Chapter_6IM

Chapter_6IM - Chapter 6 Thermochemistry This chapter...

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Chapter 6 Thermochemistry This chapter develops the concepts of thermochemistry. Upon completion of Chapter 6, your students should be able to: 1. Define and explain the following terms: Energy Radiant energy Thermal energy Chemical energy Potential energy Thermochemistry Open system Closed system Isolated system Endothermic Exothermic Enthalpy ( H) Calorimetry Heat capacity Specific heat 2. Classify common processes as endothermic or exothermic. 3. Use thermochemical equations and stoichiometry to determine amount of heat lost or gained in a chemical reaction. 4. Perform calculations involving specific heat, mass and temperature change. 5. Sketch the main components of a constant-volume bomb calorimeter. 6. Determine heats of reactions given experimental data collected in a calorimetry experiment. 7. Calculate standard enthalpy of reactions given the standard enthalpy of formations for products and reactants. 8. Apply Hess’s law to a multi-step process to determine standard enthalpy of reaction. 9. Describe heat of solution, lattice energy, heat of hydration, heat of dilution, system, surrounding, and internal energy. 10. Classify properties of materials as state functions or non-state functions. 11. Restate the First Law of Thermodynamics. 12. Name the sign conventions for work and heat used in the textbook. 13. Apply heat and work relationships to gas-phase problems. 14. Define H in term of E, P, and V. 15. Calculate change in internal energy ( E) given thermochemical equations.
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Section 6.1 The Nature of Energy and Types of Energy Energy, the ability to do work, takes many forms, including kinetic, potential, radiant, thermal, and chemical energy. Students sometimes confuse energy and temperature. If we place a pot of water on the kitchen stove and turn the dial to high, we observe that the water’s temperature increases (using a thermometer) as the water warms up. This process continues until we reach the boiling point of the water. Once this temperature is reached, the water no longer increases in temperature, but we are still adding energy to the system because the dial on the stove still reads “high”. What this shows is that the temperature of the water and the energy pumped into it are proportional until the boiling point is reached. At that point, the energy is used to change the physical state of the liquid water to steam without changing the temperature of either. Using the concept of conservation of energy, we know that the energy provided by the stove at the boiling point of water must be used to break the forces of attraction that hold the water molecules together in the liquid phase. Section 6.2
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This note was uploaded on 02/08/2012 for the course CHEM 161 taught by Professor Shaklovich during the Spring '10 term at Harvard.

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Chapter_6IM - Chapter 6 Thermochemistry This chapter...

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