How to determine enthelpy of formation

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Enthalpy of formation values, such as those for MgO, Fe2O3, and NO, are crucial for understanding energy changes in chemical reactions. These values can be experimentally determined, often through calorimetry or using the van't Hoff equation, which relates temperature changes in electrolytic cells to enthalpy changes. While it is possible to estimate enthalpy of formation using bond formation energies, this method tends to be imprecise, with typical errors ranging from tens of percent to potentially an order of magnitude. For those seeking reference materials, several free resources are available online to aid in understanding and calculating these values.
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Background:
I've seen many different values for enthalpy of formation on Wikipedia, such as the following: MgO: -602 kJ·mol−1, Fe2O3: -826 kJ·mol−1, NO: 90.29 kJ·mol−1.

I'm curious about these values, but I have no idea how they were determined and I've only taken an introductory course in chemistry. However, my understanding is that these values can be used to determine (or at least estimate) how much energy will be released (or consumed) by a chemical process which converts one set of compounds into another.

Question:
Is it possible to calculate the enthalpy of formation for a given compound, or is it only possible to determine that based on an experiment? If so, are there any good, free reference materials for that kind of information?
 
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You can try to estimate them using bond formation energies, but the result is never very precise.
 
Okay. How do I estimate using bond formation energy? Also, how imprecise are you talking about? ±50%? An order of magnitude? More?
 
Some enthalpies can be obtained by measuring heat in a calorimeter. A very precise way to determine enthalpies is via the van't Hoff equation e.g. from the change of electric potentials of electrolytic cells with temperature.
 

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