S = 0
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Re: S = 0
Entropy total is equal to 0 when there is a reversible reaction since the reaction is 'at equilibrium' throughout the whole time. Entropy of the surroundings is equal to 0 with an expansion against a vaccum.
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Re: S = 0
When your system is isothermal and your reaction is reversible, s = 0 because the reaction is considered at equilibrium throughout.
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Re: S = 0
Entropy can also equal zero at absolute zero when the molecules only have one orientable state (no residual entropy).
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Re: S = 0
Entropy is considered 0 in an isothermal reversible expansion reaction because entropy is a state function and ends in the same final state that it initially starts in.
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Re: S = 0
S just means entropy, rather than change in entropy that should be denoted as ΔS. Entropy is almost never 0 (the entropies of all perfect crystals approach zero as the absolute temperature approaches zero; "perfect crystal" refers to a substance in which all the atoms are in a perfectly orderly array.), because even at absolute 0 where all molecular motion has ceased, positional (residual) entropy, present because of different microstates, still exists.
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Re: S = 0
S, or entropy, is zero in an isothermal reversible system since it it always at equilibrium.
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Re: S = 0
An example would be a perfect crystal like diamond at absolute zero. However absolute zero is impossible to reach at the moment and can only be reached theoretically.
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Re: S = 0
Shutong Hou_1F wrote:S just means entropy, rather than change in entropy that should be denoted as ΔS. Entropy is almost never 0 (the entropies of all perfect crystals approach zero as the absolute temperature approaches zero; "perfect crystal" refers to a substance in which all the atoms are in a perfectly orderly array.), because even at absolute 0 where all molecular motion has ceased, positional (residual) entropy, present because of different microstates, still exists.
What would be the meaning/differences of positive/negative entropies?
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Re: S = 0
In an isothermal reaction, the change in surrounding entropy is zero because energy is not transferred to the surroundings. In a reversible reaction, the total entropy change is equal to zero because the system is in equilibrium.
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Re: S = 0
Ivan Tadeja 1G wrote:Shutong Hou_1F wrote:S just means entropy, rather than change in entropy that should be denoted as ΔS. Entropy is almost never 0 (the entropies of all perfect crystals approach zero as the absolute temperature approaches zero; "perfect crystal" refers to a substance in which all the atoms are in a perfectly orderly array.), because even at absolute 0 where all molecular motion has ceased, positional (residual) entropy, present because of different microstates, still exists.
What would be the meaning/differences of positive/negative entropies?
Entropy > 0 means the reaction is favoring an increase in disorder and entropy < 0 means it's favoring order (or less disorder).
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Re: S = 0
Having zero entropy is theoretical. The substance must be in a perfect crystal structure at absolute zero. This would eliminate any positional entropy as well as any entropy from movement.
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Re: S = 0
Mariah wrote:rabiasumar2E wrote:It's zero in an isothermal reversible reaction.
Can you explain how we know whether or not it is isothermal?
The problem usually say whether or not a reaction is isothermal
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Re: S = 0
Having S=0 will never occur in reality. Theoretically it would occur in an object/system that it is at absolute 0, and is in a perfect crystal. This would mean that it would have no residual entropy.
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Re: S = 0
I believe entropy=0 when there is only 1 structural configuration. For example, O2 gas only has 1 structural configuration and therefor has an entropy of 0.
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