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CHEM 433 - 10/13/11

CHEM 433 - 10/13/11. III. 2 nd Law of THERMO • Intro & Overview ( 3.1 - 3.2 ) - 2nd Law Statements - Using it:  S SYS vs.  S SURR (this is the hard way…) READ: CHAPTER 3 HW #5 Due Monday Web is up-to-date, including review sheet (will post HW#4 key late tomorrow or M).

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CHEM 433 - 10/13/11

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  1. CHEM 433 - 10/13/11 III. 2nd Law of THERMO • Intro & Overview (3.1 - 3.2) - 2nd Law Statements - Using it: SSYS vs. SSURR (this is the hard way…) READ: CHAPTER 3 HW #5 Due Monday Web is up-to-date, including review sheet (will post HW#4 key late tomorrow or M)

  2. 1ST LAW: What can happen? (permissible changes)• ΔU = q + w or dU = dq + dw• The work needed to change an adiabatic system is the same, regardless of how the work is performed (wad = ΔU).• Energy is conserved. It is neither created nor destroyed.• “You can’t get something for nothing!”

  3. 2ND LAW: What does happen? (spontaneous changes)• No process is possible in which the sole result is absorption of heat from a reservoir and its complete conversion to work. (Kelvin, Planck)• Heat can not be conveyed from a lower temperature reservoir to a higher temperature reservoir, without the performance of work. (Clausius)• The ENTROPY of an isolated system increases in the course of spontaneous change (Stot > 0).• You can convert all your work into heat – but you can’t convert all your heat into work.—> “You can’t even break even!”

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