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why do we use the entalphy of formation of water at standard conditions to calculate the entalphy of a reaction even if water is not gas at 1bar and 298K
Entalphy of Formation: Why Use Water at Std Cond?
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SUMMARY
The enthalpy of formation of water is utilized at standard conditions (1 bar and 298K) to calculate reaction enthalpy, despite water's gaseous state at room temperature and pressure. This is due to the distinction between formation enthalpy and condensation enthalpy, where the latter accounts for thermal energy released during phase changes. The difference in heat release between combustion reactions with and without water condensation is quantified by the Higher Heating Value (HHV) and Lower Heating Value (LHV). Understanding these concepts is crucial for accurate thermodynamic calculations in chemical reactions.
PREREQUISITES- Understanding of enthalpy concepts, specifically enthalpy of formation and condensation.
- Familiarity with thermodynamic principles, including heat transfer and phase changes.
- Knowledge of Higher Heating Value (HHV) and Lower Heating Value (LHV) in combustion analysis.
- Basic grasp of standard temperature and pressure (STP) conditions in thermodynamics.
- Research the differences between Higher Heating Value (HHV) and Lower Heating Value (LHV) in combustion processes.
- Study the concept of latent heat, particularly the latent heat of condensation.
- Explore the enthalpy of formation tables for various substances, focusing on water in both liquid and vapor states.
- Learn about the implications of phase changes on thermodynamic calculations in chemical reactions.
Chemists, chemical engineers, and students studying thermodynamics who require a deeper understanding of enthalpy calculations and phase changes in reactions.
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