- Melanie Curtis
- 5 years ago
- Views:
Transcription
1 SAT Chemistry - Problem Drill 22: Thermodynamics No. 1 of A metal with a high heat capacity is placed on top of a hot plate that is turned on. What will happen to the temperature of the piece of metal? (A) The temperature will increase quickly. (B) The temperature will increase slowly. (C) The temperature will decrease quickly. (D) The temperature will decrease slowly. (E) You cannot determine. A high heat capacity means it takes a lot of energy added to the matter before temperature begins to change noticeably. B. Correct. A high heat capacity means it takes a lot of energy added to the matter before temperature begins to change noticeably. Putting an object on a hot plate will always cause the temperature to increase. Putting an object on a hot plate will always cause the temperature to increase. E. Incorrect. You can determine the answer to this question from the given information Heat capacity: The amount of energy that can be absorbed before temperature increases. A lot of energy can be absorbed before the temperature will increases. It will take longer to change temperature because it can absorb a lot of energy before changing temperature. Heat Capacity is an important concept. You will see it again in your studies! The correct answer is (B).
2 No. 2 of Determine if each of the following statements is true or false. If the second statement is a correct explanation for the first statement, mark CE as well. I. Water takes a lot of energy to change temperature. II. Water has a low heat capacity. (A) False, False (B) True, False (C) False, True (D) True, True (E) True, True, CE A. Incorrect! Water does take a lot of energy to change temperature. B. Correct! Water does take a lot of energy to change temperature because it has a high heat capacity. C. Incorrect! Water does take a lot of energy to change temperature because it has a high heat capacity. D. Incorrect! Water does take a lot of energy to change temperature. E. Incorrect! Water does take a lot of energy to change temperature. Heat capacity is the amount of energy needed for 1 gram of a substance to increase temperature by 1 degree Statement I is true water takes a lot of energy to change temperature. Statement II is false water s heat capacity is high. The correct answer is (B).
3 No. 3 of g of a solid is allowed to melt in 400. g of water. The water temperature decreases from 85.1 C to 30.0 C. What is the heat of fusion for the solid in J/g? (A) 115 J/g (B) -115 J/g (C) 460 J/g (D) -460 J/g (E) 4.18 J/g Check you calculations again. Check you calculations again. C. Correct. You correctly found the heat of fusion of this solid. Be sure to use T 2 -T 1 for change in temperature to get the correct sign for heat of fusion. E. Incorrect That is the specific heat capacity of water necessary for these calculations, but it is not the heat of fusion of the solid. m solid = 200.g = mass of the solid m water = 400. g = mass of the water T 1 water = 85.1 C T 2 water = 30.0 C Cp water = 4.18 J/g C H fus solid =? J/g ΔH water = m Cp ΔT ΔH solid = m H fus ΔH water = -ΔH solid (m Cp ΔT) water = (m H fus ) solid ( 30.0 C 85.1 C) = 200 g H fus 400. g 4.18 J. g C 400. g 4.18 J g C 200. g ( 30.0 C 85.1 C) = H fus H fus = 460. J/g Please take the time to truly understand this problem and its solution. It uses several important concepts! The correct answer is (C).
4 No. 4 of Which of the following has an incorrect pairing with the sign of the entropy? (A) I 2 (g) I 2 (s) S = + (B) H 2 O(l) H 2 O(s) S = - (C) CH 3 OH(g) + 3/2 O 2 (g) CO(g) + 2H 2 O(l) S = - (D) 2O 2 (g) + 2SO(g) 2SO 3 (g) S = - (E) None of the choices A. Correct. Moving from gas to solid is a decrease in disorder this is a mis-match in change in entropy sign. Moving from a liquid to a solid is a decrease in disorder. Moving from 5/2 gas molecules to 1 gas and 2 liquid molecules is a decrease in disorder. Moving from 4 gas molecules to 2 gas molecules is a decrease in disorder. E. Incorrect! Look closely there is an equation that is correctly paired with entropy sign. Disorder or randomness. + S is an increase in disorder. - S is a decrease in disorder. A: Gas solid is a decrease in disorder. The sign is incorrect. B: Liquid solid is a decrease in disorder. The sign is correct. C: 5/2 of gas molecules 1 gas and 2 liquid molecules is a decrease in disorder. The sign is correct. D: 4 gas molecules 2 gas molecules is a decrease in disorder. The sign is correct. The correct answer is (A).
5 No. 5 of For 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) at 25 C, the following are relevant. What is the G? H f S N 2 O kj/mole J/K*mole NO kj/mole J/K*mole O 2 0 kj/mole J/K*mole (A) 154 kj (B) kj (C) 84.6 kj (D)-154 kj (E) -43 kj A. Correct. You correctly calculated change in free energy. Be sure to change the entropy quantities to kj to match the enthalpy of fusion and the answer units. Check your calculations again. Check your sign. E. Incorrect. Be sure to multiply each change in enthalpy by the coefficient in the balanced equation.
6 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) T = 25 C+273 = 298 K H f S N 2 O kj/mole J/K*mole NO kj/mole J/K*mole O 2 0 kj/mole J/K*mole G =? ΔH = H f prod H f react ΔS = S prod Δ G = ΔH TΔS ΔH = ( ) ( ) H = kj ΔS = ( ) ( ) S = J/K ( 298K 0. kj ) Δ G = 110.2kJ 1462 K G = 154 kj Not spontaneous The correct answer is (A). S react
7 No. 6 of All of the following reactions illustrate an increase in entropy EXCEPT: (A) N 2 O 4 (g) 2 NO 2 (g) (B) C 6 H 6 (l) C 6 H 6 (g) (C) 2 KClO 3 (s) 3 O 2 (g) + 2 KCl (s) (D) 3 Fe (s) + 2 O 2 (g) Fe 3 O 4 (s) (E) None of the above This is an increase in disorder. This is an increase in disorder. This is an increase in disorder. D. Correct. This is a decrease in disorder. E. Incorrect. Look closely There is an equation that has a decrease in entropy. Entropy is disorder or randomness. A. 1 gas molecule 2 gas molecules. This is an increase in disorder. B. 1 liquid molecule 1 gas molecule. This is an increase in disorder. C. 2 solid molecules 3 gas molecules and 2 solid molecules. This is an increase in disorder. D. 3 solid and 2 gas molecules 1 solid molecule. This is a decrease in disorder. The correct answer is (D).
8 No. 7 of For the following diagram, select the answer that best which explains the difference in length between b & c and between d & e. (A) The strength of individual intermolecular forces is stronger between b & c than between d & e. (B) The strength of individual intermolecular forces is weaker between b & c than between d & e. (C) There are fewer intermolecular forces broken between b & c than between d & e. (D) There are more intermolecular forces broken between b & c than between d & e. (E) There are more molecules being boiled than being melted. The strength of the individual intermolecular forces is not a function of what state the matter is in, but the type of molecule. The strength of individual intermolecular forces doesn t change. The strength of the individual intermolecular forces is not a function of what state the matter is in, but the type of molecule. The strength of individual intermolecular forces doesn t change. C. Correct. There are fewer intermolecular forces broken between b & C than between d & e and therefore it takes less added energy. There are fewer intermolecular forces broken from solid to liquid than from liquid to gas. E. Incorrect! The number of molecules is the same during both changes in state. During phase changes, the energy being added to the system is used to break intermolecular forces Since it s the same molecule during both intervals, the strength of intermolecular forces will be the same. Since the d-e range requires more energy to be added in order to complete the phase change but the strength of the intermolecular forces is the same during both changes, there must be more intermolecular forces broken between d & e. The correct answer is (C).
9 No. 8 of If 1000 kj of energy is released, how many grams of water are produced for the following reaction? B 2 H 6 (g) + 3 O 2 (g) B 2 O 3 (s) + 2 H 2 O (g) H = kj (A) 8.86 g (B) g (C) g (D) g (E) g First convert energy to mole H 2 O using the balanced equation information and then convert moles to grams using the molar mass. First convert energy to mole H 2 O using the balanced equation information and then convert moles to grams using the molar mass. First convert energy to mole H 2 O using the balanced equation information and then convert moles to grams using the molar mass. D. Correct. You correctly used stoichiometry to calculate the grams of water produced. E. Incorrect. Check your sign. Use the energy change of the reaction along with the mole ratio from the balanced equation kj = 2 mole H 2 O (molar mass of H 2 O) 1 mole H 2 O = g H 2 O kj 2 mole H 2 O g H 2 O = g kj 1 mole H 2 O H 2 O You could solve this problem by estimation as well as by calculation. First, recognize that 1000 is about ½ of Second, recognize that there are 2 moles of H 2 O produced. Third, (1/2)*2 =1 mole. Therefore, look for an answer that is slightly less than grams that corresponds to one mole. The correct answer is (D).
10 No. 9 of For 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) find heat of reaction if: N 2 O 5 NO 2 O 2 ΔH f kj/mole kj/mole 0 kj/mole (A) kj (B) kj (C) kj (D) kj (E) None of these options is correct. Check your sign. B. Correct. You successfully used enthalpy of formation to calculate enthalpy of a reaction. Make sure to multiply the enthalpy of formation values by the moles in the balanced equation before calculating enthalpy of reaction. Make sure to multiply the enthalpy of formation values by the moles in the balanced equation before calculating enthalpy of reaction. E. Incorrect! Check your calculations again one of these choices is correct. To find heat of reaction from heat of formation, find the sum of the products and subtract the sum of the reactants. ΔH rxn = H f prod H f react [( kJ ) + ( 1 0kJ )] [ kj ] Δ H rxn = 29 mole mole = 110 kj mole Although, not asked in the question, recognize that there will be a very large increase in entropy, because you are starting with 2 moles of gas and ending with 5 moles of gas. The correct answer is (B).
11 No. 10 of For the following, N H 2 2 NH 3 ΔH = -92 kj ΔS = -199 J/K mole ΔG is between which interval at 200 K? (A) Less than -100 kj (B) Between -100 kj and -40 kj (C) Between -40 kj and +40 kj (D) Between +40 kj and +100 kj (E) More than +100 kj Find change in free energy by multiplying temperature times entropy and subtracting that value from enthalpy. B. Correct. You correctly estimated the free energy. Find change in free energy by multiplying temperature times entropy and subtracting that value from enthalpy. Find change in free energy by multiplying temperature times entropy and subtracting that value from enthalpy. E. Incorrect! Find change in free energy by multiplying temperature times entropy and subtracting that value from enthalpy. Δ G = ΔH TΔS ΔG = 92 kj 200K kJ K mole = = -52 kj The correct answer is (B).
MCAT General Chemistry Discrete Question Set 19: Thermochemistry & Thermodynamics
MCAT General Chemistry Discrete Question Set 19: Thermochemistry & Thermodynamics Question No. 1 of 10 1: A metal with a high heat capacity is put on a hot plate. What will happen? Question #01 A. The
More informationOAT General Chemistry Problem Drill 15: Thermochemistry & Thermodynamics
OAT General Chemistry Problem Drill 15: Thermochemistry & Thermodynamics Question No. 1 of 10 1. A metal with a high heat capacity is put on a hot plate. What will happen? Question #01 (A) The temperature
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 informationThermochemistry. 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 informationThermodynamics. Thermodynamics of Chemical Reactions. Enthalpy change
Thermodynamics 1 st law (Cons of Energy) Deals with changes in energy Energy in chemical systems Total energy of an isolated system is constant Total energy = Potential energy + kinetic energy E p mgh
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 19 Chemical Thermodynamics
Chapter 19 Chemical Thermodynamics Spontaneous Processes Entropy and the Second Law of Thermodynamics The Molecular Interpretation of Entropy Entropy Changes in Chemical Reactions Gibbs Free Energy Free
More informationClass XI Chapter 6 Thermodynamics Chemistry
Class XI Chapter 6 Chemistry Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii) used
More informationThermochemistry. 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 informationChemistry 123: Physical and Organic Chemistry Topic 2: Thermochemistry
Recall the equation. w = -PΔV = -(1.20 atm)(1.02 L)( = -1.24 10 2 J -101 J 1 L atm Where did the conversion factor come from? Compare two versions of the gas constant and calculate. 8.3145 J/mol K 0.082057
More informationChemical Thermodynamics
Page III-16-1 / Chapter Sixteen Lecture Notes Chemical Thermodynamics Thermodynamics and Kinetics Chapter 16 Chemistry 223 Professor Michael Russell How to predict if a reaction can occur, given enough
More informationENTHALPY CHANGE CHAPTER 4
ENTHALPY CHANGE CHAPTER 4 ENTHALPY Is the total energy of a system. E k = Kinetic energy. Vibrational Rotational Translational E due to motion H = E k + E p E P = Potential energy Attractive force b/w
More information1. How much heat is required to warm 400. g of ethanol from 25.0ºC to 40.0ºC?
Heat and q=mcδt 1. How much heat is required to warm 400. g of ethanol from 25.0ºC to 40.0ºC? 2. What mass of water can be heated from 0.00ºC to 25.0ºC with 90,000. J of energy? 3. If 7,500. J of energy
More informationStudy of energy changes that accompany physical and chemical changes.
Thermodynamics: Study of energy changes that accompany physical and chemical changes. First Law of Thermodynamics: Energy is niether created nor destroyed but simply converted from one form to another.
More informationAP CHEMISTRY SCORING GUIDELINES
Mean 5.64 out of 9 pts AP CHEMISTRY Question 1 CO(g) + 1 2 O 2 (g) CO 2 (g) 1. The combustion of carbon monoxide is represented by the equation above. (a) Determine the value of the standard enthalpy change,
More informationTHERMODYNAMICS. Dr. Sapna Gupta
THERMODYNAMICS Dr. Sapna Gupta FIRST LAW OF THERMODYNAMICS Thermodynamics is the study of heat and other forms of energy involved in chemical or physical processes. First Law of Thermodynamics Energy cannot
More informationAdvanced Chemistry Practice Problems
Thermodynamics: Review of Thermochemistry 1. Question: What is the sign of DH for an exothermic reaction? An endothermic reaction? Answer: ΔH is negative for an exothermic reaction and positive for an
More informationOCR Chemistry A H432
All the energy changes we have considered so far have been in terms of enthalpy, and we have been able to predict whether a reaction is likely to occur on the basis of the enthalpy change associated with
More informationCHM 112 Chapter 16 Thermodynamics Study Guide
CHM 112 Chapter 16 Thermodynamics Study Guide Remember from Chapter 5: Thermodynamics deals with energy relationships in chemical reactions Know the definitions of system, surroundings, exothermic process,
More informationEnergy is the capacity to do work
1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More 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 information10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics
Chapter 10 Thermochemistry 10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics OFB Chap. 10 1 OFB Chap. 10 2 Thermite Reaction
More 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 informationCHEMISTRY 202 Practice Hour Exam II. Dr. D. DeCoste T.A (60 pts.) 21 (40 pts.) 22 (20 pts.)
CHEMISTRY 202 Practice Hour Exam II Fall 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 22 questions on 7 numbered pages. Check now to make sure you have a complete exam. You have two hours
More informationCh. 14 Notes ENERGY AND CHEMICAL CHANGE NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 14 Notes ENERGY AND CHEMICAL CHANGE NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Energy the capacity to do work or produce heat A. two basic types of
More informationCHM 111 Dr. Kevin Moore
CHM 111 Dr. Kevin Moore Kinetic Energy Energy of motion E k 1 2 mv 2 Potential Energy Energy of position (stored) Law of Conservation of Energy Energy cannot be created or destroyed; it can only be converted
More informationChem 401 Unit 1 (Kinetics & Thermo) Review
KINETICS 1. For the equation 2 H 2(g) + O 2(g) 2 H 2 O (g) How is the rate of formation of H 2 O mathematically related to the rate of disappearance of O 2? 1 Δ [H2O] Δ[O 2] = 2 Δt Δt 2. Determine the
More informationSupplemental Activities. Module: Thermodynamics. Section: Second Law of Thermodynamics Key
Supplemental Activities Module: Thermodynamics Section: Second Law of Thermodynamics Key Spontaneity ACTIVITY 1 The purpose of this activity is to practice your understanding of the concept of spontaneous
More informationSecond law of thermodynamics
Second law of thermodynamics It is known from everyday life that nature does the most probable thing when nothing prevents that For example it rains at cool weather because the liquid phase has less energy
More informationWhat is a spontaneous reaction? One, that given the necessary activation energy, proceeds without continuous outside assistance
What is a spontaneous reaction? One, that given the necessary activation energy, proceeds without continuous outside assistance Why do some reactions occur spontaneously & others do not? Atoms react to
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 information17.4 Calculating Heats Essential Understanding Heats of reaction can be calculated when it is difficult or
17.4 Calculating Heats of Reaction Essential Understanding Heats of reaction can be calculated when it is difficult or impossible to measure them directly. Lesson Summary Hess s Law Hess s law provides
More informationIn previous chapters we have studied: Why does a change occur in the first place? Methane burns but not the reverse CH 4 + 2O 2 CO 2 + 2H 2 O
Chapter 19. Spontaneous Change: Entropy and Free Energy In previous chapters we have studied: How fast does the change occur How is rate affected by concentration and temperature How much product will
More informationChapter 10: Phenomena
Chapter 10: Phenomena Phenomena: Below is data from several different chemical reactions. All reaction were started by putting some of every substance in the chemical reaction into an expandable/contractable
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 17: Energy and Kinetics
Pages 510-547 S K K Chapter 17: Energy and Kinetics Thermochemistry: Causes of change in systems Kinetics: Rate of reaction progress (speed) Heat, Energy, and Temperature changes S J J Heat vs Temperature
More informationThermodynamics: Entropy
Name: Band: Date: Thermodynamics: Entropy Big Idea: Entropy When we were studying enthalpy, we made a generalization: most spontaneous processes are exothermic. This is a decent assumption to make because
More informationUnit 12. Thermochemistry
Unit 12 Thermochemistry A reaction is spontaneous if it will occur without a continuous input of energy However, it may require an initial input of energy to get it started (activation energy) For Thermochemistry
More informationUnit 4: Thermochemistry
Unit 4: Thermochemistry The making and breaking of bonds only happen as a result of energy being exchanged. Some reactions give off energy and some take in energy. This unit is all about the energy of
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 informationThermodynamics. For the process to occur under adiabatic conditions, the correct condition is: (iii) q = 0. (iv) = 0
Thermodynamics Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii) used to determine pressure volume
More informationI PUC CHEMISTRY CHAPTER - 06 Thermodynamics
I PUC CHEMISTRY CHAPTER - 06 Thermodynamics One mark questions 1. Define System. 2. Define surroundings. 3. What is an open system? Give one example. 4. What is closed system? Give one example. 5. What
More informationCh 17 Free Energy and Thermodynamics - Spontaneity of Reaction
Ch 17 Free Energy and Thermodynamics - Spontaneity of Reaction Modified by Dr. Cheng-Yu Lai spontaneous nonspontaneous Spontaneous Processes Processes that are spontaneous in one direction are nonspontaneous
More informationSecond Law of Thermodynamics
Second Law of Thermodynamics First Law: the total energy of the universe is a constant Second Law: The entropy of the universe increases in a spontaneous process, and remains unchanged in a process at
More informationChapter 19 Chemical Thermodynamics Entropy and free energy
Chapter 19 Chemical Thermodynamics Entropy and free energy Learning goals and key skills: Explain and apply the terms spontaneous process, reversible process, irreversible process, and isothermal process.
More informationEntropy. Spontaneity. Entropy. Entropy mol of N 2 at 1 atm or 1 mol of N 2 at atm. process a process that occurs without intervention
Entropy Spontaneity process a process that occurs without intervention can be fast or slow Entropy (s) the measure of molecular randomness or disorder Think of entropy as the amount of chaos Entropy Predict
More informationFree-energy change ( G) and entropy change ( S)
Free-energy change ( G) and entropy change ( S) A SPONTANEOUS PROCESS (e.g. diffusion) will proceed on its own without any external influence. A problem with H A reaction that is exothermic will result
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 informationChemical Thermodynamics. Chapter 18
Chemical Thermodynamics Chapter 18 Thermodynamics Spontaneous Processes Entropy and Second Law of Thermodynamics Entropy Changes Gibbs Free Energy Free Energy and Temperature Free Energy and Equilibrium
More informationThermochemistry Chapter 8
Thermochemistry Chapter 8 Thermochemistry First law of thermochemistry: Internal energy of an isolated system is constant; energy cannot be created or destroyed; however, energy can be converted to different
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 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 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 informationBasics of Thermodynamics: Easy learning by Dr. Anjana Sen
Basics of Thermodynamics: Easy learning by Dr. Anjana Sen Part 1: Theory and concept Part 2: Definitions and equations Part 3: Laws of Thermodynamics Part 1: theory and concept Thermodynamics means conversion
More informationChapter Eighteen. Thermodynamics
Chapter Eighteen Thermodynamics 1 Thermodynamics Study of energy changes during observed processes Purpose: To predict spontaneity of a process Spontaneity: Will process go without assistance? Depends
More informationGibb s Free Energy. This value represents the maximum amount of useful work (non PV-work) that can be obtained by a system.
Gibb s Free Energy 1. What is Gibb s free energy? What is its symbol? This value represents the maximum amount of useful work (non PV-work) that can be obtained by a system. It is symbolized by G. We only
More informationThe Laws of Thermodynamics
Entropy I. This, like enthalpy, Thus, II. A reaction is ( more on this later) if: (H, enthalpy) (S, entropy) III. IV. Why does entropy happen? Probability It s harder to keep things in order (look at my
More informationChemical thermodynamics and bioenergetics
Chemical thermodynamics and bioenergetics Thermodynamics is a branch of physics that studies energy, the forms of its transformation, and the laws controlling its properties. Basic Concepts and Definitions.
More informationGibbs Free Energy Study Guide Name: Date: Period:
Gibbs Free Energy Study Guide Name: Date: Period: The basic goal of chemistry is to predict whether or not a reaction will occur when reactants are brought together. Ways to predict spontaneous reactions
More informationNCERT THERMODYNAMICS SOLUTION
NCERT THERMODYNAMICS SOLUTION 1. Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii) used to determine
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 informationChem 1B Dr. White 1 Chapter 17: Thermodynamics. Review From Chem 1A (Chapter 6, section 1) A. The First Law of Thermodynamics
Chem 1B Dr. White 1 Chapter 17: Thermodynamics Review From Chem 1A (Chapter 6, section 1) A. The First Law of Thermodynamics 17.1 Spontaneous Processes and Entropy A. Spontaneous Change Chem 1B Dr. White
More informationUNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW
Version A UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, 2015 5-6 pm (60 minutes) Version A DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW Answer all multiple choice questions
More informationUNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW
Version B UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 13, 2015 5-6 pm (60 minutes) Version B DISPLAY YOUR STUDENT ID CARD (ONECard) ON TOP OF YOUR DESK NOW Answer all multiple choice questions
More 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 informationContents and Concepts
Contents and Concepts 1. First Law of Thermodynamics Spontaneous Processes and Entropy A spontaneous process is one that occurs by itself. As we will see, the entropy of the system increases in a spontaneous
More informationHeating Curve Worksheet If this curve is read from right to left, it is a Cooling Curve.
Heating Curve Worksheet If this curve is read from right to left, it is a Cooling Curve. The diagram below illustrates the steps involved to convert 10g of solid ice at -20 C to 10g of gaseous steam at
More informationLECTURE 25. EQUILIBRIUM, FREE ENERGY AND TEMPERATURE
LECTURE 25. EQUILIBRIUM, FREE ENERGY AND TEMPERATURE Equilibrium: We hinted at equilibrium while discussing thermodynamics (for example, noting that at a phase change, like melting or boiling, a system
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 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 informationThermochemistry is the study of the relationships between chemical reactions and energy changes involving heat.
CHEM134- F18 Dr. Al- Qaisi Chapter 06: Thermodynamics Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat. Energy is anything that has the capacity
More informationChapter 5 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 informationAP Chemistry Big Idea Review
Name: AP Chemistry Big Idea Review Background The AP Chemistry curriculum is based on 6 Big Ideas and many Learning Objectives associated with each Big Idea. This review will cover all of the Big Ideas
More informationEnergy and Chemical Change
Energy and Chemical Change Section 15.1 Energy Section 15.2 Heat Section 15.3 Thermochemical Equations Section 15.4 Calculating Enthalpy Change Section 15.5 Reaction Spontaneity Click a hyperlink or folder
More informationExam 4. Remember to refer to the Periodic Table handout that is separate from this exam copy.
001 version last name first name signature McCord CH301 unique: 49885 TTh 9:30 am - 11:00 am Exam 4 Dec 3, 2018 Monday 7:30-9:00 PM A - Mi in BUR 106 Mo - Z in JES A121A Remember to refer to the Periodic
More informationVanden Bout/LaBrake. Important Information. HW11 Due T DECEMBER 4 th 9AM. End of semester attitude survey closes next Monday
UNIT4DAY6-LaB Page 1 UNIT4DAY6-LaB Thursday, November 29, 2012 8:13 AM Vanden Bout/LaBrake CH301 The 2 nd Law of Thermodynamics GIBBS FREE ENERGY UNIT 4 Day 6 Important Information HW11 Due T DECEMBER
More informationThermodynamics and Equilibrium. Chemical thermodynamics is concerned with energy relationships in chemical reactions.
1 of 7 Thermodynamics and Equilibrium Chemical thermodynamics is concerned with energy relationships in chemical reactions. In addition to enthalpy (H), we must consider the change in randomness or disorder
More informationWarm up. 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]?
Warm up 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]? 4) What is the concentration of H 2 SO 4 if 30.1 ml
More 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 informationUnit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit.
Unit 5: Spontaneity of Reaction You need to bring your textbooks everyday of this unit. THE LAWS OF THERMODYNAMICS 1 st Law of Thermodynamics Energy is conserved ΔE = q + w 2 nd Law of Thermodynamics A
More information5.2 Energy. N Goalby chemrevise.org Lattice Enthalpy. Definitions of enthalpy changes
5.2 Energy 5.2.1 Lattice Enthalpy Definitions of enthalpy changes Enthalpy change of formation The standard enthalpy change of formation of a compound is the energy transferred when 1 mole of the compound
More informationASSIGNMENT SHEET #11 APQ ANSWERS
ASSIGNMENT SHEET #11 APQ ANSWERS #1 a. The unit for q must be an energy unit, typically Joules or calories. The unit for mass is the gram. The unit for specific heat is J per gram-degree or calorie per
More informationFor more info visit
Basic Terminology: Terms System Open System Closed System Isolated system Surroundings Boundary State variables State Functions Intensive properties Extensive properties Process Isothermal process Isobaric
More informationSpontaneity, Entropy, and Free Energy
Spontaneity, Entropy, and Free Energy A ball rolls spontaneously down a hill but not up. Spontaneous Processes A reaction that will occur without outside intervention; product favored Most reactants are
More informationExam 2 Solutions. for a gas obeying the equation of state. Z = PV m RT = 1 + BP + CP 2,
Chemistry 360 Dr. Jean M. Standard Fall 016 Name KEY 1.) (14 points) Determine # H & % ( $ ' Exam Solutions for a gas obeying the equation of state Z = V m R = 1 + B + C, where B and C are constants. Since
More informationIs NOT just ΔG = (-) It IS ΔG = -2070kJ which means it is really spontaneous.
LECTURE 21. THERMODYNAMICS LET S GET QUANTITATIVE Today we will examine the quantitative side of thermodynamics, while actually coming up with numerical values for ΔH, ΔS, etc. Up to this point we have
More informationFinal Exam Review-Honors Name Period
Final Exam Review-Honors Name Period This is not a fully comprehensive review packet. This packet is especially lacking practice of explanation type questions!!! You should study all previous review sheets
More 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 informationSolution: 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 informationCHEMISTRY 202 Hour Exam II. Dr. D. DeCoste T.A (60 pts.) 31 (20 pts.) 32 (40 pts.)
CHEMISTRY 202 Hour Exam II October 27, 2015 Dr. D. DeCoste Name Signature T.A. This exam contains 32 questions on 11 numbered pages. Check now to make sure you have a complete exam. You have two hours
More information10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics
Chapter 10 Thermochemistry 10-1 Heat 10-2 Calorimetry 10-3 Enthalpy 10-4 Standard-State Enthalpies 10-5 Bond Enthalpies 10-6 The First Law of Thermodynamics OFB Chap. 10 1 Chapter 10 Thermochemistry Heat
More informationThermodynamics Test Clio Invitational January 26, 2013
Thermodynamics Test Clio Invitational January 26, 2013 School Name: Team Number: Variables specified: s = specific heat C = heat capacity H f = heat of fusion H v = heat of vaporization Given information:
More informationClass XI Chapter 6 Thermodynamics Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii)
More 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 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 informationLearning Check. How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C?
Learning Check q = c * m * ΔT How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C? (c water =4.184 J/ C g, c iron =0.450 J/ C g) q Fe = 0.450
More 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 information= (+)206 (kj mol 1) 206 scores 1 only Units not essential if ans in kj mol 1 but penalise incorrect units
M.(a) (i) ΔH = Σ(enthalpies formation products) Σ(enthalpies formation reactants) Or correct cycle with enthalpy changes labelled = ( 75 242) = (+)206 (kj mol ) 206 scores only Units not essential if ans
More informationThermodynamics: Study of heat and its relationship with other forms of energy
Unit 6 The 6 th planet in our solar system is Saturn Ch. 5: Thermodynamics: Study of heat and its relationship with other forms of energy Two types of energy: Kinetic: movement, active energy Potential:
More informationCh. 19 Entropy and Free Energy: Spontaneous Change
Ch. 19 Entropy and Free Energy: Spontaneous Change 19-1 Spontaneity: The Meaning of Spontaneous Change 19-2 The Concept of Entropy 19-3 Evaluating Entropy and Entropy Changes 19-4 Criteria for Spontaneous
More information