Thermite
A thermite reaction (sometimes called a "Goldschmidt reaction") refers to a very
exothermic process occurring between a metal Oxide and a more active pure metal.
The more reactive metal reduces the metal Oxide, Oxidizing itself and releasing a
substantial amount of energy during the reaction.
Generally, thermite is made by mixing Iron Oxide and Aluminum powder and igniting it
at very high temperatures (a few thousand degrees). The reaction releases so much
energy, molten Iron metal is produced as one of the products.
The two most common types of thermite are made using either Iron(III) Oxide, Fe2O3
(also known as Hematite), or using Iron(II, III) Oxide, Fe3O4 (also known as Magnetite).
The Iron Oxide is mixed with finely powdered Aluminum metal. When the thermite
reacts, liquid Iron metal and Aluminum Oxide, Al2O3, is produced as a result.
Other, more exotic forms of thermite can also be produced.
Using other metal Oxides, one can produce other, sometimes
more powerful, blends of thermite. For instance, substituting
Copper(II) Oxide for Iron Oxide in a thermite mixture can
produce a very brightly burning reaction which yields Copper
metal as a result. Although Copper Oxide thermite is probably
the most common of the exotic thermites, one could also use
other metal Oxides such as Tin Oxide, Lead Oxide, or any
other metal Oxide which could be reacted with a reducing
metal (such as Aluminum or Magnesium). They key is that the
reducing metal must be sufficiently higher on the activity series
than the metal Oxide in order to support the single replacement
reaction.
Thermite has found some use as a crude method of welding
metals due to the intense heat and molten metals produced by the reaction.
Thermite reactions can also be used on occasion to produce pure metals from their
oxide counterparts as long as the reaction taking place is thermodynamically favorable
(decrease in Gibbs Free Energy).
Thermite is not easy to ignite. Thermite has a very high activation energy required to
start the reaction. The two most common ways to ignite thermite are:
•
Magnesium Ribbon (Mg)
• Magnesium metal burns in an Oxygen
environment (air) in a very bright,
exothermic reaction. Magnesium
ribbon can burn at several thousand
degrees easily igniting thermite. The
Magnesium ribbon is useful as it acts
like a fuse, calmly burning, allowing a
short delay between when the ribbon is
lit and when the thermite begins to
react.
•
•
Other forms of Magnesium metal can
be substituted for Magnesium ribbon
such as metal turnings, powders, or
even common sparkers which contain
Magnesium.
Potassium Permanganate (KMnO4) + Glycerin
• An alternative to using Magnesium
ribbon is to use the heat given off by
the reaction between Potassium
Permanganate and glycerin. Potassium
Permanganate is an extremely
powerful Oxidizer which spontaneously
ignites after coming in contact with
glycerin.
•
After adding a few drops of glycerin to
Potassium Permanganate powder and
a short delay, a violent exothermic
oxidation reaction occurs which will
ignite a thermite mixture.
It is important to mix the thermite ingredients thoroughly in order to create a
homogeneous mixture. Unless the thermite is sufficiently mixed, it may be difficult to
ignite or sustain the thermite reaction.
Thermite Types (by metal Oxide):
Iron(III) Oxide - Fe2O3
Iron(II, III) Oxide - Fe3O4
Copper(II) Oxide - CuO
Copper(I) Oxide - Cu2O
Tin(IV) Oxide - SnO2
Titanium(IV) Oxide - TiO2
Manganese(IV) Oxide - MnO2
Manganese(III) Oxide - Mn2O3
Chromium(III) Oxide - Cr2O3
Cobalt(II) Oxide - CoO
Silicon Dioxide - SiO2
Nickel(II) Oxide - NiO
Vanadium(V) Oxide - V2O5
Silver(I) Oxide - Ag2O
Molybdenum(VI) Oxide - MoO3
Click Here To See
>>> ** Videos / Pictures of Thermite Demonstrations ** <<<
Iron(III) Oxide [Fe2O3]
Iron(III) Oxide is a reddish-brown powder (left), commonly known as "rust" is mixed with
Aluminum Powder (center) to make thermite (right).
The balanced chemical reaction between Iron(III) Oxide and Aluminum is show below,
Above: Lumps of Iron metal produced by an Iron(III) Oxide thermite
reaction.
According to the reaction's stoichiometry, the ratio of Fe2O3 to Aluminum powder by
weight is about 3 to 1 (2.96 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -768.75 kJ assuming
that both the Iron metal and Aluminum Oxide are in the liquid state after the reaction, as
they solidify, they release additional energy, bringing the total change in enthalpy to, ∆H
= -851.50 kJ per 213.65 grams of thermite (-3.985 kJ/g).
Iron(II, III) Oxide [Fe3O4]
Iron(II, III) Oxide is a black powder (above), sometimes known as "Magnetite" due to its
magnetic properties.
According to the reaction's stoichiometry, the ratio of Fe3O4 to Aluminum powder by
weight is about 3.2 to 1 (3.22 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -3002.79 kJ assuming
that both the Iron metal and Aluminum Oxide are in the liquid state after the reaction, as
they solidify, they release additional energy, bringing the total change in enthalpy to, ∆H
= -3347.60 kJ per 910.46 grams of thermite (-3.677 kJ/g).
Copper(II) Oxide [CuO]
Copper(II) Oxide, or "Cupric Oxide", is a black powder shown above (left) as is CuO
Thermite (right).
According to the reaction's stoichiometry, the ratio of CuO to Aluminum powder by
weight is about 4.4 to 1 (4.42 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -1108.89 kJ assuming
that both the Copper metal and Aluminum Oxide are in the liquid state after the reaction,
as they solidify, they release additional energy, bringing the total change in enthalpy to,
∆H = -1203.8 kJ per 262.60 grams of thermite (-4.584 kJ/g).
Copper(I) Oxide [Cu2O]
Copper(I) Oxide, or "Cuprous Oxide", is a reddish colored powder which, when mixed
with Aluminum powder, forms the thermite shown above.
Above: Front and back of a Copper metal lump produced by a Cu2O
Thermite reaction.
According to the reaction's stoichiometry, the ratio of Cu2O to Aluminum powder by
weight is about 8.0 to 1 (7.96 to 1 to be more exact).
The change in entropy of this reaction is calculated to be, ∆H = -1035.21 kJ assuming
that both the Copper metal and Aluminum Oxide are in the liquid state after the reaction,
as they solidify, they release additional energy, bringing the total change in enthalpy to,
∆H = -1169.8 kJ per 483.23 grams of thermite (-2.421 kJ/g).
Tin(IV) Oxide [SnO2]
Tin(IV) Oxide, or "Stannic Oxide", is a white powder is above (left) as is Tin(IV) Oxide
thermite (right).
Above: Tin metal which was extracted from the remains of a Tin(IV)
Oxide thermite reaction and recast into shiny round lumps..
According to the reaction's stoichiometry, the ratio of SnO2 to Aluminum powder by
weight is about 4.2 to 1 (4.19 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -1477.95 kJ assuming
that both the Tin metal and Aluminum Oxide are in the liquid state after the reaction, as
they solidify, they release additional energy, bringing the total change in enthalpy to, ∆H
= -1609.30 kJ per 560.05 grams of thermite (-2.873 kJ/g).
Titanium(IV) Oxide [TiO2]
Titanium(IV) Oxide, or "titania", is a white powder (above).
Above: Lumps of Titanium metal produced from a KClO3 boosted TiO2
thermite reaction.
SEM Images
According to the reaction's stoichiometry, the ratio of TiO2 to Aluminum powder by
weight is about 2.2 to 1 (2.22 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -366.69 kJ assuming
that both the Titanium metal and Aluminum Oxide are in the liquid state after the
reaction, as they solidify, they release additional energy, bringing the total change in
enthalpy to, ∆H = -519.40 kJ per 347.52 grams of thermite (-1.495 kJ/g).
In practice, however, the reaction does not appear to proceed as described above. The
Aluminum metal does not seem to reduce the Titanium(IV) Oxide all the way down to
Titanium metal but rather stops at a less-oxidized state of Titanium. A black Titanium
Oxide, which is likely to be Titanium(III, IV) Oxide, is left after the reaction ceases. Upon
analysis, one can further reduce the black Titanium Oxide further using Magnesium as a
reducing agent. Doing so one can obtain a golden-yellow colored substance which is
presumably Titanium(II) Oxide.
Titanium(II) Oxide, TiO, is said to be golden-yellow colored,
Titanium(III) Oxide, Ti2O3, is said to be violet colored, and
Titanium(III, IV) Oxide, Ti3O5, is said to be black colored.
It has been shown that one can use Potassium Chlorate (KClO3) to boost TiO2 thermite
reactions. With the addition of Potassium Chlorate, extra Aluminum powder, and a
fluxing agent (Fluorspar, CaF2) to the thermite mixture, elemental Titanium can be
produced.
Mixing the ingredients TiO2, Al, KClO3, and CaF2 using the ratio of 100 : 72 : 61 : 47
respectively by weight*, one can achieve a fast-burning thermite reaction which
produces Titanium metal.
(* Ideal ratio still in development)
Manganese(IV) Oxide [MnO2]
Manganese(IV) Oxide is a black powder (above).
Above: Nuggets of Manganese metal produced by a MnO2 thermite
reaction
According to the reaction's stoichiometry, the ratio of MnO2 to Aluminum powder by
weight is about 2.4 to 1 (2.42 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -1639.71 kJ assuming
that both the Manganese metal and Aluminum Oxide are in the liquid state after the
reaction, as they solidify, they release additional energy, bringing the total change in
enthalpy to, ∆H = -1788.7 kJ per 368.74 grams of thermite (-4.851 kJ/g).
Manganese(III) Oxide [Mn2O3]
Manganese(III) Oxide is a dark brownish-black powder (left); Mn2O3 thermite (right).
According to the reaction's stoichiometry, the ratio of Mn2O3 to Aluminum powder by
weight is about 2.9 to 1 (2.93 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -648.7 kJ assuming
that both the Manganese metal and Aluminum Oxide are in the liquid state after the
reaction, as they solidify, they release additional energy, bringing the total change in
enthalpy to, ∆H = -716.7 kJ per 211.83 grams of thermite (-3.38 kJ/g).
Chromium(III) Oxide [Cr2O3]
Chromium(III) Oxide is a green powder shown above (left), as is Chromium(III) Oxide
thermite (right).
Above: Shiny Chromium metal exposed inside remnants of Cr2O3
thermite reaction
According to the reaction's stoichiometry, the ratio of Cr2O3 to Aluminum powder by
weight is about 2.8 to 1 (2.82 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -501.87 kJ assuming
that both the Chromium metal and Aluminum Oxide are in the liquid state after the
reaction, as they solidify, they release additional energy, bringing the total change in
enthalpy to, ∆H = -536.0 kJ per 205.95 grams of thermite (-2.603 kJ/g).
Cobalt(II) Oxide [CoO]
Cobalt(II) Oxide is a black powder shown above (left). Cobalt(II) Oxide thermite (right).
Above: Small pieces of Cobalt metal produced from a CoO thermite
reaction
According to the reaction's stoichiometry, the ratio of CoO to Aluminum powder by
weight is about 4.2 to 1 (4.17 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -858.69 kJ assuming
that both the Cobalt metal and Aluminum Oxide are in the liquid state after the reaction,
as they solidify, they release additional energy, bringing the total change in enthalpy to,
∆H = -962.0 kJ per 278.75 grams of thermite (-3.451 kJ/g).
Silicon Dioxide [SiO2]
Silicon Dioxide, in the form of common sand, shown above (left), Sulfur (center), and
SiO2 thermite (right)..
Above: Large lump of elemental Silicon produced by a SiO2 thermite
reaction
According to the reaction's stoichiometry, the ratio of SiO2 to Aluminum powder by
weight is about 1.7 to 1 (1.67 to 1 to be more exact). However, using a simple
stoichiometric ratio of only Silicon Dioxide and Aluminum powder will make the mixture
extremely difficult to ignite. In order ignite the thermite more easily one can add extra
Aluminum powder and Sulfur to the thermite mixture. Aluminum powder and Sulfur will
react together in an extremely exothermic reaction and will burn at a high enough
temperature so as to ignite and maintain the SiO2 and Aluminum powder reaction.
A mixture of Silicon Dioxide, Aluminum powder, and Sulfur in the ratio of 9 : 10 : 12 by
weight respectively, works well and is (relatively) easy to ignite.
Silicon Dioxide and Aluminum powder react to form Aluminum Oxide and elemental
Silicon. Another reaction, between Sulfur and Aluminum powder, aids the SiO2 thermite
reaction and produces Aluminum Sulfide as a result.
Aluminum Sulfide will react with water, or moisture in the air, to give off the foul smelling
and toxic Hydrogen Sulfide (H2S) gas, so avoid getting the products of the reaction wet.
Alternatively, one can boost a SiO2 thermite reaction with the addition of Potassium
Chlorate, and a fluxing agent (Fluorspar, CaF2) to the mixture and eliminate the need to
use Sulfur as in the method described above.
Mixing SiO2, Al, KClO3, and CaF2 using the ratio of 100 : 96 : 81 : 55, one can create a
fast-burning, and easy-to-ignite, SiO2 thermite reaction which has been shown to
produce elemental Silicon as a product. The elimination of Sulfur from the thermite
relieves one of the undesirable production of Aluminum Sulfide which, when wet,
releases harmful and foul-smelling, H2S gas.
Nickel(II) Oxide [NiO]
Nickel(II) Oxide is a green powder shown above (left). Nickel(II) Oxide thermite (right).
Above: Lump of Nickel metal produced during a NiO thermite reaction
According to the reaction's stoichiometry, the ratio of NiO to Aluminum powder by
weight is about 4.2 to 1 (4.15 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -883.3 kJ assuming
that both the Nickel metal and Aluminum Oxide are in the liquid state after the reaction,
as they solidify, they release additional energy, bringing the total change in enthalpy to,
∆H = -955.4 kJ per 278.03 grams of thermite (-3.44 kJ/g).
Vanadium(V) Oxide [V2O5]
Vanadium(V) Oxide, also known as Vanadium Pentoxide, is a yellowish-orange powder
shown above (left). Vanadium(V) Oxide thermite (right).
Above: Chunk of Vanadium metal from thermite reaction; colorful
oxidization layer visible on surface
According to the reaction's stoichiometry, the ratio of V2O5 to Aluminum powder by
weight is about 2.0 to 1 (2.02 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -3429.6 kJ assuming
that both the Vanadium metal and Aluminum Oxide are in the liquid state after the
reaction, as they solidify, they release additional energy, bringing the total change in
enthalpy to, ∆H = -3726.7 kJ per 815.44 grams of thermite (-4.57 kJ/g).
Silver(I) Oxide [Ag2O]
Silver(I) Oxide is a black powder shown above (left). Partially reacted Silver(I) Oxide
thermite (right).
Above: A small nugget of Silver metal produced via a Silver(I) Oxide
thermite reaction. Silver has been polished with a rotary grinder to
reveal the shiny metal underneath the slag from the thermite reaction.
According to the reaction's stoichiometry, the ratio of Ag2O to Aluminum powder by
weight is about 12.9 to 1 (12.88 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -1459.75 kJ assuming
that both the Silver metal and Aluminum Oxide are in the liquid state after the reaction,
as they solidify, they release additional energy, bringing the total change in enthalpy to,
∆H = -1582.55 kJ per 749.18 grams of thermite (-2.11 kJ/g).
Molybdenum(VI) Oxide [MoO3]
According to the reaction's stoichiometry, the ratio of MoO3 to Aluminum powder by
weight is about 2.67 to 1 (2.667 to 1 to be more exact).
The change in enthalpy of this reaction is calculated to be, ∆H = -875.4 kJ assuming
that both the Molybdenum metal and Aluminum Oxide are in the liquid state after the
reaction, as they solidify, they release additional energy, bringing the total change in
enthalpy to, ∆H = -930.53 kJ per 197.9 grams of thermite (-4.70 kJ/g).
Last updated:
Magnesium Ribbon
Magnesium ribbon will react in the presence of Oxygen to
form Magnesium Oxide. Burning Magnesium produces a
very bright reaction which liberates a substantial amount of
heat energy, easily reaching temperatures of a few
thousand degrees.
Due to its extremely high reaction temperature, Magnesium
ribbon is commonly used as one of the preferred methods
of igniting thermite and other reactions which have very
high activation energies.
Magnesium ribbon can be ignited with relative ease using a simple butane lighter or
Bunsen burner. Once ignited, the Magnesium ribbon will burn slowly but steadily down
the length of the strand, leaving a flaky, white, Magnesium Oxide residue behind.
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Potassium Permanganate (KMnO4)
Potassium Permanganate (shown left) is a dark powder which, when dissolved in water,
disassociates into K+1 and MnO4-1 ions to form a deep
purple solution.
The Permanganate ion (MnO4-1) acts as an extremely
powerful oxidizing agent in many chemical reactions.
Potassium Permanganate is such a powerful oxidizer, in
fact, that when mixed with certain substances, a
combustion reaction will proceed spontaneously without the
need for a form of ignition.
When glycerin is poured onto a pile Potassium Permanganate powder, the Potassium
Permanganate quickly begins to react, automatically starting a combustion reaction
within seconds as shown in the video below.
Due to the intense heat liberated in the process, as well as the ease of starting the
reaction, Potassium Permanganate / Glycerin is sometimes used to ignite thermite
mixtures.
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Iron(III) Oxide
Description
Video
Pictures
100 grams of Fe2O3
Thermite reacting in a
sand-filled coffee can.
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100 grams of Fe2O3
Thermite.
Unexpectedly slow
start due to poor
weather conditions.
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100 grams of extra fine
Fe2O3 thermite,
producing white hot,
liquid, Iron metal.
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500 grams of Fe2O3
thermite reacted in a
heavy cast Iron skillet.
A failed attempt to melt
through the skillet, the
skillet conducted the
heat into the wooden
planks supporting it,
catching them on fire.
Liquid Iron fused itself
onto the skillet.
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50 grams of Fe2O3
thermite react near a
can of spray paint
(don't try this at home) to
the sound of
Tchaikovsky's 1812
Overture.
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*Generously provided by
"Cody"
2000 grams of
Fe2O3 thermite, filling
a large coffee can,
reacts on top of a ¼
inch thick, steel, IBeam. The resulting
reaction is so
intensely hot that it
melts its container
and the steel beam,
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spilling vast amounts
of molten Iron and
Al2O3 everywhere.
200 grams of
Fe2O3thermite made
with fine-grain (3.2
micron) aluminum
powder reacts more
quickly due to the
smaller particle size.
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*Aluminum powder
generously provided by
"Charles"
Iron(II, III) Oxide
Description
100 grams of Fe3O4
thermite reacts very
violently as a ball of
fire and liquid Iron
metal flies out of the
coffee can reaction
vessel.
Three small Fe3O4
thermite reactions in
metal pots which
easily melt though
the bottom, dripping
molten Iron on the
ground.
*Generously provided by
"CSGLEON"
300 grams of Fe3O4
thermite react very
energetically,
however, fails to melt
through the heavy
duty cast Iron skillet.
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75 grams of Fe3O4
thermite easily melt
through a piece of
steel and molten Iron
falls into the sand
below.
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200 grams of Fe3O4
thermite reacting
inside galvanized
steel pipe on cast
Iron skillet. Due to
the heat of the
reaction, the Zinc
coating on pipe is
vaporized and
converted into fluffy
white puffs of Zinc
Oxide . The reaction
leaves the white-hot
pipe thoroughly
welded to the skillet
and covered with
ZnO.
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300 grams of Fe3O4
thermite made with
fine-grain (3.2
micron) aluminum
powder reacts more
quickly due to the
smaller particle size.
*Aluminum powder
generously provided by
"Charles"
4000 grams of Fe3O4
thermite, filling a
large, 10-inch
diameter flower pot,
reacts on top of an
old hard drive. The
molten metal
produced by the
reaction melts
through the hard
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drive casing and
platters and totally
destroys the internal
electronics. Sadly,
no video was
captured of this
extremely impressive
reaction.
Video:
6000 grams of
Fe3O4 thermite
reacts at the 2010
Bay Area Maker Faire.
The molten metal
produced by the
reaction streams out
the bottom and over
the sides of the large
flower pot and into a
pan of sand below.
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Pictures:
Shows the set up
and products of a
collection of several
thermite reactions (3
- 6 kg) performed at
the Maker Faire.
5000 grams of
Fe3O4 thermite
reacts at the 2010
Bay Area Maker Faire.
The molten metal
produced by the
reaction streams out
the bottom and over
the sides of the large
flower pot and into a
pan of sand below.
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8200 grams of
Fe3O4 thermite (+ 10
w% cryolite flux)
reacts at the 2011
Bay Area Maker Faire.
The molten metal
pours from bottom
and sides of the
severely cracked
flower pot and
sprays into the air
above.
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Copper(II) Oxide
Description
100 gram, blindingly
bright, CuO Thermite
reaction glowing white
hot and partially
melting the coffee
can.
Using extra fine
Copper Oxide powder,
the 100 gram thermite
reaction proceeds
very violently and
explosively, vaporizing
much of the remains,
starting grass fires,
and pushing
observers back with a
shockwave.
100 grams of CuO
thermite made using
very fine CuO powder.
Once ignited, the
thermite mixture
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reacts extremely
quickly and
energetically,
expelling the vast
majority of the
products into the air.
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Copper(I) Oxide
Description
100 grams of Cu2O
Thermite ignite by
pouring Glycerin over a
small amount of
Potassium
Permanganate. After
the thermite reaction, a
small blob of elemental
Copper metal was
found.
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Tin(IV) Oxide
Description
A 100 gram, SnO2,
thermite reaction,
producing a gray blob
of metal containing a
region of Tin metal
which remained soft
and molten for some
time as the reaction
cooled.
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100 grams of SnO2
thermite reacts
producing liquid Tin
metal.
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Titanium(IV) Oxide
Description
This 100 gram
thermite reaction
proceeds very slowly,
steadily consuming
the thermite mixture.
The reaction failed to
reduce the white TiO2
to Titanium metal, but
instead reduced the
TiO2 to a black
compound which is
likely to be Ti3O5.
100 grams of KClO3boosted TiO2 thermite
react after being
ignited with
Magnesium Ribbon.
Thermite reaction
successfully yields
several grams of
Titanium metal as a
product.
530 grams of KClO3boosted TiO2 thermite
using a TiO2 : Al :
KClO3 : CaF2 ratio of
100 : 75 : 50 : 40.
Reaction produces
several large blobs of
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Titanium metal.
SEM Images
EDAX Analysis – Element
Composition
2000 grams of KClO3boosted TiO2 thermite
using a TiO2 : Al :
KClO3 : CaF2 ratio of
100 : 72 : 61 : 47.
Reaction produces
several large blobs of
Titanium metal.
[SEM Images
EDAX Analysis – Element
Composition]
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Manganese(IV) Oxide
Description
A quick, 100 gram
MnO2 thermite
reaction, leaving a
small, brownish-black
metal chunk behind
which contained very
small, trace, pieces of
what appeared to be
Manganese metal.
200 grams of MnO2
thermite + 10 grams of
Cryolite flux. Several
Manganese metal
nuggets produced.
Chromium(III) Oxide
Video
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Description
A 100 gram of Cr2O3
thermite reaction. The
reaction proceeds
very slowly, not unlike
Titanium(IV) Oxide
thermite. Afterward,
small chunks of shiny
Chromium metal are
found in the cooled
remains.
Video
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Cobalt(II) Oxide
Description
25 grams of CoO
thermite react while
tiny, red-hot, metal
fragments are thrown
from the container.
Video
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Yellow Iron Oxide
Description
100 grams of Yellow
Iron Oxide thermite
reaction reacts
surprisingly
vigorously, leaving a
very hot blob of
glowing metal.
Video
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400 grams of Yellow
Iron Oxide thermite
reacts inside nested
flower pots. Liquid
metal is clearly visible
pouring through hole
in the bottom of the
pot into the sand
below.
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Silicon Dioxide
Description
300 gram mixture of
Silicon Dioxide,
Aluminum powder,
and Sulfur burns
slowly with a bright
blue flame; a large
lump of elemental
Silicon is produced
during reaction.
Reaction continues
even after camera
stops filming. Out of
site of the camera, the
thermite reaction
melts through the side
of the steel reaction
vessel.
SEM Images
1000 gram mixture of
Silicon Dioxide,
Aluminum powder,
and Sulfur burns
slowly for about 2
minutes 30 seconds.
Video
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Nickel(II) Oxide
Description
50 grams of green
Nickel Oxide thermite.
The NiO thermite
begins to react after a
short delay after the
Potassium Chlorate
and sugar ignition
mixture is lit.
Video
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Vanadium(V) Oxide
Description
50 grams of
Vanadium Pentoxide
thermite. Reaction
proceeds extremely
quickly after being
ignited by Potassium
Chlorate and sugar.
200 grams of V2O5
thermite + 20 grams of
Cryolite flux (total
mixture 220 grams).
The reaction proceeds
quickly after ignition
by Potassium
Chlorate, sugar, and
Magnesium Ribbon.
Video
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Silver(I) Oxide
Description
Video
Pictures
Two attempts to ignite
a 21 gram Ag2O
thermite mixture using
a Magnesium ribbon
fuse. Thermite begins
to react but quickly
stops, appearing to
'blow itself out' after
area around Mg
ribbon ignites. Small
round globules of
Silver metal found
around areas where
reaction occurred.
EDAX Analysis – Element
Composition
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Molybdenum(VI) Oxide
Description
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17 grams of MoO3
thermite description
reacts quickly in a bright
flash.
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Alloy Thermite
Description
200 grams of thermite
made using a mixture
of Fe2O3, Cu2O, and
Cr2O3 thermites in a
ratio of 7 : 8 : 5 by
weight. As a result of
the reaction, a copper-
Video
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colored metal alloy
was formed containing
Iron, Copper, and
Chromium metals in a
theoretical ratio of 3 :
5 : 2 by weight. A
small amount of
Cryolite flux was
utilized.
200 grams of
Manganese(III) Oxide
thermite (placed on
bottom of container)
with about 125 grams
of Iron(II, III) Oxide
thermite on top. The
Fe3O4 thermite was
ignited which, in turn,
ignited the Mn2O3
thermite. Excellent
slag-metal separation
leaving a large blob of
ferromanganese alloy
metal. No flux used.
220 grams of thermite
made with a ratio of 5
: 3 : 2 between
stoichiometric
mixtures of NiO,
Fe3O4, and Mn2O3
thermites respectively.
Additionally, 30 grams
of Cryolite flux was
added bringing the
total mass of the
mixture to 250 grams.
The reaction
proceeded somewhat
slowly once ignited
using Potassium
Chlorate, sugar, and
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Magnesium Ribbon,
but burned quite hot
and left a large chunk
of alloyed metal
behind.
Original pictures and videos available upon request.