Morg_NZ
Contributor
Is it true that this reg CANNOT be used with nitrox??
Need to settle argument:monster:
Need to settle argument:monster:
AtomicTi2 Titanium Question
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I think that they recommend that you do not use gas with more than 40% O2 and titanium can become brittle with exposure to high concentration of Oxygen. I would say that you CAN use nitrox with your titanim reg, but it is not recommended!
Morg_NZ:
Untrue to a point.
Titanium will spontaneously combust (burn) when exposed to elevated levels of O2 at elevated pressure. IN a lab setting they can get titanium to burn well within recreational nitrox parameters (35% O2 and a catylist and just the right conditions, IIRC) but in practice this doesn't seem to be a problem.
What *has* happened, however is that a titanium regulator has burst into flame when exposed to O2 from a deco bottle. I only know of one such case of this happening. It seems to me that it's ok with use up to 32%. Between 32% and 40% I have my doubts becasue they can make it happen in a lab and above 40% it's probably not very smart.
Hope that helps.
R..
Morg_NZ:
From Atomic website...
"Nitrox ready: Factory ready for Nitrox to 40%."
http://www.atomicaquatics.com/
Settled...
WarmWaterDiver
Contributor
Titanium is more brittle than many other metals whether exposed to oxygen / enriched oxygen or not - this is just a measure of malleability. Interestingly, it's typically the high reactivity of titanium that underlies its corrosion resistance - it rapidly forms a reaction product film on the surface that protects the base metal (somewhat) - but as others have mentioned here that very reactivity is a double-edged sword. Reactive metal fires are one of the most difficult to extinguish once started. Think of junior high or high school science class and experiments involving burning a small thin strip of magnesium to get a frame of reference.
Why doesn't anyone produce a Sodium or Potassium regulator. Now that would be interesting...
WarmWaterDiver
Contributor
It woudn't be DIR . . . .
Actually, since Sodium and Potassium both spontaneously combust when put in water...your air source would not last long, but you would not need a light and be real warm for the short dive...
As a chemistry major at university, I remember throwing chunks of sodium into the school fountain to watch them flash, burn and hiss while scooting crazily on top of the water. Quite a sight to see. Someone in my department claimed to have blown up a toilet by flushing down a Sodium down...those crazy kids...
As a chemistry major at university, I remember throwing chunks of sodium into the school fountain to watch them flash, burn and hiss while scooting crazily on top of the water. Quite a sight to see. Someone in my department claimed to have blown up a toilet by flushing down a Sodium down...those crazy kids...
MookieMoose
Guest
jagfish:
Sodium and potassium react to hydrolyse water. The metal itself doesn't burn, but reacts (read: is consumed in the process) with water to split it into hydrogen gas and oxygen gas, producing enough heat in the process to burn the hydrogen gas. If you had thrown a chunk of sodium into the fountain that was large enough to sink, it would have caused an underwater explosion. having that happen behind you head a couple of minutes into the dive would spice things up a little...
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