Why should we consider enthalpy more important than internal energy when it comes to a chemical reaction?

<p dir="ltr">We consider the enthalpy change (delta H) more important than the internal energy (delta U) for practical reasons. When we go by the definitions alone, internal energy is the heat absorbed or released at a constant volume. This only happens in a sealed container. But in real life experiments held at laboratories, we have open vessels like test tubes, and there, only atmospheric pressure as a state variable remains constant, and not volume per se. This condition of constant pressure becomes more useful to calculate enthalpy in the chemical reaction.&nbsp;</p>

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