Timeline for Balancing a reaction with unknown products
Current License: CC BY-SA 3.0
22 events
| when toggle format | what | by | license | comment | |
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| S Feb 16, 2018 at 13:21 | history | edited | pentavalentcarbon | CC BY-SA 3.0 |
title fixed+can this question be not tagged with anything except inorganic chem?
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| S Feb 16, 2018 at 13:21 | history | suggested | Gaurang Tandon | CC BY-SA 3.0 |
title fixed+can this question be not tagged with anything except inorganic chem?
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| Feb 16, 2018 at 12:25 | review | Suggested edits | |||
| S Feb 16, 2018 at 13:21 | |||||
| Jan 3, 2017 at 5:45 | vote | accept | Imagine Dragons | ||
| Jul 27, 2016 at 2:30 | vote | accept | Imagine Dragons | ||
| Aug 29, 2016 at 4:45 | |||||
| Jul 27, 2016 at 2:30 | answer | added | Imagine Dragons | timeline score: -2 | |
| Jul 8, 2016 at 18:28 | answer | added | Robert Budd Haemer | timeline score: -2 | |
| Oct 31, 2015 at 13:59 | comment | added | Mithoron | related chemistry.stackexchange.com/questions/27393/… | |
| Oct 31, 2015 at 13:23 | comment | added | Technetium | It is correct both ways (to write the intermediate or not) but more conventionally written with the hydroxide byproduct as under normal conditions the oxide fully converts to the hydroxide so it is the end product. | |
| Oct 31, 2015 at 13:15 | comment | added | Technetium | Sodium ion taking the oxygen atom or water molecule leaving oxygen atom , same thing ( sorry if it was confusing) . | |
| Oct 31, 2015 at 13:14 | comment | added | Imagine Dragons | Oh okay @Joel that makes a lot of sense. I have this question for a science lab, however we weren't taught this so should I keep the answer with OH? Thank you so much!!! | |
| Oct 31, 2015 at 13:05 | comment | added | Technetium | No, think if the sodium or potassium (as you just mentioned) takes the oxygen from a water molecule (H2O) , hydrogen is left. Sorry I can't do the required format for any equations on my phone. Due to the fact that these oxides are so unstable , the product is just written as sodium hydroxide , using the thinking that there's no need to mention the intermediate sodium oxide . | |
| Oct 31, 2015 at 12:40 | comment | added | Imagine Dragons | @Joel I think it's the same case with Potassium + Water but I don't know why | |
| Oct 31, 2015 at 12:38 | comment | added | Imagine Dragons | I don't really get it though :/... I thought single displacement would take the form of A + BC -> AB + C with no exceptions. Na+H2O... So Na bonds with oxygen right? And they form Na2O and O2 is left? @Joel | |
| Oct 31, 2015 at 12:36 | comment | added | Technetium | If you did the reaction practically you can definetly observe the sodium reacting with the water, the pH of the water will turn alkaline as the sodium hydroxide is formed. | |
| Oct 31, 2015 at 12:29 | comment | added | Technetium | The H comes from the water, think about what happened to the water molecule that reacted with the sodium ion and left an oxygen atom , hence the speculation of sodium oxide formation, where did the hydrogens go?. Sorry identify when what does what? | |
| Oct 31, 2015 at 12:25 | comment | added | Imagine Dragons | @Joel But how can I identify when it does that? and where did H come from? | |
| Oct 31, 2015 at 12:16 | comment | added | Technetium | The hydrogen is created from the exothermic reaction between the highly reactive sodium metal and water. | |
| Oct 31, 2015 at 12:15 | comment | added | M.A.R. | Please visit this page, this page and this one on how to format your posts better. Alternatively, visit this chatroom for further formatting guidance. | |
| Oct 31, 2015 at 12:15 | history | edited | M.A.R. | CC BY-SA 3.0 |
added 56 characters in body; edited tags
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| Oct 31, 2015 at 12:14 | comment | added | Technetium | The Na2O is unstable so it would very quickly convert to the more stable NaOH. | |
| Oct 31, 2015 at 11:58 | history | asked | Imagine Dragons | CC BY-SA 3.0 |