B 2 Fe(s) O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.
|
|
- Phebe Kelley
- 5 years ago
- Views:
Transcription
1 B 2 Fe(s) O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.0 g sample of Fe(s) is mixed with 11.5 L of O 2 (g) at 2.66 atm and 298 K. (a) Calculate the number of moles of each of the following before the reaction occurs. (i) Fe(s) (ii) O 2 (g) (b) Identify the limiting reactant when the mixture is heated to produce Fe 2 O 3. Support your answer with calculations. (c) Calculate the number of moles of Fe 2 O 3 produced when the reaction proceeds to completion. (d) The standard free energy of formation, G f of Fe 2 O 3 is 740. kj mol 1 at 298 K. (i) Calculate the standard entropy of formation S f of Fe 2 O 3 at 298 K. Include units with your answer. (ii) Which is more responsible for the spontaneity of the formation reaction at 298K, the standard enthalpy or the standard entropy? The reaction represented below also produces iron(iii) oxide. The value of H for the reaction is 280 kj per mol. 2 FeO(s) O 2(g) Fe 2 O 3 (s) (e) Calculate the standard enthalpy of formation, H f of FeO(s).
2 D [repeated in electrochem] AgNO 3 (s) Ag + (aq) + NO 3 (aq) The dissolving of AgNO 3 (s) in pure water is represented by the equation above.. (a) Is G for the dissolving of AgNO 3 (s) positive, negative, or zero? Justify your answer. (b) Is S for the dissolving of AgNO 3 (s) positive, negative, or zero? Justify your answer. (c) The solubility of AgNO 3 (s) increases with increasing temperature. (i) What is the sign of H for the dissolving process? Justify your answer. (ii) Is the answer you gave in part (a) consistent with your answers to parts (b) and (c) (i)? Explain. The compound NaI dissolves in pure water according to the equation NaI(s) Na + (aq) + I (aq). Some of the information in the table of standard reduction potentials given below may be useful in answering the questions that follow. Half-reaction E (V) O 2 (g) + 4 H e- 2 H 2 O(l) 1.23 I 2 (s) + 2 e- 2 I H 2 O(l) + 2 e- H 2 (g) + 2 OH Na + + e- Na(s) (d) An electric current is applied to a 1.0 M NaI solution. (i) Write the balanced oxidation half reaction for the reaction that takes place. (ii) Write the balanced reduction half-reaction for the reaction that takes place. (iii) Which reaction takes place at the anode, the oxidation reaction or the reduction reaction? (iv) All electrolysis reactions have the same sign for G. Is the sign positive or negative? Justify your answer.
3 B CO(g) O2(g) CO2(g) The combustion of carbon monoxide is represented by the equation above. (a) Determine the value of the standard enthalpy change, H rxn for the combustion of CO(g) at 298 K using the following information. C(s) O2(g) CO(g) H 298 = kj mol-1 C(s) + O2(g) CO2(g) H 298 = kj mol -1 (b) Determine the value of the standard entropy change, S rxn, for the combustion of CO(g) at 298 K using the information in the following table. Substance S 298 (J mol -1 K -1 ) CO(g) CO2(g) O2(g) (c) Determine the standard free energy change, G rxn, for the reaction at 298 K. Include units with your answer. (d) Is the reaction spontaneous under standard conditions at 298 K? Justify your answer. (e) Calculate the value of the equilibrium constant, Keq, for the reaction at 298 K.
4 part A, question #2 o N2(g) + 3 F2(g) 2 NF3(g) H J K 1 mol 1 = 264 kj mol 1 o ; S 298 = The following questions relate to the synthesis reaction represented by the chemical equation in the box above. o (a) Calculate the value of the standard free energy change, G 298 for the reaction. (b) Determine the temperature at which the equilibrium constant, Keq, for the reaction is equal to (Assume that H and S are independent of temperature.) (c) Calculate the standard enthalpy change, H, that occurs when a mol sample of NF3(g) is formed from N2(g) and F2(g) at 1.00 atm and 298 K. The enthalpy change in a chemical reaction is the difference between energy absorbed in breaking bonds in the reactants and energy released by bond formation in the products. (d) How many bonds are formed when two molecules of NF3 are produced according to the equation in the box above? (e) Use both the information in the box above and the table of average bond enthalpies below to calculate the average enthalpy of the F F bond. Bond Average Bond Enthalpy (kj mol -1 ) N N 946 N F 272 F F?
5 part A, form B, question #1 A sample of solid U308 is placed in a rigid L flask. Chlorine gas, Cl2(g), is added, and the flask is heated to 862 C. The equation for the reaction that takes place and the equilibriumconstant expression for the reaction are given below. U308(s) + 3 Cl2(g), 3 UO2Cl2(g) + O2(g) K P (P UO 2 Cl 2 ) 3 (P O2 ) (P Cl2 ) 3 When the system is at equilibrium, the partial pressure of Cl2(g) is atm and the partial pressure of UO2Cl2(g) is atm (a) Calculate the partial pressure of O2(g) at equilibrium at 862 C. (b) Calculate the value of the equilibrium constant, KP, for the system at 862 C. (c) Calculate the Gibbs free-energy change, G, for the reaction at 862 C. (d) State whether the entropy change, S for the reaction at 862 C is positive, negative, or zero. Justify your answer. (e) State whether the enthalpy change, H, for the reaction at 862 C is positive, negative, or zero. Justify your answer. (f) After a certain period of time, mol of O2(g) is added to the mixture in the flask. Does the mass of U308(s) in the flask increase, decrease, or remain the same? Justify your answer.
6 D Answer the following questions that relate to the chemistry of nitrogen. (a) Two nitrogen atoms combine to form a nitrogen molecule, as represented by the following equation. 2 N(g) N2(g) Using the table of average bond energies below, determine the enthalpy change, H, for the reaction. Bond Average Bond Energy (kj mol 1 ) N N 160 N=N 420 N N 950 (b) The reaction between nitrogen and hydrogen to form ammonia is represented below. N2(g) + 3 H2(g) 2 NH3(g) H = 92.2 kj Predict the sign of the standard entropy change, S, for the reaction. Justify your answer.
7 B 2 NO(g) + O2(g) 2 NO2(g) H = kj, S = J K -1 The reaction represented above is one that contributes significantly to the formation of photochemical smog. (a) Calculate the quantity of heat released when 73.1 g of NO(g) is converted to NO2(g). (b) For the reaction at 25 C, the value of the standard free-energy change, G, is kj. (i) Calculate the value of the equilibrium constant, Keq, for the reaction at 25 C. (ii) Indicate whether the value of G would become more negative, less negative, or remain unchanged as the temperature is increased. Justify your answer. (c) Use the data in the table below to calculate the value of the standard molar entropy, S, for O2(g) at 25 C. Standard Molar Entropy, S (J K -1 mol -1 ) NO(g) NO2(g) (d) Use the data in the table below to calculate the bond energy, in kj mol -1, of the nitrogenoxygen bond in NO2. Assume that the bonds in the NO2 molecule are equivalent (i.e., they have the same energy). Bond Energy (kj mol -1 ) Nitrogen-oxygen bond in NO 607 Oxygen-oxygen bond in O2 495 Nitrogen-oxygen bond in NO2?
8 B C 2H 2(g) + 2 H 2(g) C 2H 6(g) Information about the substances involved in the reaction represented above is summarized in the following tables. Substance S (J/mol K) H f (kj/mol) C 2H 2(g) H 2(g) C 2H 6(g) Bond Bond Energy (kj/mol) C-C 347 C=C 611 C-H 414 H-H 436 (a) If the value of the standard entropy change, S, for the reaction is joules per mole Kelvin, calculate the standard molar entropy, S, of C 2H 6 gas. (b) Calculate the value of the standard free-energy change, G, for the reaction. What does the sign of G indicate about the reaction above? (c) Calculate the value of the equilibrium constant, K, for the reaction at 298 K. (d) Calculate the value of the C C bond energy in C 2H 2 in kilojoules per mole.
9 A sample of CH3CH2NH2 is placed in an insulated container, where it decomposes into ethene and ammonia according to the reaction represented above. Substance Absolute Entropy, S, in J/( mol K) at 298 K CH3CH2NH2(g) CH2CH2(g) NH3(g) a. Using the data in the table above, calculate the value, in J/(molrxn K), of the standard entropy change, ΔS, for the reaction at 298 K. b. Using the data in the table below, calculate the value, in kj/molrxn, of the standard enthalpy change, ΔH, for the reaction at 298 K. Bond C C C = C C H C N N H Average Bond Enthalpy (kj/mol)
10 c. Based on your answer to part (b), predict whether the temperature of the contents of the insulated container will increase, decrease, or remain the same as the reaction proceeds. Justify your prediction. An experiment is carried out to measure the rate of the reaction, which is first order. A mol sample of CH 3CH 2NH 2 is placed in a previously evacuated 2.00 L container at 773 K. After 20.0 minutes, the concentration of the CH 3CH 2NH2 is found to be mol/l. Calculate the rate constant for the reaction at 773 K. Include units with your answer. Calculate the initial rate, in M min 1, of the reaction at 773 K. If 1/[CH 3CH 2NH 2] is plotted versus time for this reaction, would the plot result in a straight line or would it result in a curve? Explain your reasoning.
11 MgO(s) + 2 H + (aq) Mg 2+ (aq) + H2O(l) A student was assigned the task of determining the enthalpy change for the reaction between solid MgO and aqueous HCl represented by the net-ionic equation above. The student uses a polystyrene cup calorimeter and performs four trials. Data for each trial are shown in the table below. Trial Volume of 1.0 M HCl (ml) Mass of MgO(s) Added (g) Initial Temperature of Solution (qc) Final Temperature of Solution (qc) (a) Which is the limiting reactant in all four trials, HCl or MgO? Justify your answer. (b) The data in one of the trials is inconsistent with the data in the other three trials. Identify the trial with inconsistent data and draw a line through the data from that trial in the table above. Explain how you identified the inconsistent data. For parts (c) and (d), use the data from one of the other three trials (i.e., not from the trial you identified in part (b) above). Assume the calorimeter has a negligible heat capacity and that the specific heat of the contents of the calorimeter is 4.18 J/(g Cq). Assume that the density of the HCl(aq) is 1.0 g/ml. (b) Calculate the magnitude of q, the thermal energy change, when the MgO was added to the 1.0 M HCl(aq). Include units with your answer. (c) Determine the student s experimental value of Hq for the reaction between MgO and HCl in units of kj/molrxn. (d) Enthalpies of formation for substances involved in the reaction are shown in the table below. Using the information in the table, determine the accepted value of Hq for the reaction between MgO(s) and HCl(aq). Substance H (kj/mol) f MgO(s) 602 H2O(l) 286 H + (aq) 0 Mg 2+ (aq) 467 (e) The accepted value and the experimental value do not agree. If the calorimeter leaked heat energy to the environment, would it help account for the discrepancy between the values? Explain.
Saturday 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 informationSt. John s College High School Mr. Trubic AP Midterm Review Packet 2
Name Date Directions: Read each question carefully and write your response in the space provided following each question. Your responses to these questions will be scored on the basis of the accuracy and
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 informationAP Questions: Thermodynamics
AP Questions: Thermodynamics 1970 Consider the first ionization of sulfurous acid: H2SO3(aq) H + (aq) + HSO3 - (aq) Certain related thermodynamic data are provided below: H2SO3(aq) H + (aq) HSO3 - (aq)
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 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. 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 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 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 information(E) half as fast as methane.
Name AP Chem / / AP Chem Practice Exam #2 Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the BLUE SIDE of your scantron for each of the following.
More informationIB Topics 5 & 15 Multiple Choice Practice
IB Topics 5 & 15 Multiple Choice Practice 1. Which statement is correct for this reaction? Fe 2O 3 (s) + 3CO (g) 2Fe (s) + 3CO 2 (g) ΔH = 26.6 kj 13.3 kj are released for every mole of Fe produced. 26.6
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 informationThe chemical potential energy of a substance is known as its ENTHALPY and has the symbol H.
Enthalpy Changes The chemical potential energy of a substance is known as its ENTHALPY and has the symbol H. During chemical reactions, the enthalpy can increase or decrease. The change in enthalpy during
More informationName period AP Unit 8: equilibrium
Name period AP Unit 8: equilibrium 1. What is equilibrium? Rate of the forward reaction equals the rate of the reverse reaction 2. How can you tell when equilibrium has been reached? The concentrations
More informationCh 10 Practice Problems
Ch 10 Practice Problems 1. Which of the following result(s) in an increase in the entropy of the system? I. (See diagram.) II. Br 2(g) Br 2(l) III. NaBr(s) Na + (aq) + Br (aq) IV. O 2(298 K) O 2(373 K)
More informationChapter 6. Thermochemistry
Chapter 6. Thermochemistry 1 1. Terms to Know: thermodynamics thermochemistry energy kinetic energy potential energy heat heat vs. temperature work work of expanding gases work of expanding gases under
More informationChapter 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 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 informationUNIVERSITY OF SIERRA LEONE FOURAH BAY COLLEGE. FIRST EXAMINATION FOR THE DEGREE OF B. Sc. HONOURS LEVEL I SECOND SEMESTER EXAMINATION
UNIVERSITY OF SIERRA LEONE FOURAH BAY COLLEGE CHEM 121 INSTRUCTIONS: FIRST EXAMINATION FOR THE DEGREE OF B. Sc. HONOURS LEVEL I SECOND SEMESTER EXAMINATION WEDNESDAY 12 th SEPTEMBER 2018 13.30 16.45 CHEM
More informationAdditional Calculations: 10. How many joules are required to change the temperature of 80.0 g of water from 23.3 C to 38.8 C?
Additional Calculations: 10. How many joules are required to change the temperature of 80.0 g of water from 23.3 C to 38.8 C? q = m C T 80 g (4.18 J/gC)(38.8-23.3C) = 5183 J 11. A piece of metal weighing
More informationName AP CHEM / / Collected Essays Chapter 17
Name AP CHEM / / Collected Essays Chapter 17 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the reaction
More information2) C 2 H 2 (g) + 2 H 2 (g) ---> C 2 H 6 (g) Information about the substances
Thermochemistry 1) 2 C 4 H 10 (g) + 13 O 2 (g) ------> 8 CO 2 (g) + 10 H 2 O(l) The reaction represented above is spontaneous at 25 C. Assume that all reactants and products are in their standard states.
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 informationCHEM 1423 Chapter 17 Homework Questions TEXTBOOK HOMEWORK
CHEM 1423 Chapter 17 Homework Questions TEXTBOOK HOMEWORK 17.29 At 425 o C, Kp = 4.18x10-9 for the reaction 2HBr(g) H 2 (g) + Br 2 (g) In one experiment, 0.20 atm of HBr(g), 0.010 atm of H 2 (g), and 0.010
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 informationAP Chemistry. Free-Response Questions
2018 AP Chemistry Free-Response Questions College Board, Advanced Placement Program, AP, AP Central, and the acorn logo are registered trademarks of the College Board. AP Central is the official online
More informationName: Kinetics & Thermodynamics Date: Review
Name: Kinetics & Thermodynamics Date: Review 1. What is required for a chemical reaction to occur? A) standard temperature and pressure B) a catalyst added to the reaction system C) effective collisions
More informationChapter 11 Thermochemistry Heat and Chemical Change
Chemistry/ PEP Name: Date: Chapter 11 Thermochemistry Heat and Chemical Change Chapter 11:1 35, 57, 60, 61, 71 Section 11.1 The Flow of Energy - Heat 1. When 435 of heat is added to 3.4 g of olive oil
More 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 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 informationMultiple Choices: The red color is the correct answer
Multiple Choices: The red color is the correct answer 1. 2. 3. 4. 5. Which one of the following thermodynamic quantities is not a state function? (a) Gibbs free energy (b) enthalpy (c) entropy (d) internal
More informationKinetic energy is the energy of motion (of particles). Potential energy involves stored energy (energy locked up in chemical bonds)
Enthalpy (H) Enthalpy (H) is the total energy amount (Epotential + Ekinetic) of a system during a chemical reaction under constant temperature and pressure conditions. Kinetic energy is the energy of motion
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 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 informationQ1. (a) Explain the meaning of the terms mean bond enthalpy and standard enthalpy of formation. Mean bond enthalpy
Q1. (a) Explain the meaning of the terms mean bond enthalpy and standard enthalpy of formation. Mean bond enthalpy......... Standard enthalpy of formation............ (5) (b) Some mean bond enthalpies
More informationEntropy, Free Energy, and Equilibrium
Entropy, Free Energy, and Equilibrium Chapter 17 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Spontaneous Physical and Chemical Processes A waterfall runs
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
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 information3.2 Calorimetry and Enthalpy
3.2 Calorimetry and Enthalpy Heat Capacity Specific heat capacity (c) is the quantity of thermal energy required to raise the temperature of 1 g of a substance by 1 C. The SI units for specific heat capacity
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 informationCHEMISTRY. Section II (Total time 95 minutes) Part A Time 55 minutes YOU MAY USE YOUR CALCULATOR FOR PART A.
CHEMISTRY Section II (Total time 95 minutes) Part A Time 55 minutes YOU MAY USE YOUR CALCULATOR FOR PART A. CLEARLY SHOW THE METHOD USED AND THE STEPS INVOLVED IN ARRIVING AT YOUR ANSWERS. It is to your
More information(03) WMP/Jun10/CHEM4
Thermodynamics 3 Section A Answer all questions in the spaces provided. 1 A reaction mechanism is a series of steps by which an overall reaction may proceed. The reactions occurring in these steps may
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 informationWrite equilibrium law expressions from balanced chemical equations for heterogeneous and homogeneous systems. Include: mass action expression.
Equilibrium 1 UNIT 3: EQUILIBRIUM OUTCOMES All important vocabulary is in Italics and bold. Relate the concept of equilibrium to physical and chemical systems. Include: conditions necessary to achieve
More information8. A piece of Mg(s) ribbon is held in a Bunsen burner flame and begins to burn according to the equation: 2Mg(s) + O2 (g) 2MgO(s).
1. Which event must always occur for a chemical reaction to take place? A) formation of a precipitate B) formation of a gas C) effective collisions between reacting particles D) addition of a catalyst
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 2 Pre-Test Reaction Equilibrium
Unit 2 Pre-Test Reaction Equilibrium Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Consider the following equilibrium system: 2HF(g) F 2(g) + H 2 (g)
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 informationAS Paper 1 and 2 Energetics
AS Paper 1 and 2 Energetics Q1.Nitric acid is produced industrially from ammonia, air and water using the following sequence of reactions: 4NH 3 (g) + 5O 2(g) 4NO(g) + 6H 2O(g) H = 909 kj mol 1 (2) 2NO(g)
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 informationChemistry 30: Thermochemistry. Practice Problems
Name: Period: Chemistry 30: Thermochemistry Practice Problems Date: Heat and Temperature 1. Pretend you are doing a scientific study on the planet Earth. a. Name three things in the system you are studying.
More 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 informationSlide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c
Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system
More 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 informationName: Section: Score: /10 PRE LABORATORY ASSIGNMENT EXPERIMENT 7
Name: Section: Score: /10 PRE LABORATORY ASSIGNMENT EXPERIMENT 7 1. Is the sign of Δ r H for an exothermic reaction positive or negative? Why? 2. When 4.21 grams of potassium hydroxide are added to 250.
More information(for tutoring, homework help, or help with online classes) 1.
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. 2. Consider the following processes used to produce energy. Which does not predominantly use potential energy? 1. Fossil
More informationChapter 7: Stoichiometry in Chemical Reactions
Chapter 7: Stoichiometry in Chemical Reactions Mini Investigation: Precipitating Ratios, page 315 A. ZnCl 2 (aq) + Na 2 CO 3 (aq) ZnCO 3 (s) + 2 NaCl(aq) 3 AgNO 3 (aq) + Na 3 PO 4 (aq) Ag 3 PO 4 (s) +
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 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 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 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 informationAP Questions: Electrochemistry
AP Questions: Electrochemistry I 2 + 2 S 2O 2-3 2 I - + S 4O 2-6 How many moles of I 2 was produced during the electrolysis? The hydrogen gas produced at the cathode during the electrolysis was collected
More informationCollision Theory. Unit 12: Chapter 18. Reaction Rates. Activation Energy. Reversible Reactions. Reversible Reactions. Reaction Rates and Equilibrium
Collision Theory For reactions to occur collisions between particles must have Unit 12: Chapter 18 Reaction Rates and Equilibrium the proper orientation enough kinetic energy See Both In Action 1 2 Activation
More information1. As the number of effective collisions between reacting particles increases, the rate of reaction (1) decreases (3) remains the same (2) increases
1. As the number of effective collisions between reacting particles increases, the rate of reaction (1) decreases (3) remains the same (2) increases 2. The energy needed to start a chemical reaction is
More information1 A reaction that is spontaneous.
Slide 1 / 55 1 A reaction that is spontaneous. A B C D E is very rapid will proceed without outside intervention is also spontaneous in the reverse direction has an equilibrium position that lies far to
More 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 informationThermochemistry HW. PSI Chemistry
Thermochemistry HW PSI Chemistry Name Energy 1) Objects can possess energy as: (a) endothermic energy (b) potential energy A) a only B) b only C) c only D) a and c E) b and c (c) kinetic energy 2) The
More informationK P VERSUS K C PROPERTIES OF THE EQUILIBRIUM CONSTANT
K P VERSUS K C 1. What are the units of K p and K c for each of the following? a) 2H 2 S(g) 2H 2 (g) + S 2 (g) b) 4NH 3 (g) + 3O 2 (g) 2N 2 (g) + 6H 2 O(g) 2. What are the units of K p and K c for each
More informationThermochemistry Notes
Name: Thermochemistry Notes I. Thermochemistry deals with the changes in energy that accompany a chemical reaction. Energy is measured in a quantity called enthalpy, represented as H. The change in energy
More informationEnd of Year Review ANSWERS 1. Example of an appropriate and complete solution H = 70.0 g 4.19 J/g C T = 29.8 C 22.4 C 7.4 C
End of Year Review ANSWERS 1. Example of an appropriate and complete solution H = mc T mol HCl m = 70.0 g c = 4.19 J/g C T = 9.8 C.4 C = 7.4 C mol HCl = 3.00 mol/ 0.000 = 0.0600 mol H = 70.0 g 4.19 J/g
More informationEnthalpy, Entropy, and Free Energy Calculations
Adapted from PLTL The energies of our system will decay, the glory of the sun will be dimmed, and the earth, tideless and inert, will no longer tolerate the race which has for a moment disturbed its solitude.
More informationCHEMISTRY 110 Final EXAM Dec 17, 2012 FORM A
CEMISTRY 110 Final EXAM Dec 17, 2012 FORM A 1. Given the following reaction which of the following statements is true? Fe(s) + CuCl 2 (aq)! Cu(s) + FeCl 2 (aq) A. Iron is oxidized and copper is reduced.
More information8. The table below describes two different reactions in which Reaction 1 is faster. What accounts for this observation? Reaction 1 Reaction 2.
Public Review - Rates and Equilibrium June 2005 1. What does X represent in the diagram below? (A) activation energy for the forward reaction (B) activation energy for the reverse reaction (C) heat of
More informationCHE 105 Fall 2016 Exam 3
CHE 105 Fall 2016 Exam 3 Your Name: Your ID: Question #: 1 Samples of CO2(g), C6H6(g), Cl2(g) and C3H8(g) are placed in separate glass vessels (only one gas to a vessel) at the same temperature and pressure.
More informationCHEMpossible. Final Exam Review
CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a
More informationExam 3, Ch 7, 19, 14 November 9, Points
Chem 30 Name Exam 3, Ch 7, 9, 4 November 9, 206 00 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More informationCHAPTER 20 THERMODYNAMICS: ENTROPY, FREE ENERGY, AND THE DIRECTION OF CHEMICAL REACTIONS
CHAPTER 0 THERMODYNAMICS: ENTROPY, FREE ENERGY, AND THE DIRECTION OF CHEMICAL REACTIONS FOLLOW UP PROBLEMS 0.1A Plan: Particles with more freedom of motion have higher entropy. In general the entropy of
More informationChapter 6 Energy and Chemical Change. Brady and Senese 5th Edition
Chapter 6 Energy and Chemical Change Brady and Senese 5th Edition Index 6.1 An object has energy if it is capable of doing work 6.2 Internal energy is the total energy of an object s molecules 6.3 Heat
More informationBonus Final Exam 3. 1 Calculate the heat of reaction,δh 0 rxn, for the following reaction as written at 298 K: g 2H 2 CH 4. g CF 4.
Bonus Final Exam 3 1 Calculate the heat of reaction,δh rxn, for the following reaction as written at 298 K: CH 4 2F 2 CF 4 2H 2 substance CH 4 CF 4 ΔH f kj/mol 75 68 (A) ΔH rxn 23 kj (B) ΔH rxn 914 kj
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 informationChapter 3. Thermochemistry: Energy Flow and Chemical Change. 5.1 Forms of Energy and Their Interconversion
Chapter 3 Thermochemistry: Energy Flow and Chemical Change 5.1 Forms of Energy and Their Interconversion 5.2 Enthalpy: Chemical Change at Constant Pressure 5.3 Calorimetry: Measuring the Heat of a Chemical
More 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 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 informationCHEMISTRY 12 UNIT II EQUILIBRIUM D Learning Goals
CHEMISTRY 12 UNIT II EQUILIBRIUM D Learning Goals 1. Chemical equilibrium is said to by dynamic because a. The reaction proceeds quickly b. The mass of the reactants is decreasing c. The macroscopic properties
More informationLecture 2. Review of Basic Concepts
Lecture 2 Review of Basic Concepts Thermochemistry Enthalpy H heat content H Changes with all physical and chemical changes H Standard enthalpy (25 C, 1 atm) (H=O for all elements in their standard forms
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 informationNo Brain Too Small CHEMISTRY AS91390 Demonstrate understanding of thermochemical principles and the properties of particles and substances
COLLATED QUESTIONS Hess s Law including application of ΔrH = Σ fh((products) Σ fh(reactants)) and related calculations. 2018:2 (i) The equation for the combustion of propan-1-ol is: C3H7OH(l) + 4.5O2(g)
More information6. Which will react faster: Magnesium and 2M hydrochloric acid, or Magnesium and 0.5M hydrochloric acid?
REACTION RATES WORKSHEET WS#1 1. Identify the three components of collision theory. What are the three factors that must be true for a collision to be successful? a. b. c. 2. Do all collisions result in
More informationCHEMISTRY Practice Exam #2
CHEMISTRY 1710 - Practice Exam #2 Section 1 - This section of the exam is multiple choice. Choose the BEST answer from the choices which are given. 1. Which of the following solutions will have the highest
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 informationCHEM J-11 June /01(a)
CHEM1001 2014-J-11 June 2014 22/01(a) Combustion of 15.0 g of coal provided sufficient heat to increase the temperature of 7.5 kg of water from 286 K to 298 K. Calculate the amount of heat (in kj) absorbed
More informationf) Perchloric acid g) Dihydrogen sulfide i) Barium phosphate j) Copper(II) sulfate pentahydrate
1 2 1. For the following provide the correct name or formula. [8] a) Hg2(NO3)2 b) Mg(C2H3O2)2 c) (NH4)2CO3 d) Ca(OH)2 f) Perchloric acid g) Dihydrogen sulfide i) Barium phosphate j) Copper(II) sulfate
More informationCHAPTER 12: Thermodynamics Why Chemical Reactions Happen
CHAPTER 12: Thermodynamics Why Chemical Reactions Happen Useful energy is being "degraded" in the form of unusable heat, light, etc. A tiny fraction of the sun's energy is used to produce complicated,
More information6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.
CH141 Practice Problems/Practice Final Exam Page 1 of 12 Name: 1. What is the SO 4 2- concentration of a solution prepared by dissolving 3.00 g of Na 2 SO 4 in 1.00 L of water? 2. What is the hybridization
More information(B) K2O potassium dioxide
PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium
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 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 information33. a. Heat is absorbed from the water (it gets colder) as KBr dissolves, so this is an endothermic process.
31. This is an endothermic reaction so heat must be absorbed in order to convert reactants into products. The high temperature environment of internal combustion engines provides the heat. 33. a. Heat
More 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 informationc) Explain the observations in terms of the DYNAMIC NATURE of the equilibrium system.
Chemical Equilibrium - Part A: 1. At 25 o C and 101.3 kpa one mole of hydrogen gas and one mol of chlorine gas are reacted in a stoppered reaction vessel. After a certain time, three gases are detected
More information