Timeline for How to explain disagreement between Le Châtelier's principle and the simplified Gibbs free energy equation?
Current License: CC BY-SA 4.0
5 events
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| Jun 4, 2019 at 21:24 | comment | added | Buck Thorn♦ | Finally, van't Hoff's equation will not predict the expected Le Chatelier's behavior if you use the wrong $\Delta H$. In particular, you should not use the value for the limiting (infinitely dilute solution) heat of solvation. Rather you should use the value associated with transferring a solute molecule into a saturated solution. | |
| Jun 4, 2019 at 21:21 | comment | added | Buck Thorn♦ | I think I misunderstood the original question, and Andrew nailed the answer because he saw where the confusion lay (it has nothing to do with van't Hoff's equation or the particular value of $\Delta H$). | |
| Jun 4, 2019 at 21:19 | comment | added | Buck Thorn♦ | You provide a lot of useful data to compare, which I'll have to look at more closely. I think as far as the posted question is concerned, the answer is that it's sort of a self-fulfilling prophecy: the van't Hoff expression can't fail, because it's a way to define $\Delta H$ for a process from the temperature dependence of K. Of course $\Delta H$ has an independent meaning, and values can be provided by calorimetry, but the point is that van't Hoff's expression is always right, provided you use the right value of $\Delta H$. | |
| Jun 4, 2019 at 2:21 | history | edited | Michael Lautman | CC BY-SA 4.0 |
Major edit,
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| Jun 3, 2019 at 18:34 | history | answered | Michael Lautman | CC BY-SA 4.0 |