- Introduction to energy
- Types of energy
- First Law of Thermodynamics introduction
- Introduction to entropy
- Second Law of Thermodynamics
- Second Law of Thermodynamics and entropy
- Why heat increases entropy
- The laws of thermodynamics
- Energy and thermodynamics
Introduction to entropy, and how entropy relates to the number of possible states for a system.
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- Wait, if energy cannot be destroyed or created, then how does the entropy of the universe increase over time?(49 votes)
- Entropy is not energy; entropy is how the energy in the universe is distributed. There is a constant amount of energy in the universe, but the way it is distributed is always changing. When the way the energy is distributed changes from a less probable distribution (e.g. one particle has all the energy in the universe and the rest have none!) to a more probable distribution (e.g. most particles have an amount of energy close to the average), we say that the entropy increases.(120 votes)
- So, is entropy this disease / virus, or is it actually profitable for this Sun-dude to have entropy.
Like, is it a bad thing(-) or good thing(+) ? Or does it make no difference?
How does knowledge of entropy affect us ? Does it appear in our daily life or something?(19 votes)
- It's just a tendency of the universe. We, as living beings, fight against the increase of entropy in our bodies, as a result, it's a little bad for business if you consider it's inevitable that entropy increases.
On the other hand, it doesn't really matter for non-living beings. In fact, it may even be benefitial if you consider that non-living beings tend to the most stable state, such as an electron that "wants" to be in the shell closest to the nucleus. Heat is the highest state of entropy, supposedly, and that's where it all tends to: the heat death of the universe is when it finally becomes just heat, evenly distributed across space.(13 votes)
- Please provide some clarification.
I just don't see the moon - sun comparison as being a good example. For instance, I easily imagine a piece of sun breaking off and evolving to a collection of fused protons collapsing into a sphere similar to moon. But I can't imagine the reverse... a group of moons coming together to become our fusion-driven Sun.
I think I get Sal's mediating point that with quantity part of the Entropy equation, the Sun wins hands-down. And in the context of the age of the Universe, the variance between Moon/Sun energy states is likely small. But from my earth-view, it looks like the moon has runs its course and reached its lowest state ... unlike the Sun whose future processes are described to us in science class.(12 votes)
- What you describe, a piece of the Sun breaking off and fusing together to a cold lump of rock, can only happen when the energy in that piece of the Sun escapes the system. By the first law of thermodynamics, energy is never destroyed. In the Sun's case, it radiates outward in the form of light, and this light would ultimately increase the entropy of some other place in the universe.
On the other hand, imagine what would happen if the Moon would collide with some other cool object like the Earth. The particles from the Moon and the Earth would be sent in all sorts of unpredictable directions, which would require lots of information to describe. In other words, entropy increases. Chaos ensues, if you like. Both bodies would also heat up from the friction. And if enough moons would collide, a star could theoretically be born (though most stars are currently fusing hydrogen or helium, which the Moon has fairly little of).(15 votes)
- why hot water has less entropy (S < 0) and cold water has great entropy (S > 0)?(5 votes)
- It is because water when it goes from 4 degrees celsius to less, expands in volume and thus gains entropy.(5 votes)
- I'm a bit confused about what is considered as a "high" entropy. If an object is able to have more molecule configurations, does that mean it has a higher entropy?(5 votes)
- Yes. More configurations = more entropy. In fact, entropy = K times the log of the number of configurations. S=K log W, or S=K log omega. (To really nail down what these configurations are, we need to get into quantum mechanics. Also, if we are interested in things that radiate photons, we must take into account the number of possible configurations of the photons.) (Also if we are interested in changes to the molecules themselves, then we need to take into account the possible configurations of the particles which make up the molecules.)(4 votes)
- But the messy room creates more potential energy for me, right? If I had to walk over or trip over everything, wouldn't that convert the potential energy to kinetic energy? I totally get what you're saying, Sal. I just want to understand that part. *Curiosity.(3 votes)
- The probability of tripping over something in a tidy room can also be higher if the room is bigger & has more objects than a messy room. This way even a tidy room can have more entropy than a messy room.(3 votes)
- Which has more entropy? A star or a black hole with the same diameter? The black hole has more mass, but the star would have the ability to move the molecules more. Or is that incorrect?(2 votes)
- A black hole has the maximum possible entropy for the volume of space inside their event horizon.(3 votes)
- how the entropy is constantly increasing in the universe(3 votes)
- In the large fields of nebulae gas molecules will often clump together, due to their gravitational attraction. . This would seem to reduce the number of microstates. How does this not violate the second law of thermodynamics?(1 vote)
- The heat radiates out into the rest of the universe. Locally entropy is lower, but non-locally it increases.(4 votes)
- But how exactly is entropy related to biology?(1 vote)
- Living organisms exist by finding a way to decrease entropy locally even though the entropy of a closed system never decreases. This means living organisms have to take in energy from the environment around them.(4 votes)
What I want to do in this video is start exploring entropy. When you first get exposed to the idea entropy it seems a little bit mysterious. But as we do more videos we'll hopefully build a very strong intuition of what it is. So one of the more typical definitions, or a lot of the definitions you'll see of entropy, they'll involve the word disorder. So it might be considered the disorder of a system. Now with just that definition in your head, I want you to pause this video and I want you to compare this system to this system. I want you to compare this room to this room, and ask yourself, which of these has more entropy. And then I want you to compare the moon here to the sun, and these clearly aren't at scale, the sun would be way more massive or way larger if I was drawing it to scale. But which of these systems has more entropy? Alright, so I'm assuming you've had a go at it. So when you look at these rooms you might say okay this room over here, this looks ordered, It's a clean room. And this over here looks disordered, it's a messy room. So if all you had is this definition, you'd say okay maybe this one is more disordered, maybe this one has more entropy. And you wouldn't be alone in thinking that. In fact, even in a lot of textbooks they'll use this analogy of a clean room verses a messy room. And the messy room somehow being indicative of having more entropy. But this isn't exactly the case. This form of disorder is not the same thing as this form of disorder. So let me make this very, very clear. So something being messy, does not equal entropy. To think about what disorder means in the entropy sense we're going to have to flex our visualization of muscles a little bit more, but hopefully it'll all sink in. Entropy, this kind of a disorder is more of the number of states that a system can take on. What do I mean by states of a system? Well if I have a container like this, and if I have four molecules that are bouncing around. So I have this magenta molecule, I have this blue molecule, I have this yellow molecule right over here, and then I have a green molecule. Well this would be a particular state, a particular configuration. But that system these molecules are bouncing around could take on other configurations. Or it could take on other states. Or maybe the yellow molecule is over here, they bounce around enough for the yellow molecule to get there, the blue molecule to get over here, maybe the pink molecule is now over here, and the green molecule is now over here. And so a system can take on a bunch of different states. I've just drawn two states for this system. But there could be many, many more states for this system. So each of these are a particular state for the system. So imagine this system where I have this box with the four molecules in it, and let's compare it to another system where I have a larger box. And let's say it has even more molecules in it. Let's say that it has two yellow molecules, let's say that is has a blue molecule, let's say that it has a green molecule, let's say that it has a magenta molecule, this is fun. Let's say it has a mauve molecule right over here. So this system that is larger, there's more places for the molecules to be and there's actually more molecules in it. This can actually take on more configurations or more states. I've just drawn one of them but there's many more. If you imagine these molecules all bouncing around in different ways there's many, many different states that it could take on. So the system without even knowing what the actual molecules are doing at that given moment in time, we would say that there's more possible states relative to this one, this has fewer possible states. And because this system over here has more possible states, more configurations, it would take more to tell you exactly where everything is. We would say that this has more entropy. So when we talk about disorder, we're really talking about the number of states something could have. And it makes sense that this thing you could imagine there's a lot more stuff moving around and a lot more different directions and they have a lot more space to move around. So it makes sense that the system as a whole has more entropy. So when we talk about entropy we're not talking about any one of the particular states, any one of the particular configurations, we're talking about the system as a whole without really knowing exactly where the molecules are. In this example with the rooms, we're just talking about particular states. Messy is a particular state, clean is a particular state. But we're not talking about the number of configurations that a room could actually have. In fact if this room is larger, this room actually could have more configurations. And if we're talking about the molecular level if this room was warm and this room were cold, and actually if this room is just larger, it's going to have more molecules in it. And those molecules are going to be in way more configurations that they could be arranged so there could be an argument that this actually has a higher entropy. And so using that same reasoning, let's go back to that comparison of the moon and the sun. Which of these would have more entropy? Well let's think about it. The sun is larger, it has way, way more molecules and those molecules are moving around way faster and they're hotter and they're moving past each other. While the moon is small, it's cold, it has fewer molecules. It's for the most part rigid, it doesn't have a very high temperature so these things aren't moving around a lot. It has way fewer states, way fewer configurations than the sun does. So the sun's entropy, if you view it as a system. If you view the sun as a system, it's entropy is way higher than the moon. It's entropy is much larger than the entropy of the moon. Think about it, how much information you would need. You would need a lot of information if someone wanted to tell you where every molecule or every atom on the moon is. But you would need even more to know where every atom or molecule for in a given moment on the sun is. If you're just looking at the sun, wow all these things are moving around and it's this huge volume. And they're very energetic and all of these molecules. So hopefully this starts to give you a sense of what entropy is. And you might say okay this is all fun intellectual discussion, what's the big deal? But the big deal is that to some degree you can describe the universe in terms of entropy. As we learn in the second law of thermodynamics, the entropy in the universe is constantly increasing. We are constantly moving to a universe with more possible states, which has all sorts of interesting implications.