On 12/7/2023 5:42 AM, The Natural Philosopher wrote:
On 07/12/2023 10:39, Jeff Layman wrote:
On 07/12/2023 10:17, The Natural Philosopher wrote:
On 07/12/2023 09:35, Paul wrote:
On 12/7/2023 3:23 AM, Jeff Layman wrote:
On 06/12/2023 22:37, Tim Streater wrote:
On 06 Dec 2023 at 21:23:36 GMT, "alan_m" <junk@admac.myzen.co.uk> wrote: >>>>>>
For batteries in my wireless temperature sensors in the fridge and >>>>>>> freezer I use Energiser Ultimate Lithium. Although expensive they work >>>>>>> down to -40C whereas alkaline batteries are unreliable in the freezer as
they are only specified to -20C
I use these in the sensors for my garage doors. They have the longest life of
any I've tried so far.
They have some interesting chemistry inside...
<https://www.youtube.com/shorts/yGDkiUAwxRs>
The datasheet makes no specific mention of
what would happen in a long term immersion of
a battery. They don't want the contents exposed
to water, and that's why the thing has the layers
that it does. But I don't see anything guaranteeing
against the cell eventually being penetrated by
water internally.
Lithium Primary cell.
https://data.energizer.com/pdfs/lithiuml91l92_appman.pdf
2 Li(s) + 2 H2O -> 2 LiOH (aq) + H2(g) [Exothermic]
What makes you think that there is any lithium *metal* in the cells at all? >>
Because there is a small amount - less than 1g according to:
<https://batteryspecialists.com.au/blogs/news/everything-there-is-to-know-about-the-energizer-lithium-battery>
(This agrees with the product data sheet, which says the battery contains less than 1g. The SDS says it contains about 6% of lithium or lithium alloy. As the AA weighs about 15g, this confirms the lithium content)
No. 'less than' does not equal 'equal'.
The lithium is in the electrolyte, as a salt.
But you saw the Youtube video, right ?
You saw the alkali metal response to water.
We don't know what the exact (layered) setup
of the foil is, but at a guess, the outside layer
is an alkali metal. Maybe the substrate of the
foil, tends to be flammable. (Or, it could be
the chemical residue on the ribbon, which
aids in the response.)
That's a more vigorous response than the one you
get in schooling, where they take a piece of
sodium from sodium-under-oil jar, and drop that
into water. How that one differs, is it is not
self-igniting as easily. Other materials in that
series of the periodic table, are more energetic.
We also had a TV series, shown on Saturday mornings,
where they walk through the entire periodic table, demonstrating
the elements. And you get to see the vigorous reactions
of some of them.
https://en.wikipedia.org/wiki/Don_Showalter
"In 1988 Showalter became the series demonstrator in a 26-program
PBS education series by Annenberg/CPB, The World of Chemistry,
opposite with series host, Nobel prize winner Roald Hoffmann.
While Hoffmann introduced a series of concepts and ideas, Showalter
provided a series of demonstrations and other visual representations
to help students and viewers to better understand the information."
https://archive.org/stream/TheWorldOfChemistry/The%20World%20Of%20Chemistry/07%20-%20The%20Periodic%20Table/World%20of%20Chemistry%20-%20Transcript%2007%20-%20The%20Periodic%20Table_djvu.txt
We call this family the alkali metals.
They make up Group 1 in the periodic
table. The first element is lithium, and
then there's sodium, and potassium.
Down here is rubidium, and this one is
cesium. And do you notice anything that
they all have in common? You probably
see that they're all stored in very
unusual ways.
I'm gonna take
a piece of this lithium and put it into the
water. And watch what happens, how it
Starts to fizz a little bit. The fizzing now
is the reaction of lithium with the water
to produce hydrogen gas. Let's try the
sodium. I'll get a small piece of that,
not too big, because we don't want the
reaction to be too violent. Oh, that
reacts much faster, doesn't it? See the
sodium bouncing around there, again
fizzing, giving off that hydrogen gas.
Okay. Let's try potassium, the most
reactive of the three. I'll get a small
piece of that and put it into the water.
Wow! That really reacted violently.
Did you see the immediate reaction of
the potassium? Again, it's formed that
hydrogen gas and the hydrogen gas was
ignited.
Using a thin ribbon, having a decent surface
area, accelerates the reaction. If the foil
continued to be rolled up, the reaction
could not consume the material with the same
speed, which is where some of the "safety"
comes from.
Paul
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