On 22/04/2020 11:49, Spike wrote:
On 22/04/2020 10:24, Brian Reay wrote:
On 22/04/2020 09:17, Robin wrote:
On 22/04/2020 08:16, harry wrote:

They fail due to the air/gas inside heating up and expanding.
Bigger gaps have more air & therefore subjected to higher pressure.

Gay-Lussac's law: the pressure changes the same with temperature
independent of the volume.Â* Bigger gaps means more gas but also more
volume.

As I recall, Gay-Lussac's Law applies to an ideal gas. Chances an sealed
unit has (at least) some water vapour in it and isn't therefore an ideal gas.

The concept of an ideal gas is based on theory.

(Water vapour is a polarised molecule and that stops it being an ideal gas,
if I remember my Physics.)

You have remembered wrongly. I recall that real gasses are not ideal
gasses, whether they have water vapour in them or not. However, some
might approach ideal behaviour depending on the circumstances.


And in any event why would the departures from the ideal gas laws (which
do of course occur) be volume dependent? Does someone think the
molecules suffer from agoraphobia?

--
Robin
reply-to address is (intended to be) valid