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What else can I help you with?
Explain the second law of thermodynamics and explain why it is not violated by living organisms?
this increase in organization over time in no way violates the second law. The entropy of a particular system, such as an organism, may actually decrease, so long as the total entropy of the universe-the system plus its surroundings-increases. Thus, organisms are islands of low entropy in an increasingly random universe. The evolution of biological order is perfectly consistent with the laws of thermodynamics.
How can an endothermic reaction be spontaneous at room temperature?
An endothermic reaction can be spontaneous at room temperature if the increase in entropy of the system is large enough to overcome the energy input required for the reaction. This can happen if the products of the reaction have higher entropy than the reactants. As a result, the overall change in free energy can be negative even though the reaction is endothermic.
What happens to the entropy of a system as more heat is added beyond the boiling point?
Fundamentally, if the entropy of a system increases, that means that the energy of the system ("normalized" to , i.e., divided by the temperature of the system) has become more "dispersed" or "dilute". For instance, if a system increases its volume at constant energy and temperature, then the energy per unit temperature is now more "dilute", being spread over a larger volume. All spontaneous processes result in a "dilution" or "spreading out" of the energy of the universe. The more dilute the energy of a system is (the higher the entropy of that system) the harder is is to harness that energy to do useful work. Another useful way of thinking about entropy is to consider it as a measure of the amount of information needed to completely specify the state of a system. Ultimately, this means how much information is needed to specify the positions and momenta of every particle in the system.
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.
Can entropy be zero?
I am not sure whether you refer to delta S (change in entropy) or entropy itself. So I'll answer for both.For S (entropy), which is defined by the function S=kln(omega), where k is Boltzmann's constant and omega is the number of microstates corresponding to a given state, the answer is no. Why? Omega (the number of microstates possible for a certain state) can never be smaller than one. Since Boltzmann's constant is a positive number and ln(omega) will always be greater or equal to zero, entropy will never be negative.However, when calculating delta S (change in entropy in a thermodynamic process), yes entropy can be negative. Remember entropy is essentially the state of disorder of a system since (on a macroscopic level) the natural progression of the world is from order to disorder. (For example, there are more ways to have a messy room than to have an impeccable, neat room). For the change in entropy to be negative just think of it in terms of the room analogy: initially, it was messy, but then it got neater. The state of disorder of things was lessened. Applying this to a chemistry example:CO 2 (g)--> CO 2 (s)An element/compound in a gaseous state always has a greater state of entropy (gaseous molecules are more free to move). However, an element/compound in a solid state has a smaller state of entropy because molecules in a solid are less free to move. Smaller state of entropy - greater state of entropy=negative entropy
Entropy increases when heat is added because the particles do what?
When heat is added, the particles in a system gain energy and move more freely, increasing their randomness and disorder. This leads to an increase in entropy because there are more possible arrangements and microstates for the particles to occupy.
Why is it thermodynamically possible for some ionic solids to dissolve even though the solution process is endothermic?
Even though dissolving some ionic solids is an endothermic process (requires energy input), it is still thermodynamically possible due to the increase in entropy that occurs when the solid breaks apart into individual ions in solution. The increase in entropy favors the dissolution process, even if it requires energy input to overcome the lattice energy holding the solid together.
Explain the second law of thermodynamics and explain why it is not violated by living organisms?
this increase in organization over time in no way violates the second law. The entropy of a particular system, such as an organism, may actually decrease, so long as the total entropy of the universe-the system plus its surroundings-increases. Thus, organisms are islands of low entropy in an increasingly random universe. The evolution of biological order is perfectly consistent with the laws of thermodynamics.
How can an endothermic reaction be spontaneous at room temperature?
An endothermic reaction can be spontaneous at room temperature if the increase in entropy of the system is large enough to overcome the energy input required for the reaction. This can happen if the products of the reaction have higher entropy than the reactants. As a result, the overall change in free energy can be negative even though the reaction is endothermic.
What happens to the entropy of a system as more heat is added beyond the boiling point?
Fundamentally, if the entropy of a system increases, that means that the energy of the system ("normalized" to , i.e., divided by the temperature of the system) has become more "dispersed" or "dilute". For instance, if a system increases its volume at constant energy and temperature, then the energy per unit temperature is now more "dilute", being spread over a larger volume. All spontaneous processes result in a "dilution" or "spreading out" of the energy of the universe. The more dilute the energy of a system is (the higher the entropy of that system) the harder is is to harness that energy to do useful work. Another useful way of thinking about entropy is to consider it as a measure of the amount of information needed to completely specify the state of a system. Ultimately, this means how much information is needed to specify the positions and momenta of every particle in the system.
Is the Roman formations the same as Roman tactics?
No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.No, tactics and formations are not strictly the same even though they are often used interchangeably. A formation was a structure of sorts, such as the square formation or the tortoise formation. A tactic was how the formation was used or moved around or dropped back. A tactic could be likened to a battle plan.
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.
What can you increase by using more cells?
You can increase the current. It depends on how you add them, though: that is, how they are connected to each other.
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.
If water H2O is polar and oxygen O2 non-polar how can there be dissolved oxygen in water?
The simple answer is that most everything happens at least a little bit. The reason why is EQUILIBRIUM. You are correct---water is polar and oxygen is non-polar. The water molecules have great hydrogen bonding and dipole-dipole interactions with each other that the oxygen molecules cannot replace, and so it will take energy or ENTHALPY for oxygen to mix its way into the water. So the process is ENDOTHERMIC and hence unfavorable. However, when you dissolve oxygen in water, you get disorder---something that scientists quantify by talking about a solution's ENTROPY. It is favorable for entropy to increase, and in this case the entropy of the water solution would go up if you were to be able to squeeze some water molecules in there. So entropy and enthalpy are at odds for this reaction. Enthalpy is unfavorable, entropy is favorable. In situations like that systems will reach a state of equilibrium in which the reaction partially occurs. How much will depend on the relative sizes of the entropy and enthalpy changes.
Why a producer would continue to increase output even though the marginal cost?
...of production may be rising? Answer: Because of increase in demand.
Can entropy be zero?
I am not sure whether you refer to delta S (change in entropy) or entropy itself. So I'll answer for both.For S (entropy), which is defined by the function S=kln(omega), where k is Boltzmann's constant and omega is the number of microstates corresponding to a given state, the answer is no. Why? Omega (the number of microstates possible for a certain state) can never be smaller than one. Since Boltzmann's constant is a positive number and ln(omega) will always be greater or equal to zero, entropy will never be negative.However, when calculating delta S (change in entropy in a thermodynamic process), yes entropy can be negative. Remember entropy is essentially the state of disorder of a system since (on a macroscopic level) the natural progression of the world is from order to disorder. (For example, there are more ways to have a messy room than to have an impeccable, neat room). For the change in entropy to be negative just think of it in terms of the room analogy: initially, it was messy, but then it got neater. The state of disorder of things was lessened. Applying this to a chemistry example:CO 2 (g)--> CO 2 (s)An element/compound in a gaseous state always has a greater state of entropy (gaseous molecules are more free to move). However, an element/compound in a solid state has a smaller state of entropy because molecules in a solid are less free to move. Smaller state of entropy - greater state of entropy=negative entropy
