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What the example of the statement the entropy of the universe can never decrease?
Wiki User
∙ 11y ago
If a source of heat energy starts radiating from a point and continues without stop the entropy around that point will never decrease. As sun is the endless heat energy radiating source and surrounding's of that is known as universe accepted by everybody. So this is the example for the statement ' the entropy of the universe can never decrease.'
Wiki User
∙ 11y ago
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What is a statement of the second law of thermodynamics?
Every reaction in the universe increases the disorder, or entropy, of the universe. This is because energy that goes into a reaction is usable energy, but after the reaction, the energy is not usable anymore.
Is ice melting an example of thermal energy?
Ummm . . . let's just say that thermal energy is used to melt ice.
What are the difference between the law of conversation of energy and law of degradation?
The difference between the two is that the law of degradation implies that there is a finite non-zero amount of potential energy that is used cause a process to happen. Recent theory suggests that this is caused by the expanding universe: more energy is converted to potential energy since objects in the universe are moving further and further away from each other. It is possible to create a process that will decrease the entropy of a system (in fact that is how we are able to reach temperatures in the microKelvin range), but the overall entropy of a closed system will always be increasing. This is different from the law of conservation of energy, which does not imply that this quantity exists. In a straight conservation of energy, it is theoretically possible for all the potential energy to converted to kinetic energy and all kinetic energy to be converted to usable potential energy. It is worth noting that the existence of entropy does not make the law of conservation of energy wrong. Think of it this way: the law of degradation of energy is an addition to the law of conservation of energy that states that some of the energy of a system must be stored as unusable potential energy. A real world example would be a middleman in a trade. It is theoretically possible that the middleman could buy items and sell them for the same price. However, the middleman would make no money to support himself and would starve. Therefore, he must buy items and then sell them at a higher price, thereby reserving some of the profit for himself. In this example, money would represent energy and the profit that the middleman makes represents the increasing entropy of the system. The total amount of money in the system stays the same, but the middleman must take some money for every transaction he completes in order for the system to keep functioning.
What is an example sentence for the word plasma?
Here is an example sentence with the word "plasma":It was hard to imagine that stars were merely burning balls of plasma in the universe.
Explain how the gravitational force between objects changes when the distance?
The gravitational force is inversely proportional to the square of the distance. For example, if you increase the distance by a factor of 10, the force will decrease by a factor of 100 (10 squared).The gravitational force is inversely proportional to the square of the distance. For example, if you increase the distance by a factor of 10, the force will decrease by a factor of 100 (10 squared).The gravitational force is inversely proportional to the square of the distance. For example, if you increase the distance by a factor of 10, the force will decrease by a factor of 100 (10 squared).The gravitational force is inversely proportional to the square of the distance. For example, if you increase the distance by a factor of 10, the force will decrease by a factor of 100 (10 squared).
What happens to the entropy in the reaction?
Entropy increases. In a reaction comprised of sub-reactions, some sub-reactions may show a decrease in entropy but the entire reaction will show an increase of entropy. As an example, the formation of sugar molecules by living organisms is a process that shows decrease in entropy at the expense of the loss of entropy by the sun.
What is an example of decrease?
This is a trick question, because in the world as we know it, entropy never decreases, since the chance of this happening approaches and infinitely small fraction. To answer the question though: Take any closed system of events that you've observed, and rewind the events as if you were "going back in time". Example: An egg the has splattered all of a sudden recombines off the floor and becomes a whole egg again. Some scientists believe that the last time entropy ever decreased in our universe was right before the big bang. Since this chance occurrence, entropy throughout the whole universe has been steadily increasing. My addition (person 2) - However, entropy CAN decrease locally, just not universally. Essentially entropy rests on the fact that work ultimately comes from a flow of heat energy from high to low, eventually balancing out. Once all the heat energy is uniform in the universe, we will experience "heat death" at which point no work will be able to be done. However, in systems WITHIN the closed system of the universe, entropy CAN be decreased. Freezing an ice cube, if you follow the entropy equation which I don't have with me, is one example of this. The cost of this local decrease in entropy is a universal increase in entropy from the heat released that is greater than the local decrease in entropy, thus the second law is not violated. Another example is biological growth. We humans develop from a single cell into a vastly complex arrangement of cells, but at the same time we produce heat that increases universal entropy more than our bodies decrease it.
Under what condition can entropy decrease in a system?
First of all, entropy is the defined as the extent to which something is disordered. In chemistry, for entropy in a SYSTEM to decrease, the products of a reaction must be less disordered than the reactants. The extent of "disordered-ness" can be seen by the physical states of the substances. A gas is more disordered than a liquid, which is more disordered than a solid. So, an example of a reaction that leads to a decrease in entropy is: HCl(gas) +NH3(gas) -----> NH4Cl(solid) So you see, there are more gaseous molecules in the reactant side of the equation than in the product side, which means the products are less disordered than the reactants. ----------------------------------------------- However, one must note that if the entropy of a system(reaction) decreases, the entropy of the surroundings should increase. This is because change in TOTAL entropy(A) = change in entropy of SYSTEM(B) + change in entropy of SURROUNDINGS(C). It is a rule that A must increase in every case ( have a positive value). If the B is negative(a decrease in entropy), C must be positive(an increase in entropy) to keep the value of A positive.
When someone order something don't he reduce entropy of the universe?
No. You can reduce the entropy of some system, but that will be at the cost of an entropy increase somewhere else. This is because it costs energy to put something in order. The TOTAL entropy in the Universe will always increase. For example, the entropy on planet Earth probably remains more or less constant over millions of years - but we do so using energy, mainly from the Sun, and the fact that energy from the Sun radiates into space is an increase of entropy; much greater than any small change of entropy on our planet.
What are Examples of entropy increasing?
This is a trick question, because in the world as we know it, entropy never decreases, since the chance of this happening approaches and infinitely small fraction. To answer the question though: Take any closed system of events that you've observed, and rewind the events as if you were "going back in time". Example: An egg the has splattered all of a sudden recombines off the floor and becomes a whole egg again. Some scientists believe that the last time entropy ever decreased in our universe was right before the big bang. Since this chance occurrence, entropy throughout the whole universe has been steadily increasing. My addition (person 2) - However, entropy CAN decrease locally, just not universally. Essentially entropy rests on the fact that work ultimately comes from a flow of heat energy from high to low, eventually balancing out. Once all the heat energy is uniform in the universe, we will experience "heat death" at which point no work will be able to be done. However, in systems WITHIN the closed system of the universe, entropy CAN be decreased. Freezing an ice cube, if you follow the entropy equation which I don't have with me, is one example of this. The cost of this local decrease in entropy is a universal increase in entropy from the heat released that is greater than the local decrease in entropy, thus the second law is not violated. Another example is biological growth. We humans develop from a single cell into a vastly complex arrangement of cells, but at the same time we produce heat that increases universal entropy more than our bodies decrease it.
Cosmologists expect the universe to?
They expect the Universe to continue expanding. Right now, the evidence is that the expansion is speeding up. They also expect entropy to continue increasing, so in the distant future, there will not be any free energy left to support life, for example. They also expect quite a few other things; the Wikipedia article on the "future of the Universe" can give you some ideas.
The sun was the center of the universe is an example of?
The sun was the center of the universe is an example of:
When Energy Is Used Is It Gone Forever?
If it is an isolated system, then according to the second law of thermodynamics, it should decrease its entropy and continues to reach a thermal equilibrium. Energy is never lost nor created, so no, heat is not the final stage of energy that is wrong. The universe too will one day reach to its maximum entropy and there will no longer be any free energy for matter to interact with to perform work. But the energy of the universe will always remain the same. It is the disorderly of different energy states that allows free energy to be harnessed, for example, two adjacent rooms with a door in the middle having different temperature, the other being hotter while the other is colder, the moment the door is opened, hot air from the room will move to the colder room as what we observe as wind, that motion of air particles from hot to cold is free energy which can be used to perform work. Overtime, the temperature of the two rooms will equalize and there will no longer be any free energy to use. Say, at the beginning they have a room temperature of 30 C and 20 C, they have a difference of 10 C, therefore they are not a their thermal equilibrium, overtime they will settle to a final temperature (25 C) to follow the second law. The universe at its infancy was in a thermodynamic equilibrium, but because of quantum fluctuations, some areas had more matter than the other, causing an imbalance in the gravitational forces allowing the entropy of the universe to decrease, overtime the entropy of the universe will (or might have) reach minimum and will eventually increase as the system balances itself to a thermal equilibrium.
Claim: Schools should decrease class size by hiring more teachers. Which statement is an example of a commonsense counterclaim to the claim above?
A decrease in class size would require more teachers, which would be too expensive :) -Apex-
What is an increase in entropy?
In almost every process there is an increase in the entropy in the universe. For example, lets say your room is dirty so you think you are decreasing entropy by cleaning it up (decreasing disorder). The truth is that you expend a great amount of energy cleaning your room, and that energy is ultimately released into the universe as heat energy. That heat energy is a less ordered form of energy than the form you received it in, which are the chemical bonds in food. The chemical bonds in food are relatively ordered, but heat energy is very random. heat energy dissipates into the universe randomly, with little order or integrity. So you see, no process conserves all the energy in the process, as some energy is dissipated, or "wasted", as heat energy. When you hit a pool ball into another, the friction between the balls takes some of the energy of the collision away, in the form of friction. Friction generates heat (as you know from rubbing your hands togeter in the cold). I hope these brief examples demonstrate that all processes increase the entropy of the universe (in the form of heat energy).
When does entropy increases?
Entropy increases when ever energy is used up. Energy cannot be destroyed, but it is always lost in the form of unusable energy. Entropy is the % of unusable energy compared to usable energy in a given system.
What is a statement of the second law of thermodynamics?
Every reaction in the universe increases the disorder, or entropy, of the universe. This is because energy that goes into a reaction is usable energy, but after the reaction, the energy is not usable anymore.
