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| Thread ID: 111753 | 2010-08-10 07:13:00 | Chemistry Help! | xyz823 (13649) | PC World Chat |
| Post ID | Timestamp | Content | User | ||
| 1126346 | 2010-08-10 22:34:00 | Double arrows are used for an equilibrium equation. I used an equals sign as the easier alternative to finding out how to type in an arrow. I also don't think it would be an equilibrium reaction since it would essentially go to completion. The Na and Cl would not precipitate out for the same reason that they don't in the sea. NaCl is rather soluble and would stay in solution. |
user (1404) | ||
| 1126347 | 2010-08-10 23:53:00 | Double arrows are used for an equilibrium equation. I used an equals sign as the easier alternative to finding out how to type in an arrow. I also don't think it would be an equilibrium reaction since it would essentially go to completion. The Na and Cl would not precipitate out for the same reason that they don't in the sea. NaCl is rather soluble and would stay in solution. I see. I think I was thinking of organic chemistry reactions which are more likely to establish equilibrium. I guess the green colour is from the chlorine irons. |
kahawai chaser (3545) | ||
| 1126348 | 2010-08-11 00:51:00 | I guess the green colour is from the chlorine irons. You are thinking of chlorine gas (Cl2) rather than chloride ions here. Chloride ions = colourless. A glass of salt solution is colourless. :) |
Renmoo (66) | ||
| 1126349 | 2010-08-11 00:52:00 | Double arrows are used for an equilibrium equation. I used an equals sign as the easier alternative to finding out how to type in an arrow. I also don't think it would be an equilibrium reaction since it would essentially go to completion. I don't mean to be too pedantic here, but technically all chemical reactions are equilibrium reactions. The favoured direction depends on the condition and entropy. |
Renmoo (66) | ||
| 1126350 | 2010-08-11 00:52:00 | God im glad i dont go to school, i feel like a dummy | Gobe1 (6290) | ||
| 1126351 | 2010-08-11 00:57:00 | I don't mean to be too pedantic here, but technically all chemical reactions are equilibrium reactions. The favoured direction depends on the condition and entropy. Technically yes. For practical considerations, not all. Consider the reaction of hydrogen and oxygen to form water. Once water is formed, the activation energy for the reverse reaction at room temp makes it essentially non-reversible. Also the formation of polymers is not an equilibrium reaction. The green colour is owing to the hydrated ferrous ion in the solution. |
user (1404) | ||
| 1126352 | 2010-08-11 01:01:00 | Because Cl and Na are present what prevents (or could induce) them from precipitating/forming a salt solution? Since user has answered the first half of the question, I will attempt to explain the second half. Common ion effect - The addition of either positive ions or negative ions can induce precipitation. The presence of NaCl salt in solution has the following equilibrium: NaCl (s) < = > Na+(l) + Cl-(l) Where s = solid, l = liquid. When more of the positive ions or negative ions are added to the solution, it can push the equilibrium towards the left side (Le Chatelier's principle), whereby the ions are induced to form the solid form again. Cheers :) |
Renmoo (66) | ||
| 1126353 | 2010-08-11 01:04:00 | The green colour is owing to the hydrated ferrous ion in the solution. Does the complex contain two or three H2O molecules? It's been a while... |
Renmoo (66) | ||
| 1126354 | 2010-08-11 01:13:00 | H2O + HSO3 (-1) = SO4 (-2) + 3H (+1) + 2e Fe (+3) + e = Fe (+2) H20 + HSO3 + 2Fe (+3) = SO4 (-2) + 2Fe(+2) + 3H(+1) Talked to the chem teacher, had the electrons on the wrong side man. Left hand side overall is -1. Right hand side is +1 (-2 + 3) so add 2 electrons to the right hand side to balance each side. And apparently if you have electrons on the same side in each equation you've done something wrong. |
xyz823 (13649) | ||
| 1126355 | 2010-08-11 01:33:00 | H2O + HSO3 (-1) -2e = SO4 (-2) + 3H(+1) Fe (+3) + e = Fe(+2) Note the negative sign posted by user. |
Renmoo (66) | ||
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