The enthalpies of fusion and vaporization of F2 are 0.5 and 6.6 kJ mol^-1, and the melting and b

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The enthalpies of fusion and vaporization of F2 are 0.5 and...

The enthalpies of fusion and vaporization of $\mathrm{F}_{2}$ are 0.5 and $6.6 \mathrm{kJ} \mathrm{mol}^{-1},$ and the melting and boiling points are 53 and $85 \mathrm{K}$ respectively. Determine values (per mole of $\mathrm{F}_{2}$ ) of $\Delta_{\text {fus }} S$ and $\Delta_{\text {vap }} S,$ and comment on their relative magnitudes.

Key Concepts

Relative Magnitude of Entropy Changes

The relative magnitudes of the entropy changes reflect the extent of disorder introduced during the phase transitions. Typically, vaporization involves a greater increase in molecular disorder compared to melting; hence, the entropy of vaporization is usually significantly larger than the entropy of fusion. Understanding this relationship helps in comparing the molecular dynamics of substances during different phase transitions.

Phase Transitions

Phase transitions, such as melting (fusion) and boiling (vaporization), involve the transformation of a substance from one physical state to another. During these transitions, the substance absorbs or releases energy without a change in temperature, corresponding to latent heats. This concept is fundamental in understanding how energy input causes changes in the structural order of matter.

Enthalpy Change

Enthalpy change refers to the amount of heat absorbed or released during a phase transition at constant pressure. The enthalpies of fusion and vaporization are the energy required for melting and boiling, respectively. These quantities are essential for quantifying the energetic requirements of changing phases and are typically expressed in kilojoules per mole.

Entropy Change

Entropy change in a phase transition quantifies the increase or decrease in disorder when a substance changes phase. It is calculated using the relation ?S = ?H/T, where ?S is the entropy change, ?H is the enthalpy change, and T is the temperature at which the transition occurs (in Kelvin). This provides insight into the degree of randomness or disorder introduced in the substance as it transitions from one phase to another.

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