Timeline for Is every chemical reaction in equilibrium?
Current License: CC BY-SA 3.0
7 events
| when toggle format | what | by | license | comment | |
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| Mar 3, 2016 at 19:16 | comment | added | Lighthart | @MaxW if the amount of BaSO4 was under the incredibly small solubility limit, adding more of it would shift the equilibrium. The effect would be so small that you could pragmatically say there is no change in the equilibrium, but that is not quite true. It is however, a useful imprecision. | |
| Mar 3, 2016 at 12:15 | comment | added | Curt F. | (1) Equilibrium can be applied to open systems in some cases. (2) insoluble precipitates and gases can and do participate in equilibrium reactions, whether or not they are "reabsorbed". An example is rising bicarbonate levels in the ocean due to higher CO2 levels in the atmosphere. There is an equilibrium. (3) It is unclear what definition of "pragmatic" you are using. | |
| Mar 3, 2016 at 2:20 | comment | added | MaxW | Look at it this way - adding solid BaSO4 to the solution won't shift the "equilibrium" to the left . So how could there be an equilibrium?!? | |
| Mar 2, 2016 at 19:18 | comment | added | Lighthart | I cannot rationally interpret the idea of a chemical equilibrium not existing. I can rationally interpret is it pragmatically zero. | |
| Mar 2, 2016 at 17:29 | comment | added | MaxW | If there were an "equilibrium" for the reaction then the equation would be something like: $$\ce{K_{eq}} = \dfrac{\ce{[BaSO4][HCl]^2}}{ \ce{[BaCl2][H2SO4]}}$$ and such an equilibrium just doesn't exist. | |
| Mar 2, 2016 at 17:06 | history | edited | Lighthart | CC BY-SA 3.0 |
added 30 characters in body
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| Mar 2, 2016 at 16:59 | history | answered | Lighthart | CC BY-SA 3.0 |