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Ch.18 - Free Energy and Thermodynamics
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.18 - Free Energy and ThermodynamicsProblema 34
Capitolo 18, Problema 34

Calculate the change in entropy that occurs in the system when 55.0 g of water vaporizes from a liquid to a gas at its boiling point (100.0 °C). See Table 11.7 for heats of vaporization.

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Determine the number of moles of water: Use the molar mass of water (18.02 g/mol) to convert the mass of water (55.0 g) into moles.
Identify the heat of vaporization: Look up the heat of vaporization for water at its boiling point, which is typically given in kJ/mol.
Calculate the total heat absorbed: Multiply the number of moles of water by the heat of vaporization to find the total heat absorbed during the phase change.
Convert the heat absorbed to the same units as entropy: Since entropy is often expressed in J/K, convert the total heat absorbed from kJ to J.
Calculate the change in entropy: Use the formula \( \Delta S = \frac{q_{rev}}{T} \), where \( q_{rev} \) is the heat absorbed (in J) and \( T \) is the temperature in Kelvin (373 K for water at boiling point).

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Entropy

Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it quantifies the amount of energy in a physical system that is not available to do work. When a substance changes state, such as from liquid to gas, the entropy typically increases because gas molecules have more freedom of movement and occupy a larger volume than liquid molecules.
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Entropy in Thermodynamics

Heat of Vaporization

The heat of vaporization is the amount of energy required to convert a unit mass of a substance from liquid to gas at its boiling point without changing its temperature. This value is crucial for calculating the change in entropy during phase transitions, as it directly relates to the energy input needed for vaporization, which influences the disorder of the system.
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Heat Capacity

Phase Change and Temperature

Phase changes, such as vaporization, occur at specific temperatures where the substance can transition between states. For water, the boiling point is 100.0 °C at standard atmospheric pressure. Understanding the relationship between temperature and phase changes is essential for calculating thermodynamic properties like entropy, as these transitions involve significant energy changes while maintaining constant temperature.
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Entropy in Phase Changes
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