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Ch.6 - Thermochemistry
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.6 - ThermochemistryProblema 107
Capitolo 6, Problema 107

Derive a relationship between ΔH and ΔE for a process in which the temperature of a fixed amount of an ideal gas changes.

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Start with the first law of thermodynamics: \( \Delta E = q + w \), where \( \Delta E \) is the change in internal energy, \( q \) is the heat exchanged, and \( w \) is the work done.
For an ideal gas, the work done by the system during expansion or compression at constant pressure is given by \( w = -P_{\text{ext}} \Delta V \), where \( P_{\text{ext}} \) is the external pressure and \( \Delta V \) is the change in volume.
The enthalpy change \( \Delta H \) is defined as \( \Delta H = \Delta E + P \Delta V \).
Substitute the expression for work into the first law equation: \( \Delta E = q - P_{\text{ext}} \Delta V \).
Combine the expressions for \( \Delta E \) and \( \Delta H \) to derive the relationship: \( \Delta H = q - P_{\text{ext}} \Delta V + P \Delta V = q + (P - P_{\text{ext}}) \Delta V \).

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Enthalpy (ΔH)

Enthalpy (ΔH) is a thermodynamic quantity that represents the total heat content of a system at constant pressure. It accounts for the internal energy of the system plus the product of its pressure and volume. In processes involving gases, changes in enthalpy can be related to heat transfer, making it crucial for understanding energy changes during reactions or phase transitions.
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Internal Energy (ΔE)

Internal Energy (ΔE) is the total energy contained within a system, encompassing kinetic and potential energies of the particles. For an ideal gas, changes in internal energy are primarily due to changes in temperature. The relationship between internal energy and temperature is significant, as it helps in calculating energy changes during heating or cooling processes.
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Ideal Gas Law

The Ideal Gas Law (PV = nRT) describes the behavior of ideal gases, relating pressure (P), volume (V), temperature (T), and the number of moles (n) of gas. This law is essential for deriving relationships between ΔH and ΔE, as it allows for the calculation of changes in state variables when temperature changes, providing a framework for understanding how energy is transferred in gas systems.
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