1 / 16

Hour Exam II

Prepare for the upcoming Thermodynamics and Kinetics exam scheduled on March 15, 7:00-9:00 PM at 103 Mumford Hall. This guide covers essential thermodynamic concepts such as the spontaneity of reactions, Gibbs free energy (ΔG), enthalpy (ΔH), and entropy (ΔS). Additionally, it addresses reaction kinetics, including rate laws, mechanisms, and factors affecting reaction rates. Review the equations and principles vital for understanding spontaneity and reaction rates to excel in your exam.

oni
Télécharger la présentation

Hour Exam II

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. Hour Exam II Wednesday, March 15 7:00 – 9:00 pm 103 Mumford Hall AQG, AQI Allen AQJ Blair AQF 150 Animal Science Fisher AQB, AQC Koys AGD Pearson AQA conflict exam 4:30 – 6:30 162 Noyes

  2. Kinetics Thermodynamics : spontaneity of reaction G < 0spontaneous 2H2(g) +O2(g) 2H2O(l) Go = -474 kJ Go = Ho- TSo a) low T b) high T Ho < 0 favorable So < 0 unfavorable Thermodynamically spontaneous very slow

  3. thermodynamics thermodynamics Kinetics rates of reaction mechanism of reaction O2(g)  2 H2O(l) Greaction < 0 2 H2(g) + Greactants Gproducts kinetics

  4. qn qe r + + Kinetics 2H2(g) + O2(g)2 H2O(l) Go = -474 kJ spontaneous P.E.n-e - +

  5. Low Temperature

  6. High Temperature

  7. + + High Temperature exothermic endothermic

  8. Kinetics rate of reaction [reactant] decrease increase [product] 1. Temperature (K.E.) 2. Concentration 3. Orientation

  9. - 1 2 differential rate laws A + B C - d[A] = d[C] dt d[B] = dt a) + b) - + rate = dt A + B 2 C - d[A] = dt d[C] dt -d[B] = dt rate =  A + B C +

  10. 100 [ ] 50 0 1 2 3 4 5 time (min) [ ] = t -[ ] = t x t (min) 0 100 100 0 x 72 1 72 28 x 2 52 52 48 x x 3 37 37 63 x 4 27 27 73 5 19 19 81 81 - 0 = 16.2 min-1 ave. rate = 5 - 0 (19 ) - 100 ave. rate = - = 16.2 min-1 5 - 0

  11. x 100 t (min) 0 100 100 0 x [ ] 72 1 72 28 x 50 2 52 52 48 x x 3 37 37 63 x 4 27 27 73 0 5 19 19 81 1 2 3 4 5 time (min) overall ave. rate = - (19 - 100) = 16.2 min-1 5 - 0 1st minute ave. rate = = 28.0 min-1 - (72 ) - 100 1 - 0 5th minute ave. rate = - 27) = 8.0 min-1 - (19 5 - 4

  12. x 100 x [ ] x 50 x x x 0 1 2 3 4 5 time (min) instantaneous rate slope of line tangent to curve = at t = 0 initial rate fastest rate

  13. t instantaneous (min) rate k = rate [reactant] 100 33.0 0 0.33 1 72 23.8 2 52 17.2 3 37 12.2 4 27 8.9 5 19 6.3 0.33 0.33 0.33 0.33 0.33 rate [reactant] = k [reactant] k = rate constant

  14. k = rate [reactant] k independent of [reactants] dependent on Temperature k [A]a [B]b [C]c ... (-d[A]) k rate = = dt k, a, b and c determined experimentally isolation method

  15. [A] [A] Concentration (M) Concentration (M) t (ms) t (ms) Exp. 1 [B]i initial rate [A]i (M) (M) (M s-1) 1.0 1.0 1.0 x 10-3 Exp. 2 [A]i [B]I initial rate (M)(M)(M s-1) 2.0 1.0 2.0 x 10-3 Exp. 3 [A]i [B]I initial rate (M)(M)(M s-1) 1.0 x 10-3 1.0 2.0

  16. Exp. 1 k rate = [A]a [B]b [A]i [B]I initial rate (M)(M)(M s-1) 1.0 1.0 a = 0 a = 1 a = 2 2 x 10-3 = 1 x 10-3 [2.0]a [1.0]a rate 2 = rate 1 1.0 x 10-3 Exp. 2 1 x 10-3 = 1 x 10-3 rate 3 = rate 1 [2.0]b [1.0]b b = 0 b = 1 b = 2 [A]i [B]I initial rate (M)(M)(M s-1) 2.0 1.0 rate = k [A] 2.0 x 10-3 1storder reaction Exp. 3 [A]i [B]I initial rate (M)(M)(M s-1) 1.0 2.0 1x10-3(M s-1) = k [1.0 M] k = 1 x 10-3 s-1 1.0 x 10-3

More Related