Author Topic: ionizing oxygen  (Read 11909 times)

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ionizing oxygen
« on: October 12, 2008, 12:14:32 pm »
now the air ionizer was placed on the incoming air to ionize oxygen making it highly unstable and attacking hydrogen instead of trying to recombine when entered together in the combustion chamber......but i always wondered what type of LED's were used in the air ionizer......what wave length?

stumbled upon this from this site.

"I will deal with your questions one at a time.

1) Oxygen ionizes in the presence of an energy discharge such as a
UltraViolet lamp. Do the ionized oxygen atoms remain ionized as long
as they are in the presence of the energy field?

Once the oxygen atoms are ionized, they enter into a series of very rapid
reactions, including recombinations with electrons to become neutral
species again. They do not "remain ionized" much at all. But there is a
continuing pool of ionized oxygen atoms because new ones are being formed
all the time.

A side issue: you cannot form oxygen ions with a UV lamp. The quartz
windows of the lamp will only transmit light of wavelength 160 nm or more;
oxygen will only ionize efficiently in UV light of wavelength 130 nm or
less. The oxygen reaction that you can drive with a UV lamp involves
neutral atomic oxygen, which can be generated by photodissociation with
light of 210 nm or less. The easier and more usual way to generate oxygen
ions is in an electrical discharge.
---------

2) How soon after being ionized do the oxygen atoms reform into Ozone?

Much less than one second. But the reaction that forms ozone does not
involve oxygen ions; ozone is formed by

O + O2 + inert third molecule ---> O3 + third molecule

Atomic oxygen (O) is readily formed from oxygen ions; molecular oxygen (O2)
is abundantly present in air anyway.
---------

3) If an ionized oxygen atom has a -2 charge, how can these atoms
bond into Ozone when they should be magnetically repulsed by one
another?

Ionized oxygen, as formed in an electrical discharge or by very low
wavelength UV light has a +1 charge. The most readily formed ion is
molecular oxygen missing one electron: O2+ . Atomic oxygen missing one
electron, O+ , also enters into the reaction system, but it is a much
higher energy species. Because of the electrostatic repulsion (not
magnetic) between ions with like charge, the chemical reactions in the
system do not involve two ions reacting together; it is always one ion with
a neutral species.
----------

4) Is there some way to speed up the decomposition of Ozone?

There are many ways to speed up the decomposition of ozone. Ozone (O3) is a
high energy form of oxygen, so it is quite ready to revert to the lower
energy, more stable form of molecular oxygen (O2). There are many ways of
achieving the transformation. Atomic chlorine or bromine -- from molecular
chlorine or bromine and visible light -- are particularly effective as gas
phase catalysts, as is nitric oxide. Nearly all organic substances are
directly oxidized by ozone. Rubber perishes very rapidly into a powdery
heap, for example. Reducing solutions -- ferrous sulfate or potassium
iodide -- will effectively remove ozone from a gas bubbled through them.
"

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Re: ionizing oxygen
« Reply #1 on: October 12, 2008, 17:10:13 pm »
pulsed high voltage field can be used for ionizing air , you dont even need the leds.

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Re: ionizing oxygen
« Reply #2 on: October 12, 2008, 22:21:31 pm »
stan used pulsed high voltage and led's.

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Re: ionizing oxygen
« Reply #3 on: October 18, 2008, 00:48:04 am »

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Re: ionizing oxygen
« Reply #4 on: October 18, 2008, 00:53:29 am »
so what i've come to conclude is that it takes 193nm to dissasociate O2 into O and O and it takes 225nm to ionize Oxygen.

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Re: ionizing oxygen
« Reply #5 on: February 27, 2009, 01:08:00 am »
Stevie can this be moved under my projects section.....thank you !