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Lime for garden...
bobharvey wrote:
On 18 Mar, 18:35, (Nick Maclaren) wrote: God alone knows what sodium oxide is like, but I don't want to get anywhere near even a small quantity! You do right. http://msds.chem.ox.ac.uk/SO/sodium_oxide.html "Reacts violently with water, acids and with many other compounds. Store under dry inert gas. May lead to fire in contact with combustible material." Strangely inaccurate for the last sentence (but then there is a disclaimer page http://msds.chem.ox.ac.uk/ - which also seems odd for Oxford Uni). I doubt Sodium oxide would lead to fire in contact with combustible material. But Sodium Peroxide, well, that's another matter entirely - http://msds.chem.ox.ac.uk/SO/sodium_peroxide.html -- Jeff (cut "thetape" to reply) |
#2
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Lime for garden...
In article , "Jeff Layman" writes: | | I doubt Sodium oxide would lead to fire in contact with combustible | material. But Sodium Peroxide, well, that's another matter entirely - | http://msds.chem.ox.ac.uk/SO/sodium_peroxide.html No, that's not what they mean. If it is in contact with anything combustible, I believe that the water vapour in the air is enough to cause a fire. Regards, Nick Maclaren. |
#3
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Lime for garden...
Jeff Layman says...
bobharvey wrote: On 18 Mar, 18:35, (Nick Maclaren) wrote: God alone knows what sodium oxide is like, but I don't want to get anywhere near even a small quantity! You do right. http://msds.chem.ox.ac.uk/SO/sodium_oxide.html "Reacts violently with water, acids and with many other compounds. Store under dry inert gas. May lead to fire in contact with combustible material." Strangely inaccurate for the last sentence (but then there is a disclaimer page http://msds.chem.ox.ac.uk/ - which also seems odd for Oxford Uni). I doubt Sodium oxide would lead to fire in contact with combustible material. But Sodium Peroxide, well, that's another matter entirely - http://msds.chem.ox.ac.uk/SO/sodium_peroxide.html I don't know about Sodium oxide, but I've had "fun" with sodium and potassium metals in contact with combustible organic chemicals. They have a tendency towards spontaneous combustion even in the absence of oxygen. I had one experiment years ago that did just that and it was impossible to put the resulting fire out. My employer wasn't too impressed either because it was a total flame free environment and I'd got a beaker with six feet high flames roaring out. T'was fun though. -- David in Normandy. To e-mail you must include the password FROG on the subject line, or it will be automatically deleted. |
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