"Steve Peterson" wrote in message
link.net...
2Al + 6HCl -- 2AlCl3 + 3 H2 sorry, no subscripts for email
but 2Al + 6OH- -- Al2O3 + 3 H2O

The proper equation
http://www.madsci.org/posts/archives...1850.Ch.r.html
The process
http://www.elmhurst.edu/~chm/demos/hydrogenbubbles.html

so the reaction with acid produces hydrogen gas

Aluminum chlorhydrate - anti perspirant.

http://www.scienceproject.com/projec...nior/SC040.asp

On Sun, 16 Oct 2005 09:12:53 -0400, "George" George@least wrote:

,;
,;"Dave Jackson" wrote in message
arthlink.net...
,; put some strips of aluminum foil in the bottle and add a little HCL ("The
,; Works" toilet bowl cleaner works real well) tighten the cap, give a shake,
,; and toss out back. In a few minuites there will be a real big "BANG" when
,; the bottle explodes from the reaction. be sure to stay clear! --dave
,;
,;
,;You'll want to review your inorganic chemistry. It's hydroxides you're
,;after if you want to generate hydrogen. Lye is the preferred for its punch
,;by weight. Drano and some other drain cleaners even include some aluminum
,;chips for the foaming and the mechanical action it generates.

I would suggest that you review your inorganic chemistry before
pontificating.

Aluminum metal reacts with either strong base or strong acid to
produce hydrogen.

"George" George@least wrote in message
...

"Steve Peterson" wrote in message
link.net...
2Al + 6HCl -- 2AlCl3 + 3 H2 sorry, no subscripts for email
but 2Al + 6OH- -- Al2O3 + 3 H2O

The proper equation
http://www.madsci.org/posts/archives...1850.Ch.r.html
The process
http://www.elmhurst.edu/~chm/demos/hydrogenbubbles.html

so the reaction with acid produces hydrogen gas

Aluminum chlorhydrate - anti perspirant.

http://www.scienceproject.com/projec...nior/SC040.asp

It says:
"Explanation: The aluminum foil in the presence of NaOH pellets reacts with
water, producing hydrogen gas. As the gas rises from the flask, it travels
through the tube to the beaker of water. Since hydrogen gas is less dense
than water, it bubbles out of the water.

When producing a gas, more molecules are being made. The number of
collisions the molecules make against their container makes pressure.
Therefore, the more molecules made, the more collisions occur, creating a
greater pressure. When the gas is fed into the upside down test tube, the
bubbles of gas create a pressure which pushes the water out of the test
tube.

The hydrogen gas now in the test tube is flammable. So when I hold the tube
over the flame, the hydrogen gas ignites and creates a popping sound. It is
like a tiny bomb or fireworks.

Al + NaOH --- H2 + Al3+ + Na+

H2 + O2 --- H2O + energy"

The first reaction isn't balanced, where did the O go? The explanation says
Al reacts with water; where is that reaction? No problem with the second
rxn, but it produces water, rather than reacting with it.

Screw the cap onto an empty bottle and you have a great dog toy.

Mark

"Steve Peterson" wrote in message
hlink.net...



The first reaction isn't balanced, where did the O go? The explanation
says Al reacts with water; where is that reaction? No problem with the
second rxn, but it produces water, rather than reacting with it.



Read for understanding. Note the sodium tetrahydroxoaluminate product.
http://www.madsci.org/posts/archives...1850.Ch.r.html

Note also the amount of water bound in the chlorhydrate in the second.
That's a reaction, too.

Reactions with acids are slowed because of the self-protective coat of oxide
that makes aluminum so useful in exposure to the elements and carbonic acid
(Pepsi). That's why I said you wanted (K)(Na)OH for punch in Hydrogen
production.

That rxn I can accept, but it certainly isn't what you listed first.

Steve

"George" George@least wrote in message
...

"Steve Peterson" wrote in message
hlink.net...



The first reaction isn't balanced, where did the O go? The explanation
says Al reacts with water; where is that reaction? No problem with the
second rxn, but it produces water, rather than reacting with it.



Read for understanding. Note the sodium tetrahydroxoaluminate product.
http://www.madsci.org/posts/archives...1850.Ch.r.html

Note also the amount of water bound in the chlorhydrate in the second.
That's a reaction, too.

Reactions with acids are slowed because of the self-protective coat of
oxide that makes aluminum so useful in exposure to the elements and
carbonic acid (Pepsi). That's why I said you wanted (K)(Na)OH for punch
in Hydrogen production.

On Mon, 17 Oct 2005 01:00:00 GMT, "Steve Peterson"
wrote:

,;
,;"George" George@least wrote in message
...
,;
,; "Steve Peterson" wrote in message
,; link.net...
,; 2Al + 6HCl -- 2AlCl3 + 3 H2 sorry, no subscripts for email
,; but 2Al + 6OH- -- Al2O3 + 3 H2O

Al
,;
,; The proper equation
,; http://www.madsci.org/posts/archives...1850.Ch.r.html
,; The process
,; http://www.elmhurst.edu/~chm/demos/hydrogenbubbles.html
,;
,; so the reaction with acid produces hydrogen gas
,;
,; Aluminum chlorhydrate - anti perspirant.
,;
,; http://www.scienceproject.com/projec...nior/SC040.asp
,;
,; It says:
,;"Explanation: The aluminum foil in the presence of NaOH pellets reacts with
,;water, producing hydrogen gas. As the gas rises from the flask, it travels
,;through the tube to the beaker of water. Since hydrogen gas is less dense
,;than water, it bubbles out of the water.
,;
,;When producing a gas, more molecules are being made. The number of
,;collisions the molecules make against their container makes pressure.
,;Therefore, the more molecules made, the more collisions occur, creating a
,;greater pressure. When the gas is fed into the upside down test tube, the
,;bubbles of gas create a pressure which pushes the water out of the test
,;tube.
,;
,;The hydrogen gas now in the test tube is flammable. So when I hold the tube
,;over the flame, the hydrogen gas ignites and creates a popping sound. It is
,;like a tiny bomb or fireworks.
,;
,;Al + NaOH --- H2 + Al3+ + Na+

Actually the reaction is between aluminum and water. The NaOH just
dissolves the protective oxide coating. You will note in your reaction
(above) that the sodium does not change valence.

2 Al + 6 H2O --- 2 Al(OH)3 + 3 H2

This can be demonstrated with a trace of mercury on the aluminum
surface. With mercury present the reaction goes until you run out of
aluminum or water. This reaction runs using moisture in the air.
,;
,;H2 + O2 --- H2O + energy"
,;
,;The first reaction isn't balanced, where did the O go? The explanation says
,;Al reacts with water; where is that reaction? No problem with the second
,;rxn, but it produces water, rather than reacting with it.
,;