The boiling point of a substance is defined as the temperature at which liquid and vapor coexist in equilibrium. Use the heat of vaporization ΔHvap = 30.91 kJ/mol and the entropy of vaporization ΔSvap = 93.2 J/K·mol to calculate the boiling point (°C) of liquid bromine.

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

검증된 단계별 안내

Step 1: Understand the relationship between the boiling point, heat of vaporization (ΔHvap), and entropy of vaporization (ΔSvap). At the boiling point, the Gibbs free energy change (ΔG) for the phase transition is zero.

Step 2: Use the Gibbs free energy equation for phase transitions: ΔG = ΔHvap - TΔSvap. Set ΔG to zero because at the boiling point, the liquid and vapor are in equilibrium.

Step 3: Rearrange the equation to solve for the temperature (T): T = ΔHvap / ΔSvap.

Step 4: Convert the units of ΔHvap from kJ/mol to J/mol to match the units of ΔSvap. (1 kJ = 1000 J)

Step 5: Substitute the values of ΔHvap and ΔSvap into the equation to calculate the temperature in Kelvin, then convert the temperature from Kelvin to Celsius by subtracting 273.15.

주요 개념

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Boiling Point

The boiling point of a substance is the temperature at which its liquid phase transitions to the vapor phase, occurring when the vapor pressure equals the external pressure. At this point, the liquid and vapor coexist in equilibrium, meaning that the rate of evaporation equals the rate of condensation. Understanding this concept is crucial for calculating boiling points using thermodynamic properties.

Heat of Vaporization (ΔHvap)

The heat of vaporization (ΔHvap) is the amount of energy required to convert one mole of a liquid into vapor at constant temperature and pressure. It is a critical factor in determining the boiling point, as higher ΔHvap values typically indicate stronger intermolecular forces, leading to higher boiling points. In this context, ΔHvap is given as 30.91 kJ/mol for bromine.

Entropy of Vaporization (ΔSvap)

The entropy of vaporization (ΔSvap) measures the change in disorder when a liquid transitions to a vapor. It is expressed in J/K·mol and reflects how much the molecular arrangement becomes more disordered during vaporization. This concept is essential for calculating the boiling point using the Gibbs free energy equation, which relates ΔHvap and ΔSvap to temperature.