Final exam guuide

Final exam guuide - Final Exam Study Guide: Can You Do All...

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1 Final Exam Study Guide: Can You Do All These Things? CHE 132 Spring 2010, Stony Brook University MSJ = the Moore, Stanitski, Jurs textbook section PSE = problem solving example and practice (PSP) in the textbook chapter CE = conceptual exercise in the textbook chapter E = exercise in the textbook chapter QRT = end of the chapter Questions for Review and Thought FofC = the activity book Foundations of Chemistry SRPC = the activity book Solving Real Problems with Chemistry MSJ Chapter 6, Lectures 1 - 5 1) Explain what is meant by a system, surroundings, temperature, and heat in thermodynamics. (CE 6.3, MSJ 6.2) 2) Explain the meaning of E = q + w and relate the change in internal energy to heat and work. (PSE 6.2, PSE 6.3, QRT 6.25, MSJ 6.2) 3) Define and write units for heat capacity, specific heat capacity, and molar heat capacity, use heat capacities to relate heat, mass, and temperature change, and explain why some objects warm up or cool off faster than others. (PSE 6.4, PSE 6.5, QRT 6.29, QRT 6.33, QRT 6.34, QRT 6.37, MSJ 6.3) 4) Explain what is meant by PV work and how it relates to the change in energy and the change in enthalpy. (PSE 6.6, MSJ 6.4) 5) Define the following terms exothermic, endothermic, enthalpy change ( H), enthalpy of fusion, and enthalpy of vaporization. (MSJ 6.4) 6) Calculate the total enthalpy change upon heating or cooling with phase changes. (QRT 6.46, MSJ 6.4) 7) Use a thermo-chemical reaction equation to calculate the energy transferred as the result of a chemical reaction. (QRT 6.62, QRT 6.63, QRT 6.67, MSJ 6.6) 8) Use calorimetric data to determine changes in internal energy and enthalpy. (QRT 6.81, QRT 6.83, MSJ 6.8) 9) Explain Hess’s Law, and use it to calculate enthalpy changes for one reaction from other reactions. (QRT 6.90, QRT 6.94, QRT 6.97, MSJ 6.9, MSJ 6.10) MSJ Chapter 18, Lectures 6 - 8 10) Write Boltzmann’s famous equation defining entropy, and explain what it means. (Lecture 6, MSJ 18.3) 11) Recognize qualitatively whether the entropy of a substance is high or low and if the entropy increases or decreases in some physical process or chemical reaction. (PSE 18.2, CE 18.4, QRT 18.21, QRT 18.22, QRT 18.27, QRT 18.31, MSJ 18.3) 12) Calculate the change in entropy for a reversible constant temperature process given the energy flow into or out of the system or surroundings. (PSE 18.1, QRT 18.35, QRT 18.45, MSJ 18.3, MSJ 18.5) 13) Use standard molar entropy values to determine the entropy of a substance and changes in entropy. (PSE 18.3, PSE 18.4, QRT 18.55, MSJ 18.3, MSJ 18.4). 14) Use standard Gibbs free energies of formation to calculate changes in the standard Gibbs Free Energy. (PSE 18.5, MSJ 18.6) 15) Identify whether a reaction is spontaneous or not from S universe and G system (QRT 18.57, QRT 18.63, QRT 18.65, MSJ 18.2, MSJ 18.6).
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2 16) Use H, S, and T to determine whether a reaction will be spontaneous or not, and determine the temperature at which a reaction occurs or reverses. ( PSE 18.6, QRT 18.73, MSJ 18.6).
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This note was uploaded on 11/14/2010 for the course CHE 131 taught by Professor Kerber during the Spring '08 term at SUNY Stony Brook.

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Final exam guuide - Final Exam Study Guide: Can You Do All...

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