Workbook 5. Chem 1A Dr. White 1

Size: px
Start display at page:

Download "Workbook 5. Chem 1A Dr. White 1"

Transcription

1 Chem 1A Dr. White 1 Workbook 5 5-1: Dalton s Law, KMT, Effusion/Diffusion/Real Gases 1. What is the total pressure and the partial pressure of each gas (in atm) in a mixture of 3.2 g of O 2, 1.6 g of CH 4 and 6.4 g of S 2 in an 11.2 L container at 273 C? 2. What is the partial pressure of He (in atm) in a mixture of 1.0 g H 2 and 5.0 g He in a 5.0 L cylinder at 20.0 o C? 3. A g sample of impure calcium carbide reacts with water to give 561 ml of C 2 H 2 collected by water displacement at 20 C and 745 mm Hg. The vapor pressure of water is 17.5 mm Hg. What is the % CaC 2? CaC 2 (s) + 2 H 2 O(l) Ca(OH) 2 (s) + C 2 H 2 (g) 4. A 3.00 g sample of a mixture contains copper and zinc. Zinc reacts with HCl but copper does not. What is the % Zn if 927 ml of hydrogen gas is collected over water at 740 mm Hg and 20 C. The vapor pressure of water is 17.5 mm Hg. 5. In an apparatus, helium effuses at the rate of 15 ml/min. At what rate will xenon effuse in the same apparatus? 6. In an effusion apparatus, H 2 is found to effuse at the rate of 5.9 ml/s. Another gas in the same apparatus effuses at the rate of 0.55 ml/s. What is the molar mass of the gas? 7. The van der Waals constants a and b are L 2 atm mole -2 and L mole -1 for Xe. Calculate the observed pressure for 1.25 moles of the compound in a L flask at 75 C. 8. The van der Waals constants a and b are L 2 atm mole -2 and L mole -1 for NH 3. Calculate the pressure (atm) of a 2.00 moles sample of NH 3 in a 2.95 L flask at 47 o C. 9. The Ne atom has 10 times the mass of H 2. Which of the following statements is true? I. At 25 C they both have the same kinetic energy. II. Ten moles of H 2 would have the same volume as 1 mole of Ne. III. One mole of Ne exerts the same pressure as one mole of H 2 at STP. IV. A H 2 molecule effuses 10 times faster than a Ne atom. 10. Real gases approach ideal gas behavior at: (chose one) a) high pressure and low temperature b) low pressure and low temperature c) low pressure and high temperature d) high pressure and high temperature 5-2: Bond Energies and Calorimetry 1. Use the bond energies in the table in your handout to calculate ΔE for the following reactions (suggestion: draw Lewis structures first): (a) CH 4 + Cl 2 CH 3 Cl + HCl (b) CH 3 CH 2 OH + 3 O 2 2 CO H 2 O

2 Chem 1A Dr. White 2 2. How much heat is required to raise 335 g of water from 20.0 C to 95.5 C? 3. A 36.9 g sample of metal is heated to C, and then added to a calorimeter containing g of water at 23.1 C. The temperature of the water rises to a maximum of 25.2 C before cooling back down. Did the water absorb heat or did it release heat? How many joules of heat was exchanged between the water and the metal? 4. When 1.00 g of solid NH 4 Cl is dissolved in g water contained in a coffee cup calorimeter, both reagents initially being at 25.0 C, the temperature falls to 22.4 C. Calculate the heat (enthalpy) of solution of NH 4 Cl, (a) in J/g and (b) in kj/mol g of solid NaOH is dissolved in g water in a coffee cup calorimeter, all the reagents initially being at 20.0 C. Calculate the final temperature of the solution obtained, given the following information: NaOH(s) NaOH(aq) ΔH soln = kj 6. The reaction 2NaOH(aq) + H 2 SO 4 (aq) Na 2 SO 4 (aq) + 2H 2 O(l) was studied in a coffee cup calorimeter ml portions of 1.00 M aqueous NaOH and H 2 SO 4, each at 24.0 C, were mixed. The maximum temperature achieved was 30.6 C. Neglect the heat capacity of the cup and the thermometer, and assume that the solution of products has a density of exactly 1 g/ml. Calculate ΔH, the heat (enthalpy) of reaction, in kj/mol of Na 2 SO 4 produced. 7. A mass of g of benzoic acid (C 7 H 6 O 2 ) was completely combusted in a bomb calorimeter. If the heat capacity of the calorimeter was kj/k and the heat of combustion of benzoic acid is kj/mol, calculate (to three decimal places) the temperature increase that should have occurred in the apparatus. 8. A common laboratory reaction is the neutralization of an acid with a base. When 50.0 ml of M HCl at 25.0 C is added to 50.0 ml of M NaOH at 25.0 C in a coffee cup calorimeter, the temperature of the mixture rises to 28.2 C. What is the heat of reaction per mole of acid? Assume that the densities of the reactant solutions are both 1.00 g/ml 9. A 5.00 g sample of HNO 3 is dissolved in water in a calorimeter whose heat capacity is 5.16 kj/ o K. The temperature increases o K. Calculate the heat released (kj) per mole of HNO 3 dissolved. 10. When 2.62 g of lactic acid, C 3 H 6 O 3, is burned in a calorimeter whose heat capacity is 21.7 kj/ o K, the temperature increases by o K. Calculate the heat released by the combustion of lactic acid in kj per mole. 5-3: Thermochemical Stoichiometry & Hess Law 1. Calcium hydroxide, which reacts with carbon dioxide to form calcium carbonate, was used by the ancient Romans as mortar in stone structures. The reaction for this process is Ca(OH) 2 (s) + CO 2 (g) CaCO 3 (s) + H 2 O(g) ΔH = kj What is the enthalpy change if 3.8 mol of calcium carbonate is formed? 2. The highly exothermic thermite reaction, in which aluminum reduces iron(iii) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2Al(s) + Fe 2 O 3 (s) 2Fe(s) + Al 2 O 3 (s) ΔH = -8.5 x 10 2 kj. What mass of iron is formed when 725 kj of heat are released?

3 Chem 1A Dr. White 3 3. Triglycerides are the main form in which fats are stored in the body. During periods of starvation, a person s fat stores are used for energy. Tristearin (C 57 H 110 O 6 ) is a typical animal fat that is oxidized according to the following thermochemical equation: 2C 57 H 110 O 6 (s) O 2 (g) 114 CO 2 (g) H 2 O (l) ΔH rxn = -7.0 x 10 4 kj a. How much heat is released per gram of tristearin oxidized? b. When 325 L of O 2 at 37 C and 755 torr is used, how many grams of tristearin can be oxidized? c. When 325 L of O 2 at 37 C and 755 torr is used, how many kj of heat are released? 4. The reaction of barium metal with liquid water produces kj of heat for every mole of barium that reacts. (a) Write a complete balanced thermochemical equation for this reaction. (b) Is this reaction endothermic of exothermic? (c) Calculate the amount of heat associated with 3.65 g of water reacting at constant pressure. Make sure your answer has the proper sign! (d) How many grams of barium metal must react to produce 586 kj of heat? 5. Pure liquid octane (C 8 H 18, d= 0.702g/mL) is used as the fuel in a test of a new automobile drive train. a. How much energy is produced (in kj) when a tank full (20.4gal) is combusted? ΔH comb = -5.45x10 3 kj/mol)? (Start with a balanced equation for the combustion of one mole of octane.) b. The energy delivered at the wheels at 65mph is 5.5x 10 4 kj/hr. Assuming that all the energy is transferred to the wheels, what is the cruising range of the car (in km) on a full tank? 6. Calculate the enthalpy change for the reaction NO(g) + O(g) NO 2 (g) from the following data: NO(g) + O 3 (g) NO 2 (g) + O 2 (g) ΔH = kj O 3 (g) 1.5O 2 (g) ΔH = kj O 2 (g) 2O(g) ΔH = kj (Note: O is NOT stable, as you know, and exists for a very short amount of time) 7. Use the thermochemical equations shown below to determine the enthalpy for the reaction: H 2 O(l) H 2 (g) + 1/2O 2 (g) C(s) + O 2 (g) CO 2 (g) CO 2 (g) + 2H 2 O(l) CH 4 (g) + 2O 2 (g) C(s) + 2H 2 (g) CH 4 (g) ΔH=-590.2KJ ΔH=1335.7KJ ΔH=-112.2KJ

4 Chem 1A Dr. White 4 8. One problem with using hydrogen as a fuel is producing enough hydrogen efficiently. One series of reactions being studied has as its net reaction the splitting of liquid water: H 2 O (l) H 2 (g) + 1/2 O 2 (g) ΔH rxn = kj This series of reactions involves each of the following steps in some form. Use Hess s Law to calculate the missing ΔH rxn. H 2 (g) + I 2 (g) 2HI (g) ΔH rxn = kj H 2 O (l) + 1/2 SO 2 (g) +1/2 I 2 (g) 1/2 H 2 SO 4 (aq) + HI (g) ΔH rxn =? 2 H 2 O (l) + 2 SO 2 (g) + O 2 (g) 2 H 2 SO 4 (aq) ΔH rxn = kj (NOTE that this particular system is inefficient as one reaction requires a temperature of 825 C. The goal of research in this area is to find a system that requires low enough temperatures that sunlight can be used as an energy source) 5-4: Heats of Formation & The Born Haber Cycle 1. a. Define, or explain fully what is meant by the standard enthalpy of formation of a substance, ΔH f. b. What is the standard state of the element oxygen? c. Write down in full the formation reaction for liquid ethanol, C 2 H 5 OH(l). The equation should be balanced and should indicate the physical state of each substance. 2. Write balanced chemical reactions for the formation of one mole of each of the following compounds from its elements in their standard states: a) Liquid water b) Aqueous strontium nitrate c) Solid iron (III) bromide d) Solid aluminum oxide e) Solid magnesium phosphate 3. Lithium fluoride is formed from lithium and fluorine. Its lattice energy may be calculated from a Born-Haber cycle using the following experimental data. i. Li (g) Li + (g) + e - ΔH= +520 kj ii. Li (s) Li (g) ΔH= +161 kj iii. Li(s) + ½ F 2 (g) LiF (s) ΔH = -617 kj iv. F 2 (g) 2F(g) ΔH= +159 kj v. F(g) + e - F - (g) ΔH = -328 kj a. Which reaction above refers to the heat of formation for lithium fluoride? b. Which reaction above refers to an electron affinity rection? c. Which reaction above refers to a bond energy? d. Write the reaction that refers to the lattice energy of LiF (s). e. Calculate the lattice energy of lithium fluoride.

5 Chem 1A Dr. White 5 4. Nitric acid, which is among the top 15 chemicals produced in the United States, was first prepared over 1200 years ago by heating naturally occurring sodium nitrate (called saltpeter) with sulfuric acid and collecting the vapors produced. Calculate ΔH rxn for this reaction. ΔH f [NaNO 3 (s)] = kj/mol; ΔH f [NaHSO 4 (s)] = kj/mol; ΔH f [H 2 SO 4 (l) = kj/mol; ΔH f [HNO 3 (g)] = kj/mol NaNO 3 (s) + H 2 SO 4 (l) NaHSO 4 (s) + HNO 3 (g) 5. The space shuttle orbiter uses the oxidation of methyl hydrazine by dinitrogen tetroxide for propulsion. The unbalanced reaction is as follows: N 2 H 3 CH 3 (l) + N 2 O 4 (l) H 2 (g) + N 2 (g) + CO 2 (g) a) Balance this equation b) Calculate ΔH rxn for this reaction using the following info: Substance ΔH f (kj/mol) N 2 O 4 (g) 9.16 N 2 O 4 (l) N 2 H 3 CH 3 (l) 54.0 CO (g) CO 2 (aq) CO 2 (g) a. Write a balanced equation for the combustion of benzene, C 6 H 6 (l) in oxygen. b. The standard heat of combustion of benzene is kj/mol. Calculate its standard heat of formation, ΔH f, given the data: ΔH f [CO 2 (g)] = -394 kj; ΔH f [H 2 O(l)] = -286 kj 7. Lightweight camp stoves often make use of a mixture of C 5 and C 6 liquid hydrocarbons (a fuel called white gas. ) a. Write the reaction for the combustion of C 5 H 12 (l) and determine the standard heat of formation of C 5 H 12 (l) if the standard heat of combustion is kj per mole of C 5 H 12. The ΔH f [CO 2 (g)] = kj/mol and The ΔH f [H 2 O(g)] = kj/mol. b. How much heat is produced by the complete combustion of 3.00 L of C 5 H 12 (l) if the density of C 5 H 12 (l) = g/ml? 5-5: Heat, Work, and the First Law of Thermodynamics 1. What are the two main components of internal energy of a substance? What are the symbols for internal energy and its two components? 2. A system which undergoes an adiabatic change is one in which no heat is transferred. For an adiabatic change that does work on its surroundings, indicate if q, w and ΔE for such a process should be positive, negative, or equal to zero. Explain.

6 Chem 1A Dr. White 6 3. For each of the following, define the system and the surroundings, and indicate the direction of heat transfer. a) Natural gas is burned in a gas furnace in your home. b) Water drops, sitting on your skin after a dip in the pool, evaporate 4. A system delivers 200. J of pressure-volume work against the surroundings while releasing 300. J of heat energy. What is the change in the internal energy of the system? 5. The work done when a gas is compressed in a cylinder is 199 J. A heat transfer of 270 J occurs from the surrounding to the gas. Calculate E of the gas in J. 6. One mole of a gas at 25 o C expands in volume from 1.0 L to 4.0 L at constant temperature. What work (J) is done if the gas expands against an external pressure of 3.0 atm? 7. One mole of a gas at 25 o C expands in volume from 2.0 L to 6.0 L at constant temperature. What work is done if the gas expands against an external pressure of 0.75 atm? moles of a gas with a molar heat capacity of 5.75 J/mol C are placed in a 1.50 L container at 25.0 C. The temperature increases from 25.0 C to 31.0 C, and the container expands to 2.75 L against a pressure of 1.02 atm. Calculate q, w, ΔE, and ΔH for the gas. 5-1: Dalton s Law, KMT, Effusion/Diffusion/Real Gases 1. P total = 1.2 atm, partial pressure of each = 0.40 atm atm % % ml/min x 10 2 g/mol atm atm 9. I. TRUE II. FALSE III. TRUE IV. FALSE 10. C 5-2: Bond Energies & Calorimetry 1. a x 10 2 kj b kj x 10 5 J 3. absorbs, 1.24 x 10 3 J 4. a. 2.8 x 10 2 J/g b. 15 kj/mol C 6. a J b kj/mol Na 2 SO 4 7. Temperature increase is K (or C) kj/mol kj/mol x 10 3 kj/mol x 10 2 kj g 5-3: Thermochemical Stoichiometry & Hess Law

7 Chem 1A Dr. White 7 3. a. -39 kj/g b. 138 g c x 10 3 g 4. a. Ba(s) + 2H 2 O (l) Ba(OH) 2 (aq) + H 2 (g) ΔH rxn = kj b. exothermic c kj d. 122 g 5. a x 10 6 kj b. 4.9 x 10 3 km kj kj kj 5-4: Heats of Formation & The Born Haber Cycle 1. a. ΔH f is the enthalpy change accompanying the formation of one mole of a substance from its elements, all substances being in their standard states. b. Pure O 2 gas at a pressure of 1 atm and a specified temperature. c. 2C(graphite) + 3H 2 (g) + ½O 2 (g) C 2 H 5 OH(l) 2. a. ½ O 2 (g) + H 2 (g) H 2 O (l)) b. Sr(s) + N 2 (g) +3 O 2 (g) Sr(NO 3 ) 2 (aq) c. Fe (s) +3/2 Br 2 (l) FeBr 3 (s) d. 2Al (s) + 3/2 O 2 (g) Al 2 O 3 (s) e. 3Mg (s) + ½ P 4 (s) + 4O 2 (g) Mg 3 (PO 4 ) 2 (s) 3. a. rxn iii b. rxn v c. rxn iv d. Li + (g) + F - (g) LiF (s) e kj kj 5. a. 2 N 2 H 3 CH 3 (l) + N 2 O 4 (l) -> 6H 2 (g) + 3 N 2 (g) +2CO 2 (g) b kj 6. a. C 6 H 6 (l) + 15/2 O 2 (g) 6CO 2 (g) + 3H 2 O (l) b. 49 kj 7. a. 122 kj/mol b x 10 4 kj 5-5: Heat, Work, and the First Law of Thermodynamics 1. Internal energy (E) is composed Heat (q) and work (w). 2. q = 0 (no heat is exchanged), w = - (energy lost from the system as work), ΔE = - (since ΔE = q + w and q is 0) 3. a. System burning of gas Surroundings everything else (furnace, home and the entire rest of the universe) Heat transferred from the system to surroundings (-q) b. System water drops Surroundings everything else Heat transferred from the surroundings to system (+q) (this is why your skin part of the surroundings feels cool when sweat or water evaporates) J J x 10 2 J x 10 2 J 8. q = ΔH = 17 J w = -129 J ΔE = -112 J

8 Chem 1A Dr. White 8

(a) graph Y versus X (b) graph Y versus 1/X

(a) graph Y versus X (b) graph Y versus 1/X HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below

More information

EXTRA HOMEWORK 5A 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below is determined with

More information

Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c

Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system

More information

Chapter 3. Thermochemistry: Energy Flow and Chemical Change. 5.1 Forms of Energy and Their Interconversion

Chapter 3. Thermochemistry: Energy Flow and Chemical Change. 5.1 Forms of Energy and Their Interconversion Chapter 3 Thermochemistry: Energy Flow and Chemical Change 5.1 Forms of Energy and Their Interconversion 5.2 Enthalpy: Chemical Change at Constant Pressure 5.3 Calorimetry: Measuring the Heat of a Chemical

More information

Enthalpies of Reaction

Enthalpies of Reaction Enthalpies of Reaction Enthalpy is an extensive property Magnitude of H is directly related to the amount of reactant used up in a process. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) H = 890 kj 2CH 4 (g)

More information

Thermochemistry HW. PSI Chemistry

Thermochemistry HW. PSI Chemistry Thermochemistry HW PSI Chemistry Name Energy 1) Objects can possess energy as: (a) endothermic energy (b) potential energy A) a only B) b only C) c only D) a and c E) b and c (c) kinetic energy 2) The

More information

Thermochemistry: Heat and Chemical Change

Thermochemistry: Heat and Chemical Change Thermochemistry: Heat and Chemical Change 1 Heat or Thermal Energy (q) Heat is a form of energy Is heat the same as temperature? Heat flows between two objects at different temperatures. Hot Cold 2 Chemical

More information

Chemistry 30: Thermochemistry. Practice Problems

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

More information

Name: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry

Name: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical

More information

CHEM J-11 June /01(a)

CHEM 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 information

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

Chapter 6 Energy and Chemical Change. Brady and Senese 5th Edition Chapter 6 Energy and Chemical Change Brady and Senese 5th Edition Index 6.1 An object has energy if it is capable of doing work 6.2 Internal energy is the total energy of an object s molecules 6.3 Heat

More information

Brown, LeMay Ch 5 AP Chemistry Monta Vista High School

Brown, LeMay Ch 5 AP Chemistry Monta Vista High School Brown, LeMay Ch 5 AP Chemistry Monta Vista High School 1 From Greek therme (heat); study of energy changes in chemical reactions Energy: capacity do work or transfer heat Joules (J), kilo joules (kj) or

More information

Thermochemistry. Chapter 6. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Thermochemistry. Chapter 6. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Thermochemistry Chapter 6 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Energy is the capacity to do work. Radiant energy comes from the sun and is earth s

More information

Chapter 5. Thermochemistry

Chapter 5. Thermochemistry Chapter 5 Thermochemistry Dr. A. Al-Saadi 1 Preview Introduction to thermochemistry: Potential energy and kinetic energy. Chemical energy. Internal energy, work and heat. Exothermic vs. endothermic reactions.

More information

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is

More information

Selected Questions on Chapter 5 Thermochemistry

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

More information

CHEM 1105 S10 March 11 & 14, 2014

CHEM 1105 S10 March 11 & 14, 2014 CHEM 1105 S10 March 11 & 14, 2014 Today s topics: Thermochemistry (Chapter 6) Basic definitions Calorimetry Enthalpy Thermochemical equations Calculating heats of reaction Hess s Law Energy and Heat Some

More information

Thermochemistry: Energy Flow and Chemical Reactions

Thermochemistry: Energy Flow and Chemical Reactions Thermochemistry: Energy Flow and Chemical Reactions Outline thermodynamics internal energy definition, first law enthalpy definition, energy diagrams, calorimetry, theoretical calculation (heats of formation

More information

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

Thermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation THERMOCHEMISTRY Thermochemistry Energy 1st Law of Thermodynamics Enthalpy / Calorimetry Hess' Law Enthalpy of Formation The Nature of Energy Kinetic Energy and Potential Energy Kinetic energy is the energy

More information

Chapter 5 Practice Multiple Choice & Free

Chapter 5 Practice Multiple Choice & Free Name Response 1. A system has an increase in internal energy, E, of 40 kj. If 20 kj of work, w, is done on the system, what is the heat change, q? a) +60 kj d) -20 kj b) +40 kj e) -60 kj c) +20 kj 2. Which

More information

THERMOCHEMISTRY & DEFINITIONS

THERMOCHEMISTRY & DEFINITIONS THERMOCHEMISTRY & DEFINITIONS Thermochemistry is the study of the study of relationships between chemistry and energy. All chemical changes and many physical changes involve exchange of energy with the

More information

3.2 Calorimetry and Enthalpy

3.2 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 information

Topic 05 Energetics : Heat Change. IB Chemistry T05D01

Topic 05 Energetics : Heat Change. IB Chemistry T05D01 Topic 05 Energetics 5.1-5.2: Heat Change IB Chemistry T05D01 5.1 Exothermic and endothermic reactions - 1 hour 5.1.1 Define the terms exothermic reaction, endothermic reaction and standard enthalpy change

More information

Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes

Thermochemistry: 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 information

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

Ch 6. Energy and Chemical Change. Brady & Senese, 5th Ed. Ch 6. Energy and Chemical Change Brady & Senese, 5th Ed. Energy Is The Ability To Do Work Energy is the ability to do work (move mass over a distance) or transfer heat Types: kinetic and potential kinetic:

More information

Chapter 6 Thermochemistry 許富銀

Chapter 6 Thermochemistry 許富銀 Chapter 6 Thermochemistry 許富銀 6.1 Chemical Hand Warmers Thermochemistry: the study of the relationships between chemistry and energy Hand warmers use the oxidation of iron as the exothermic reaction: Nature

More information

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

June Which is a closed system? (A) burning candle (B) halogen lightbulb (C) hot water in a sink (D) ripening banana June 2005 28. Which is a closed system? burning candle halogen lightbulb hot water in a sink ripening banana 29. Which involves the greatest energy change? chemical reaction nuclear reaction phase change

More information

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided

More information

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

The Nature of Energy. Chapter Six: Kinetic vs. Potential Energy. Energy and Work. Temperature vs. Heat The Nature of Energy Chapter Six: THERMOCHEMISTRY Thermodynamics is the study of energy and its transformations. Thermochemistry is the study of the relationship between chemical reactions and energy changes

More information

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

First Law of Thermodynamics: energy cannot be created or destroyed. 1 CHEMICAL THERMODYNAMICS ANSWERS energy = anything that has the capacity to do work work = force acting over a distance Energy (E) = Work = Force x Distance First Law of Thermodynamics: energy cannot

More information

CHEM 101 Fall 09 Final Exam (a)

CHEM 101 Fall 09 Final Exam (a) CHEM 101 Fall 09 Final Exam (a) On the answer sheet (scantron) write your name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on

More information

Chapter 5 Thermochemistry

Chapter 5 Thermochemistry Chapter 5 Thermochemistry Learning Outcomes: Interconvert energy units Distinguish between the system and the surroundings in thermodynamics Calculate internal energy from heat and work and state sign

More information

1.4 Enthalpy. What is chemical 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 information

AP Chapter 6: Thermochemistry Name

AP Chapter 6: Thermochemistry Name AP Chapter 6: Thermochemistry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 6: Thermochemistry 2 Warm-Ups (Show your work for credit)

More information

Thermodynamics I. Prep Session

Thermodynamics I. Prep Session Thermodynamics I Prep Session Dr. John I. Gelder Department of Chemistry Oklahoma State University Stillwater, OK 74078 john.gelder@okstate.edu http://intro.chem.okstate.edu 12/5/09 1 Thermo I Prep Session

More information

Thermochemistry Chapter 4

Thermochemistry Chapter 4 Thermochemistry Chapter 4 Thermochemistry is the study of energy changes that occur during chemical reactions Focus is on heat and matter transfer between the system and the surroundings Energy The ability

More information

CH 221 Sample Exam Exam II Name: Lab Section:

CH 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 information

Chapter 6. Thermochemistry

Chapter 6. Thermochemistry Chapter 6. Thermochemistry 1 1. Terms to Know: thermodynamics thermochemistry energy kinetic energy potential energy heat heat vs. temperature work work of expanding gases work of expanding gases under

More information

AP* Chapter 6. Thermochemistry

AP* Chapter 6. Thermochemistry AP* Chapter 6 Thermochemistry Section 6.1 The Nature of Energy Energy Capacity to do work or to produce heat. Law of conservation of energy energy can be converted from one form to another but can be neither

More information

(g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (c) Chromium(III) sulfate: ; (h) Dinitrogen tetroxide:

(g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (c) Chromium(III) sulfate: ; (h) Dinitrogen tetroxide: 1. Name each of the following compounds: (a) Ca(OCl) 2 : ; (b) (NH 4 ) 3 PO 4 : ; (c) K 2 Cr 2 O 7 : ; (d) HBrO 2 : ; (e) PF 5 : ; (f) B 2 O 3 : ; (g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (i) Na 2 C 2 O 4

More information

I. The Nature of Energy A. Energy

I. The Nature of Energy A. Energy I. The Nature of Energy A. Energy is the ability to do work or produce heat. It exists in 2 forms: 1. Potential energy is energy due to the composition or position of an object. 2. Kinetic energy is energy

More information

Name SUNY Chemistry Practice Test: Chapter 5

Name SUNY Chemistry Practice Test: Chapter 5 Name SUNY Chemistry Practice Test: Chapter 5 Multiple Choice 1. 1... 3. 3. 4. 4. 5. 6. 7. 8. 9. 10. 11. 1. 13. 14. 15. 16. 17. 18. 19. 0. 1 1) Calculate the kinetic energy in joules of an automobile weighing

More information

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

Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat. CHEM134- F18 Dr. Al- Qaisi Chapter 06: Thermodynamics Thermochemistry is the study of the relationships between chemical reactions and energy changes involving heat. Energy is anything that has the capacity

More information

Chapter 6 Problems: 9, 19, 24, 25, 26, 27, 31-33, 37, 39, 43, 45, 47, 48, 53, 55, 57, 59, 65, 67, 73, 78-82, 85, 89, 93

Chapter 6 Problems: 9, 19, 24, 25, 26, 27, 31-33, 37, 39, 43, 45, 47, 48, 53, 55, 57, 59, 65, 67, 73, 78-82, 85, 89, 93 Chapter 6 Problems: 9, 19, 24, 25, 26, 27, 31-33, 37, 39, 43, 45, 47, 48, 53, 55, 57, 59, 65, 67, 73, 78-82, 85, 89, 93 Chapter 6 Thermochemistry The study of chemical reactions and the energy changes

More information

Lecture Outline. 5.1 The Nature of Energy. Kinetic Energy and Potential Energy. 1 mv

Lecture 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 information

Enthalpy and Internal Energy

Enthalpy and Internal Energy Enthalpy and Internal Energy H or ΔH is used to symbolize enthalpy. The mathematical expression of the First Law of Thermodynamics is: ΔE = q + w, where ΔE is the change in internal energy, q is heat and

More information

Ch. 17 Thermochemistry

Ch. 17 Thermochemistry Ch. 17 Thermochemistry 17.1 The Flow of Energy Energy Transformations Thermochemistry: study of energy changes in chemical reactions and changes in state Chemical potential energy: energy stored in bonds

More information

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

Introduction to Thermochemistry. Thermochemistry Unit. Definition. Terminology. Terminology. Terminology 07/04/2016. Chemistry 30 Thermochemistry Unit Introduction to Thermochemistry Chemistry 30 Definition Thermochemistry is the branch of chemistry concerned with the heat produced and used in chemical reactions. Most of thermochemistry

More information

1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O

1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O Pre-AP Chemistry Spring 2016 Final Review Objective 6.1: Students will recognize indicators of chemical change write balanced chemical equations to describe them based on common reactivity patterns. [S.12.C.1,

More information

Chapter 11 Thermochemistry Heat and Chemical Change

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

More information

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?

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? 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 information

Energy and Chemical Change

Energy and Chemical Change Energy and Chemical Change Section 15.1 Energy In your textbook, read about the nature of energy. In the space at the left, write true if the statement is true; if the statement is false, change the italicized

More information

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

10/23/10. Thermodynamics and Kinetics. Chemical Hand Warmers 10/23/10 CHAPTER 6 Thermochemistry 6-1 Chemical Hand Warmers Most hand warmers work by using the heat released from the slow oxidation of iron 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) The amount your hand temperature

More information

Chapter 5 - Thermochemistry

Chapter 5 - Thermochemistry Chapter 5 - Thermochemistry Study of energy changes that accompany chemical rx s. I) Nature of Energy Energy / Capacity to do work Mechanical Work w = F x d Heat energy - energy used to cause the temperature

More information

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

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

More information

ENERGY AND ENERGETICS PART ONE Keeping Track of Energy During a Chemical Reaction

ENERGY AND ENERGETICS PART ONE Keeping Track of Energy During a Chemical Reaction ENERGY AND ENERGETICS PART ONE Keeping Track of Energy During a Chemical Reaction ADEng. PROGRAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore

More information

THE ENERGY OF THE UNIVERSE IS CONSTANT.

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

More information

Energy and Chemical Change

Energy 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 information

M = Molarity = mol solute L solution. PV = nrt % yield = actual yield x 100 theoretical yield. PM=dRT where d=density, M=molar mass

M = Molarity = mol solute L solution. PV = nrt % yield = actual yield x 100 theoretical yield. PM=dRT where d=density, M=molar mass Solubility Rules: 1. Most nitrate salts are soluble. 2. Most salts of alkali metals and ammonium cations are soluble. 3. Most chloride, bromide and iodide salts are soluble. Exceptions: salts containing

More information

6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.

6. 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

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

6.5 Hess s Law of Heat Summation. 2 Chapter 6: First Law. Slide 6-2 1/3/11 Thermochemistry: Energy Flow and Chemical Change Chapter 6 6.1 Forms of Energy and Their Interconversion 6.2 Enthalpy: Heats of Reaction and Chemical Change Thermochemistry: Energy Flow and Chemical

More information

Thermodynamics- Chapter 19 Schedule and Notes

Thermodynamics- 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 information

C. Perform the following calculations and Round into correct scientific notation.

C. Perform the following calculations and Round into correct scientific notation. Name Hour Honors Chemistry Final Exam Review 2018 - HERBERHOLZ *Due on the day of the exam! No photocopying or copying other classmate s review. Must be handwritten and show work for calculations. Chapter

More information

Energy, Heat and Chemical Change

Energy, 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 information

Chemistry Lab Fairfax High School Invitational January 7, Team Number: High School: Team Members Names:

Chemistry Lab Fairfax High School Invitational January 7, Team Number: High School: Team Members Names: Chemistry Lab Fairfax High School Invitational January 7, 2017 Team Number: High School: Team Members Names: Reference Values: Gas Constant, R = 8.314 J mol -1 K -1 Gas Constant, R = 0.08206 L atm mol

More information

Chem 127, Final Exam December 14, 2001

Chem 127, Final Exam December 14, 2001 I. (55 points) This part of the final corresponds to Exam I. It covers the material in Chapters 1, 2 and 3. A. (8 points) Fill in the empty boxes with the appropriate symbol, number, word or charge. Nuclear

More information

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

Observations of Container. Hot Same Size. Hot Same Size. Hot Same Size. Observations of Container. Cold Expanded. Cold Expanded. Chapter 9: Phenomena Phenomena: Below is data from three different reactions carried out with three different amounts of reactants. All reactants were carried out in expandable/contractable containers

More information

Name. Practice Test 2 Chemistry 111

Name. Practice Test 2 Chemistry 111 Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba

More information

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

Chapter 5 Thermochemistry. 許富銀 ( Hsu Fu-Yin) Chapter 5 Thermochemistry 許富銀 ( Hsu Fu-Yin) 1 Thermodynamics The study of energy and its transformations is known as thermodynamics The relationships between chemical reactions and energy changes that

More information

Name: General Chemistry Chapter 11 Thermochemistry- Heat and Chemical Change

Name: 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 information

Chem 1A Dr. White Fall Handout 4

Chem 1A Dr. White Fall Handout 4 Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular

More information

Chemistry: The Central Science. Chapter 5: Thermochemistry

Chemistry: The Central Science. Chapter 5: Thermochemistry Chemistry: The Central Science Chapter 5: Thermochemistry Study of energy and its transformations is called thermodynamics Portion of thermodynamics that involves the relationships between chemical and

More information

Learning Check. How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C?

Learning Check. How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C? Learning Check q = c * m * ΔT How much heat, q, is required to raise the temperature of 1000 kg of iron and 1000 kg of water from 25 C to 75 C? (c water =4.184 J/ C g, c iron =0.450 J/ C g) q Fe = 0.450

More information

Study Guide Chapter 5

Study Guide Chapter 5 Directions: Answer the following 1. When writing a complete ionic equation, a. what types of substances should be shown as dissociated/ionized? soluble ionic compounds, acids, bases b. What types of substances

More information

Chapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics

Chapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics Chapter 8 Thermochemistry: Chemical Energy Chapter 8 1 Chemical Thermodynamics Chemical Thermodynamics is the study of the energetics of a chemical reaction. Thermodynamics deals with the absorption or

More information

(E) half as fast as methane.

(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 information

Thermochemistry: Part of Thermodynamics

Thermochemistry: Part of Thermodynamics Thermochemistry: Part of Thermodynamics Dr. Vickie M. Williamson @vmwilliamson Student Version 1 Chemical Thermodynamics! Thermodynamics: study of the energy changes associated with physical and chemical

More information

Name Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS

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

More information

AP Chemistry Summer Review Assignment

AP Chemistry Summer Review Assignment Name: Period: Chem I Teacher/year: AP Chemistry Summer Review Assignment Due on the FIRST DAY OF SCHOOL! A. Chemical Foundations 1. The beakers shown below have different precisions. a. Label the amount

More information

Chemical Energetics. First Law of thermodynamics: Energy can be neither created nor destroyed but It can be converted from one form to another.

Chemical Energetics. First Law of thermodynamics: Energy can be neither created nor destroyed but It can be converted from one form to another. Chemical Energetics First Law of thermodynamics: 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 information

s Traditionally, we use the calorie as a unit of energy. The nutritional Calorie, Cal = 1000 cal. Kinetic Energy and Potential Energy

s 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 information

Chapter 6. Thermochemistry

Chapter 6. Thermochemistry Chapter 6 Thermochemistry Section 5.6 The Kinetic Molecular Theory of Gases http://www.scuc.txed.net/webpages/dmackey/files /chap06notes.pdf ..\..\..\..\..\..\Videos\AP Videos\Thermochemistry\AP

More information

Gravity is a force which keeps us stuck to the earth. The Electrostatic force attracts electrons to protons in an atom.

Gravity 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 information

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

Law of conservation of energy: energy cannot be created or destroyed, only transferred One object to another One type of energy to another ch6blank Page 1 Chapter 6: Thermochemistry Thermochemistry: study of the relationships between chemistry and energy Energy: capacity to do work Work:result of a force acting over a certain distance, one

More information

1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E

1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Hour Exam I Page 1 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E 2. Consider the measurements 9.74

More information

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

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

More information

Exam 4, Enthalpy and Gases

Exam 4, Enthalpy and Gases CHEM 1100 Dr. Stone November 8, 2017 Name_ G Exam 4, Enthalpy and Gases Equations and constants you may need: ΔE system = q + w PV = nrt R = 0.0821 (L*atm)/(mole*K) w = -PΔV K.E. = 1 2 m *µ 2 rms µ rms=

More information

1. When two pure substances are mixed to form a solution, then always

1. When two pure substances are mixed to form a solution, then always Name: Date: 1. When two pure substances are mixed to form a solution, then always A) there is an increase in entropy. B) there is a decrease in entropy. C) entropy is conserved. D) heat is released. E)

More information

MgO. progress of reaction

MgO. 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

Unit 4: Reactions and Stoichiometry

Unit 4: Reactions and Stoichiometry Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)

More information

Thermochemistry. Energy and Chemical Change

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

More information

CHAPTER 16 REVIEW. Reaction Energy. SHORT ANSWER Answer the following questions in the space provided.

CHAPTER 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 information

IB Topics 5 & 15 Multiple Choice Practice

IB 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

Saturday Study Session 1 3 rd Class Student Handout Thermochemistry

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 information

Chapter 6. Thermochemistry. Chapter 6. Chapter 6 Thermochemistry. Chapter 6 Thermochemistry Matter vs Energy 2/16/2016

Chapter 6. Thermochemistry. Chapter 6. Chapter 6 Thermochemistry. Chapter 6 Thermochemistry Matter vs Energy 2/16/2016 Chapter 6 Thermochemistry Chapter 6 Chapter 6 Thermochemistry 6.1 Chemical Hand Warmers 6.2 The Nature of Energy: Key Definitions 6.3 The First Law of Thermodynamics: There is no Free Lunch 6.4 6.5 Measuring

More information

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.

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. 1 2004 B 2 Fe(s) + 3 2 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

More information

Ch. 6 Enthalpy Changes

Ch. 6 Enthalpy Changes Ch. 6 Enthalpy Changes Energy: The capacity to do work. In Physics, there are 2 main types of energy Kinetic (energy of motion) = ½ mv 2 Potential (energy of position due to gravity)= mgh In Chemistry,

More information

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

Thermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation Thermochemistry Energy 1st Law of Thermodynamics Enthalpy / Calorimetry Hess' Law Enthalpy of Formation The Nature of Energy Kinetic Energy and Potential Energy Kinetic energy is the energy of motion:

More information

Accelerated 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 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 information

17.2 Thermochemical Equations

17.2 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 information