Timeline for How is the acidic dissociation of acetic acid thermodynamically feasible?
Current License: CC BY-SA 3.0
20 events
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| Apr 17, 2017 at 1:16 | history | edited | Melanie Shebel | CC BY-SA 3.0 |
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| Apr 16, 2017 at 21:29 | answer | added | Tyberius♦ | timeline score: 5 | |
| Apr 16, 2017 at 19:52 | comment | added | airhuff | @Tyberius , I think your comment is pretty close to being a good answer...FWIW. | |
| Apr 16, 2017 at 18:13 | comment | added | Tyberius♦ | All chemical reactions are a balancing act between enthalpy and entropy. Strictly from an enthalpy standpoint, going to one side of the reaction completely should be favored. However, entropy is maximized by evenly mixing components. Combining these two factors, the equilibrium position is found by maximizing the free energy which has an enthalpic and entropic component. Due to this entropic contribution, all reactions are technically equilibria; they just might be shifted so far to one side that the reaction appears to have gone to completion. | |
| Apr 16, 2017 at 15:34 | comment | added | TAR86 | I was thinking of the collection of molecules. In terms of pure energy ($U$), they should not dissociate. But there are so many of them - so some do, because it is not likely that they all stay associated. This is quantified by entropy, an expression of probability, which results in free enthalpy ($G$). | |
| Apr 16, 2017 at 14:28 | review | Close votes | |||
| Apr 17, 2017 at 0:12 | |||||
| Apr 16, 2017 at 13:24 | comment | added | Azulene | @TAR86 So do you mean to say that every molecule has different amounts of entropy? | |
| S Apr 16, 2017 at 12:47 | history | suggested | Berry Holmes | CC BY-SA 3.0 |
Fixed equilibrium arrows, minor formatting edits
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| Apr 16, 2017 at 12:36 | comment | added | TAR86 | @Azulene You now enter the world of entropy. Suppose you have $10^{23}$ molecules of acid. Will they all behave and not dissociate? That's unlikely. So you end up with a dynamic equilibrium with some molecules recombining, other dissociating etc. | |
| Apr 16, 2017 at 12:34 | review | Suggested edits | |||
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| Apr 16, 2017 at 12:31 | history | edited | Azulene | CC BY-SA 3.0 |
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| Apr 16, 2017 at 12:27 | comment | added | Azulene | Then why do those few molecules dissociate anyway? Theoretically (considering the thermodynamics of the reaction) they shouldn't right? | |
| S Apr 16, 2017 at 8:19 | history | edited | porphyrin | CC BY-SA 3.0 |
English altered
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| S Apr 16, 2017 at 8:19 | history | suggested | Another.Chemist | CC BY-SA 3.0 |
The aesthetics of this question was improved (Equilibrium reaction)
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| Apr 16, 2017 at 7:56 | review | Suggested edits | |||
| S Apr 16, 2017 at 8:19 | |||||
| S Apr 16, 2017 at 7:40 | history | suggested | Another.Chemist | CC BY-SA 3.0 |
The aesthetics of this question was improved
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| Apr 16, 2017 at 5:11 | comment | added | airhuff | Note that the reaction should be written as an equilibrium, and, importantly, that the equilibrium lies well to the left (i.e. most of the acetic acid is not dissociated). | |
| Apr 16, 2017 at 5:07 | review | Suggested edits | |||
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| Apr 16, 2017 at 5:01 | review | First posts | |||
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| Apr 16, 2017 at 4:58 | history | asked | Azulene | CC BY-SA 3.0 |