Beauty of chemistry This web page describes a few simple
experiments, brought in a special way. The experiments
are the following:
Nitric acid cannot be obtained anymore
in the EU, but it can fairly easily be distilled from
sodium nitrate or potassium nitrate and sulfuric acid in
an all glass distillation apparatus. Another option is
to mix sodium bisulfate monohydrate (common pH-minus for
swimming pools) and sodium nitrate and distill off
nitric acid from this mix. Only a small quantity is
needed. I distilled a little yellow fuming nitric acid
(appr. 30 ml) and diluted this for the experiment to
appr. 60% by weight.
Required chemicals:
Required equipment:
Safety:
Disposal:
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Bubbling of copper metal
in concentrated (not fuming) nitric acid This is a simple
experiment. A piece of copper is added to concentrated
nitric acid and the reaction is watched. It is a very
well-known experiment, which also is demonstrated in
many high schools, but this classic remains very
interesting and when viewed at 40x slow motion, a whole
new world opens up on how the reaction starts and how
the bubbles move through the liquid. Pour a few ml of concentrated
nitric acid (appr. 60% by weight) in a test tube.
Home-made nitric acid (distilled from sodium nitrate),
usually is more concentrated. This must be diluted with
some water for a smooth and fast reaction. Heat the nitric acid somewhat.
It should not be boiling hot, a temperature of 60 °C or
so is fine. No need to be precise with this, a good
guideline is having the test tube just a little too hot
to touch it for longer than a second. Make the copper wire into a
small ball and then let it fall into the acid. As soon as the copper falls
into the acid, a violent reaction sets in. A video at
real speed can be downloaded here.
The video at 40x slow
motion is much more impressive. Below follow three
images of the formation of the bubbles, immediately
after adding the copper to the acid.
Reaction between iodine
pentoxide and hydrazine The reagents of this experiment are
less common, but the experiment itself is simple again.
A piece of solid iodine pentoxide is dropped into a
concentrated solution of hydrazine dihydrochloride. This
results in an extremely violent and exothermic reaction
in which nitrogen and iodine are formed. So much heat is
produced, that a large part of the iodine escapes as a
plume of purple gas. Prepare a few ml of a nearly
saturated solution of hydrazine dihydrochloride. The
liquid cools down a little bit when the solid is
dissolved. There is no need to heat the liquid in this
experiment. Drop a piece of solid iodine
pentoxide in the cold solution of hydrazine
dihydrochloride. As soon as the piece of
iodine pentoxide falls in the solution, the reaction
starts. Immediately, a big bubble of nitrogen is formed
and even in this short time from the start of the
reaction (just a few tens of ms), a clearly visible
purple color of iodine vapor can be observed. This
picture was made with a high speed camera at 1000 fps. The reaction itself is quite
interesting to watch, even without high speed camera. A
big plume of purple iodine vapor escapes from the test
tube:
Ignition of flash
powder by chlorine gas This experiment combines several
reactions into an impressive experiment, which also
works very well as a demonstration experiment. It is
well-known that red phosphorus reacts exothermically
with halogens. With chlorine the reaction is so
exothermic, that the red phosphorus ignites. A mix of
aluminium powder and potassium perchlorate (a flash mix)
burns extremely fast and hot, with a white flash. The
flash mix, however, is somewhat hard to ignite. The heat
of burning red phosphorus, however, is sufficient to
ignite the flash mix, if the phosphorus is sufficiently
finely divided throughout the mix. So, for this
experiment, a tiny amount of red phosphorus is mixed
with aluminium and finely powdered potassium
perchlorate. Simply immersing this mix in chlorine gas
sets off the mix. Note 1: A mix of red phosphorus and potassium perchlorate can be handled fairly safely, as long as the potassium perchlorate does not contain any chlorate impurity. For this experiment only a few tens of mg are mixed, so the risk is small anyway. Note 2: In the EU, potassium
perchlorate and sodium perchlorate cannot be obtained
anymore. Potassium nitrate can be used instead, but the
reaction is somewhat less spectacular. The flashes with
the nitrate are less intense. For this experiment, I
prepared a little potassium perchlorate from waste of
other experiments. Perchloric acid can be obtained
legally in the EU and I used that for other experiments
on transition metal complexes and the waste of these
experiments I kept and from that I made a small quantity
of potassium perchlorate (this is the only perchlorate
which can easily be made from that waste in a pure
state, due to its low solubility in cold water).
Ammonium perchlorate also can be obtained legally and
that can also be used to make small quantities of
potassium perchlorate. Using ammonium perchlorate
instead of potassium perchlorate does not give good
results. The mix with ammonium perchlorate burns much
slower. If you really need to use a substitute, then use
potassium nitrate. Do not use chlorate! Pour 20 ml or so of dilute
hydrochloric acid in an erlenmeyer. Add a teaspoon of granular
calcium hypochlorite to the acid. Adding 10 ml of
concentrated bleach also works. Use of TCCA is not
recommended, because of foaming. Wait till the
erlenmeyer is full of chlorine gas. Avoid inhaling the
gas! Using a metal spatula, pour
some of the powdered flash mix with phosphorus into the
chlorine gas in the erlenmeyer.
Another set of pictures was made, also with 10 ms intervals between images. In that series, there are many sparks, and the mix used in that experiment burns even hotter. Two videos can be downloaded of this reaction: video1 and video2. |
Discussion of results
In
the first experiment, copper reacts with nitric acid,
giving copper(II) ions in solution and nitrogen dioxide
gas. Under the conditions in this experiment (quite warm
and also quite concentrated acid), the main gaseous
product, produced in the reaction between copper metal
and nitric acid is the brown NO2 gas. The
reaction equation is: Cu + 4 HNO3 → Cu2+ +
2 NO3–
+ 2 NO2
+ 2 H2O 3 Cu
+ 8 HNO3 → 3 Cu2+
+ 6 NO3–
+ 2 NO + 4 H2O In practice, none
of the above reactions occurs exclusively, there will
always be a combination of both reactions, at the
start, when the acid is still concentrated, mainly the
first one and at the end mainly the second one. So,
this reaction between copper metal and nitric acid is
not really suitable to make pure NO2 or
pure NO, one gets a mix of these gases.
In the second experiment, iodine pentoxide
reacts with hydrazine. In solid hydrazine
dihydrochloride, the hydrazine is protonated twice,
present as an ion +H3N-NH3+.
In solution, this ion decomposes and when the solid salt
is dissolved in water, then the compound ionizes as
follows: N2H4·2HCl → N2H5+ + H+ + 2 Cl– The solution becomes strongly
acidic. It contains nearly no free hydrazine. Hydrazine
is a strong reductor, regardless of whether it is
protonated or not. Iodine pentoxide, on the other hand,
is a strong and very facile oxidizer, and hence, when
these two compounds are brought in contact with each
other a very violent and exothermic reaction occurs: 3 N2H5+ + I2O5 →
3 N2 + 2 I–
+ 5 H+
+ 5 H2O + heat When there is excess iodine
pentoxide, then any iodide reacts with iodine pentoxide
to iodine in the presence of acid. This explains the
formation of all the iodine vapor. On the solid piece of
iodine pentoxide, which also is covered with a lot of
gaseous nitrogen, the amount of hydrazine quickly is
used up and any iodide ion then is quickly oxidized to
iodine: Due to the heat, produced in
the reaction with hydrazine, the iodine partially
evaporates and escapes as purple gas. The rest remains
in solution as brown iodine and some is precipitated as
nearly black solid.
In the third experiment,
phosphorus reacts with chlorine, producing heat, and
this in turn ingites the flash mix of aluminium and
potassium perchlorate: 2 P + 3 Cl2 →
2 PCl3 + a lot of heat The heat is sufficient to ignite the
flash mix: 8 Al + 3 KClO4 → 4 Al2O3 + 3 KCl + much more heat The reaction between aluminium and
potassium perchlorate produces a really large amount
of energy, leading to white hot particles and
emission of a lot of light. The loose powder,
falling freely, does not really give an explosion,
but a finely powdered intimate mix of aluminium and
potassium perchlorate, when in a pile on a spoon,
can explode, due to self-confining, once it is
ignited.
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