What we call heat is, technically, the kinetic energy of molecules vibrating around
I’ve wondered about this. If this is so, and heat is molecules moving back and forth, how do the molecules stop, change direction, and then accelerate in the other direction, stop, change directions again, and go back, over and over and over?
It’s pretty much like billiards. They just bounce. Different chemicals (types of molecule) are different phases at different temperatures e.g. nitrogen is a gas at room temp, water is liquid. Stuff that’s a gas at room temp just has less bonding forces (and often mass) than liquids or solids. So they don’t take as much heat to go fast. There’s a lot of heat even at room temp, and even at -40deg. The temperature for nitrogen to sit in one place is -210C or -346F.
Yeah, I do apologize - I’m somewhat simplifying my explanation because when you start going into the full detail, it just brings up more questions.
So yes, like the other comment says, the particles are constantly bouncing into other things.
If they’re bounded in by something - walls of a container, or even just more gas surrounding the specific sample you’re looking at - they’ll bump into that, and transfer some of their energy to that.
If they don’t have something to bump off of and the particles are free-floating, they’ll take off in any given direction. If they only have something to bump off of in a limited number of directions, they’ll take off in the other direction. (For instance, in a rocket engine, we make a lot of molecules really, really hot and then surround them with barriers in every direction except the one we want them to zoom out in.)
In some cases, the molecules have electromagnetic bonds with each other, which take more energy to break than the energy contained in their “bouncing around”. So they’ll stay stuck, just bouncing off each other, even in a vacuum, (Or at least, until they radiate away their heat via electromagnetic energy… another whole story.)
Molecules interact with each other. Energy is transferred as they bump around. If you were to follow a single molecule it would move around randomly. What we can measure is usually the average of many molecules.
So it’s less of vibrating and more about smashing around into things?
This is easier to envision with a gas: like a chamber of balks all ricocheting like mad. It’s harder to envision for a solid. But I guess a molecule will be up smack against its neighbors, getting repelled, not so much bounding freely?
So in a solid, you can imagine each atom connected to each other by springs (bonds). They can vibrate on these springs. If they vibrate too much (by heating) then they can break the bonds and escape as a gas. Gasses basically have too much energy to bond again.
Even solids are mostly nothing. This is why neutron stars are so dense - there is a lot less nothing between the neutrons, largely due to gravity.
Here’s another way to think about it. A gas is like a bunch of balls bouncing around a room, hitting the walls and occasionally each other. A solid is like a ball pit, but the balls are vibrating. There is still a lot of bouncing, but most of themstay together.
I’ve wondered about this. If this is so, and heat is molecules moving back and forth, how do the molecules stop, change direction, and then accelerate in the other direction, stop, change directions again, and go back, over and over and over?
It’s pretty much like billiards. They just bounce. Different chemicals (types of molecule) are different phases at different temperatures e.g. nitrogen is a gas at room temp, water is liquid. Stuff that’s a gas at room temp just has less bonding forces (and often mass) than liquids or solids. So they don’t take as much heat to go fast. There’s a lot of heat even at room temp, and even at -40deg. The temperature for nitrogen to sit in one place is -210C or -346F.
Yeah, I do apologize - I’m somewhat simplifying my explanation because when you start going into the full detail, it just brings up more questions.
So yes, like the other comment says, the particles are constantly bouncing into other things.
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Nothing to apologize for - thank you for elaborating.
Molecules interact with each other. Energy is transferred as they bump around. If you were to follow a single molecule it would move around randomly. What we can measure is usually the average of many molecules.
So it’s less of vibrating and more about smashing around into things?
This is easier to envision with a gas: like a chamber of balks all ricocheting like mad. It’s harder to envision for a solid. But I guess a molecule will be up smack against its neighbors, getting repelled, not so much bounding freely?
So in a solid, you can imagine each atom connected to each other by springs (bonds). They can vibrate on these springs. If they vibrate too much (by heating) then they can break the bonds and escape as a gas. Gasses basically have too much energy to bond again.
Even solids are mostly nothing. This is why neutron stars are so dense - there is a lot less nothing between the neutrons, largely due to gravity.
Here’s another way to think about it. A gas is like a bunch of balls bouncing around a room, hitting the walls and occasionally each other. A solid is like a ball pit, but the balls are vibrating. There is still a lot of bouncing, but most of themstay together.