How is this possible (fisiks quiz)?

[VetLegion]

A package of soda with 6 plastic bottles of 1,5 litre each is stored out on the balcony. It is cold but they are not frozen. I take one bottle inside, where it is quite warm (over 25 C). I open it, pour myself a glass and immediately the soda in the bottle starts freezing, ice forming in front of my eyes. I try this with other bottles and it's the same.

What happened?

[Lul Thyme]

They were below freezing temperature but the pressure kept them from turning to ice?

[VetLegion]

Probably! Mods, you can lock this thread now

[BeBMan]

I read somehwere that water could be prevented from freezing even below zero C at least in certain conditions. To those belong an environment that does not allow for a certain level of crystallization (is that the right term?) needed to get it to ice. Movement is another factor mentioned that favors said crystallization.

So maybe you broke those conditions when you openened the bottle and poured the water in a glas so the (still very cool) water could turn into ice then.

My 0.1 cents. Maybe I'm totally wrong.

KH

[Tuberski]

He was standing behind you.....



ACK!

[Dinner]

Originally posted by Lul Thyme
They were below freezing temperature but the pressure kept them from turning to ice?

Yep.

[The Vagabond]

This is due to the gas dissolved in soda (carbon dioxide -- CO2), which lowers the freezing point (by several degrees for the ordinary soda). When you pour the soda into a glass, part of the gas is gone, its concentration in the soda drops, and consequently the freezing point rises. The temperature of the liquid cannot change so rapidly, so the liquid suddenly finds itself at a temperature below the (new) freezing point and gets frozen.

[snoopy369]

I think the pressure mattered at least as much as the CO2, but both certainly have an effect. I don't think so much CO2 evaporated in the few seconds as to drop the FP that much...

[Heraclitus]

Originally posted by Lul Thyme
They were below freezing temperature but the pressure kept them from turning to ice?

I seriously doubt the thin aluminum sheet can produce that kind of pressure.

Edit: Ahh, plastic container. Vetlegion could you post a pic and perhaps read the label and inform us of the material?

[Heraclitus]

Originally posted by The Vagabond
This is due to the gas dissolved in soda (carbon dioxide -- CO2), which lowers the freezing point (by several degrees for the ordinary soda). When you pour the soda into a glass, part of the gas is gone, its concentration in the soda drops, and consequently the freezing point rises. The temperature of the liquid cannot change so rapidly, so the liquid suddenly finds itself at a temperature below the (new) freezing point and gets frozen.

I think this is a better explanation.

[The Vagabond]

Oh no, the pressure must not play a role here. This effect is very weak. Even if you doubled the atmospheric presure, the freezing point would barely change.

Edit: this was an answer to snoopy369.

[Heraclitus]

Originally posted by The Vagabond
Oh no, the pressure must not play a role here. This effect is very weak. Even if you doubled the atmospheric presure, the freezing point would barely change.

Exactly, I think I even sort of remember the proper equation. It’s a trivial matter, but I can say the pressure involved here is way to small.

[The Vagabond]

OK, Heraclitus. We seem to agree.

[Dauphin]

Umm, it doesn't have to be fizzy either.

Check out the supercooling videos on t'internet:

[The Vagabond]

Interesting video. But I don't quite trust the comments given by the author of the video. A bottle of Walmart purified drinking water supercooled to -21 C?? This sounds strange.