ΔH = ΔU + PΔV
Understand the Problem
The question presents a thermodynamic equation relating enthalpy change (ΔH), internal energy change (ΔU), pressure (P), and volume change (ΔV). It likely seeks to understand how energy transformations occur in a system, particularly how enthalpy is defined in terms of internal energy and work done by the system.
Answer
ΔH = ΔU + PΔV relates enthalpy change to internal energy change and pressure-volume work.
ΔH = ΔU + PΔV is the equation that relates the change in enthalpy (ΔH) to the change in internal energy (ΔU) and the product of pressure (P) and change in volume (ΔV). It is used to calculate enthalpy changes at constant pressure.
Answer for screen readers
ΔH = ΔU + PΔV is the equation that relates the change in enthalpy (ΔH) to the change in internal energy (ΔU) and the product of pressure (P) and change in volume (ΔV). It is used to calculate enthalpy changes at constant pressure.
More Information
This equation is essential in thermodynamics for systems at constant pressure, as it accounts for changes in heat and expansion work done by or on a system. It simplifies calculating energy changes by separating heat from pressure-volume work.
Tips
A common mistake is forgetting that the equation applies under constant pressure conditions. Misinterpreting the terms or mixing units for pressure and volume can lead to errors.
Sources
- 5.3: Enthalpy - Chemistry LibreTexts - chem.libretexts.org
- ΔH = ΔU + PΔV - CHEMISTRY COMMUNITY - lavelle.chem.ucla.edu
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