Why Do Enthalpy and Entropy Changes Often Seem Temperature-Independent?

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The discussion centers on the assumption that enthalpy and entropy changes in reactions can be considered temperature-independent, particularly in early undergraduate chemistry. Participants question whether the enthalpy and entropy of reactants and products remain constant or if they vary with temperature, and if so, whether the rate of change is uniform across all substances. It is noted that this assumption is a simplification that does not hold true in advanced thermodynamics. Some cases may allow for a weighted value due to minimal temperature impact on enthalpy changes. The conversation emphasizes the need for deeper understanding and tools in real thermodynamic applications.
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Why is it that the change in enthalpy and entropy of a reaction often can be assumed not to depend on temperature?
 
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You've been posting long enough to know that you must do your work before anyone can help you. So what are your thoughts on the matter? Are the enthalpy and entropy of reactants and products constant? If they change with temperature, is the rate of change the same for all reactants and products?
 
It is a simplification in early undergrad chemistry. When you get to real thermodynamics, you will see that this is not true, they will give you the tools then that will aid you.

Although in some cases the change in enthalphy is so small according to temperature that you can use a weighted value.
 
But why?
 

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