1 / 23

Chapter 19 Chemical Thermodynamics

Chemistry: The Central Science , 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten. Chapter 19 Chemical Thermodynamics. Todd Austell, The University of North Carolina  2006, Pearson Prentice Hall. Yes. Nonspontaneous processes can never occur.

axelle
Download Presentation

Chapter 19 Chemical Thermodynamics

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemistry: The Central Science, 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 19 Chemical Thermodynamics Todd Austell, The University of North Carolina  2006, Pearson Prentice Hall

  2. Yes. Nonspontaneous processes can never occur. • No. Nonspontaneous processes can occur with some external assistance.

  3. Yes. Nonspontaneous processes can never occur. • No. Nonspontaneous processes can occur with some external assistance.

  4. Yes • No

  5. Yes • No

  6. The value of S actually does not change with q, just the magnitude of Sinitial and Sfinal. • S depends not merely on q but on qrev. There is only one reversible isothermal path between two states regardless of the number of possible paths. • S’s dependence on q is negligible. • q depends on H which is a state function.

  7. The value of S actually does not change with q, just the magnitude of Sinitial and Sfinal. • S depends not merely on q but on qrev. There is only one reversible isothermal path between two states regardless of the number of possible paths. • S’s dependence on q is negligible. • q depends on H which is a state function.

  8. The enthalpy of the system must increase by a greater amount than the entropy of the system decreases. • The entropy of the universe for the process must increase by the same amount as the entropy of the system decreases. • The entropy of the universe for the process must increase by a greater amount than the entropy of the system decreases. • The entropy of the universe for the process must decrease by a greater amount than the entropy of the system decreases.

  9. The enthalpy of the system must increase by a greater amount than the entropy of the system decreases. • The entropy of the universe for the process must increase by the same amount as the entropy of the system decreases. • The entropy of the universe for the process must increase by a greater amount than the entropy of the system decreases. • The entropy of the universe for the process must decrease by a greater amount than the entropy of the system decreases.

  10. Molecules and single atoms can experience all the same types of motion. • A molecule can vibrate (atoms moving relative to one another) and rotate (tumble); a single atom can do neither • A molecule can vibrate (atoms moving relative to one another) and rotate (tumble); a single atom can only rotate. • A molecule can translationally move and rotate (tumble); a single atom can do neither.

  11. Molecules and single atoms can experience all the same types of motion. • A molecule can vibrate (atoms moving relative to one another) and rotate (tumble); a single atom can do neither • A molecule can vibrate (atoms moving relative to one another) and rotate (tumble); a single atom can only rotate. • A molecule can translationally move and rotate (tumble); a single atom can do neither.

  12. S = 0 • S < H • S = W • S > H

  13. S = 0 • S < H • S = W • S > H

  14. It is a substance at the triple point. • It is pure liquid at 0°K (absolute zero). • It is an elemental standard state. • It must be a perfect crystal at 0°K (absolute zero).

  15. It is a substance at the triple point. • It is pure liquid at 0°K (absolute zero). • It is an elemental standard state. • It must be a perfect crystal at 0°K (absolute zero).

  16. always increase • always decrease • sometimes increase and sometimes decrease, depending on the process

  17. always increase • always decrease • sometimes increase and sometimes decrease, depending on the process

  18. Entropy of universe increases and free energy of the system decreases. • Entropy of system decreases and free energy of the universe increases. • Entropy of system increases and free energy of the universe decreases. • Entropy of universe decreases and free energy of the system increases.

  19. Entropy of universe increases and free energy of the system decreases. • Entropy of system decreases and free energy of the universe increases. • Entropy of system increases and free energy of the universe decreases. • Entropy of universe decreases and free energy of the system increases.

  20. It indicates the process is spontaneous under standard conditions. • It indicates the process has taken place under standard conditions. • It indicates the process has taken place at 273K and 1 barr. • It indicates the process has taken place at 1 atm and 0K.

  21. It indicates the process is spontaneous under standard conditions. • It indicates the process has taken place under standard conditions. • It indicates the process has taken place at 273K and 1 barr. • It indicates the process has taken place at 1 atm and 0K.

  22. H = TS • H < TS • H > TS • We cannot determine without additional information.

  23. H = TS • H < TS • H > TS • We cannot determine without additional information.

More Related