calculating entropy
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calculating entropy
why is the change in entropy sometimes equal to (-deltaH/T)? in other words, what does the - imply?
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Re: calculating entropy
the negative sign doesnt play much of a role until you get the final Delta S value. If the final calculated delta S is larger than 0, you have a spontaneous rxn while a delta S thats less than 0 is a non spontaneouos process.
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Re: calculating entropy
McKenna_4A wrote:why is the change in entropy sometimes equal to (-deltaH/T)? in other words, what does the - imply?
The change in entropy of the surroundings is equal to the negative change in the enthalpy of the system divided by temperature. This makes sense because when the system gives off heat (negative delta H), the surroundings gain heat and therefore entropy increases (positive delta S).
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Re: calculating entropy
It represents the heat released by the system, or heat lost by the system. Therefore, it's not always -, depends on the pathway of heat transfer that determines the sign of q.
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