Timeline for Why is the Gibbs free energy for phase changes zero at constant temperature and pressure?
Current License: CC BY-SA 3.0
9 events
| when toggle format | what | by | license | comment | |
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| Nov 14, 2017 at 4:55 | history | edited | Jan | CC BY-SA 3.0 |
Better title, extraneous space
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| Nov 13, 2017 at 15:41 | answer | added | Allan | timeline score: 3 | |
| Nov 24, 2015 at 14:18 | vote | accept | Tonylb1 | ||
| Nov 23, 2015 at 23:52 | answer | added | Chet Miller | timeline score: 15 | |
| Nov 23, 2015 at 21:31 | comment | added | Tonylb1 | I think the system here is the liquid/solid mixture. What I am not understanding in the phase change ok we have $\Delta H$ but this heat is going where at equilibrium? to the mixture or to the surrounding? Even when we dont have equilibrium $\Delta G = \Delta H - T \Delta S$ Here T$\Delta S$ represents $\Delta H$ at equilibrium right? | |
| Nov 23, 2015 at 17:34 | history | tweeted | twitter.com/StackChemistry/status/668845160135020545 | ||
| Nov 23, 2015 at 15:18 | answer | added | DavePhD | timeline score: 6 | |
| Nov 23, 2015 at 12:47 | comment | added | Chet Miller | In the inequalities you wrote for chemical reaction, the $\Delta G$ represents a change in free energy from an initial thermodynamic equilibrium state of a system to its final thermodynamic equilibrium state. Please precisely define the "system" they refer to and the initial and final equilibrium states (so that we can be sure you understand exactly what they are saying). Also, are you aware that these relations are just a rule of thumb for beginners? After we address these reaction issues, we can look at phase change. | |
| Nov 22, 2015 at 23:05 | history | asked | Tonylb1 | CC BY-SA 3.0 |