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For more information, please see full course syllabus of Chemistry
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Lecture Comments (6)

0 answers

Post by Afusat Ekiyoyo on March 6, 2014

calculate THE reaction

0 answers

Post by Marian Iskandar on September 4, 2013

If you were getting tripped up by the math in the last example, I have the corrections in the following:

For the K @298k is 1x10^+58, not negative, but his explanation is still correct (it's still reactant favored, and highly endothermic).

For K @ 2000k, (delta)H = 3(-110.5)-(-824) = -331.5 + 824 = +492.5 kJ
(delta)S is the correct value.

When you plug in all values in the (delta)G equation, the correct answer is:
-5.95x10^5 J/mole, which makes it VERY exothermic, and thus PRODUCT favored.

His explanations were sound, but he just needed to double check his math, and his negative and positive values. He's still a phenomenal professor.

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Post by Nancy Humphries on August 12, 2013

just download "Greenshot"  screen capture software, (shareware), take a screen picture and print it, its free:)

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Post by Marian Iskandar on May 2, 2013

My answer to the example calculation for K slightly different:
Did anyone get the same?

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Post by Maimouna Louche on July 28, 2012

When I need it I copy for later use, you can do the same.

0 answers

Post by Anders Løvschal on September 21, 2011

How come there is no "print buttom" so you can print the things the professor types?

Gibbs' Function, Equilibrium

  • Useful Gibbs function: DG = DH – T DS

  • And DG = -RTlnK

  • Use thermo functions to calculate DG and K for several systems

  • Can assume DH and DS don’t change with T

  • Calculate DG at non-standard T and see how K will change with T

Gibbs' Function, Equilibrium

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • The Gibbs' Function 0:35
    • Values of Delta G
  • The Gibbs' Function and K 9:11
    • Gibbs' Function Change (Free Energy)
    • Values of Gibbs' Function Standard Change
  • Calculation of K from ThermoDynamic Data 15:46
    • Example: Nitrogen Dioxide to Dinitrogen Tetroxide
  • Calculation of K 24:32
    • Example: Diamond to Graphite
  • Calculation of K 31:33
    • Example: Ammonia
  • Temperature Changes: Gibbs' Function and K 38:12
    • Estimating Gibbs' Function Values at Temperatures
  • Temperature Changes 42:29
    • Example: Oxide of Iron and Carbon
  • Additional Example 1