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On the outline when it says "explain how how ∆S is related to ∆H for a change at constant temperature and pressure and explain the relationship" I am a little confused. Like I know the general equation to relate the two, but is there a trend that when you increase ∆S, ∆H will either increase or decrease? Or does it depend on what Gibbs free energy is.
I believe it is all dependent on gibbs free energy because we need delta s and delta h to know if the reaction will be spontaneous or not. I would just make sure you know how to manipulate the variables and come to the conclusion of what needs to happen for the reaction to be spontaneous or non spontaneous. From a hw question we had (4.37), we can come to the conclusion about spontaneity can be found from S or G, if g is negative the reaction is spontaneous. If delta s total is positive it would also be spontaneous.
The relationship between delta H and delta S depends on which delta S you're referring to. If it's the entropy of the system, then as delta H increases, then delta S increases with it. If it's the entropy of the surroundings, then delta S would decrease with an increase in delta H. If its the total entropy, then delta S increases with a decrease in delta S.
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