Predict the sign of ΔS sys for each of the following processes: (a) Molten gold solidifies. (b)

step 1 Here's the program 42 in Chapter 19, and in this question, we're going to find the sign of Delta

Predict the sign of ΔS sys for each of the following...

Predict the sign of $\Delta S_{\text { sys }}$ for each of the following processes: (a) Molten gold solidifies. (b) Gaseous $C l_{2}$ dissociates in the stratosphere to form gaseous Cl atoms. (c) Gaseous CO reacts with gaseous $\mathrm{H}_{2}$ to form liquid methanol, $\mathrm{CH}_{3} \mathrm{OH} .(\mathbf{d})$ Calcium phosphate precipitates upon mixing $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)$ and $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(a q)$

Predict the sign of $\Delta S_{\text { sys }}$ for each of the following processes:
(a) Molten gold solidifies. (b) Gaseous $C l_{2}$ dissociates in the stratosphere to form gaseous Cl atoms. (c) Gaseous CO reacts with gaseous $\mathrm{H}_{2}$ to form liquid methanol, $\mathrm{CH}_{3} \mathrm{OH} .(\mathbf{d})$ Calcium phosphate precipitates upon mixing
$\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)$ and $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(a q)$

Key Concepts

Entropy

Entropy is a measure of the disorder or randomness of a system. It quantifies the number of microscopic configurations that correspond to a thermodynamic system’s macroscopic state. In general, processes that lead to a greater number of accessible microstates, such as those increasing the number of particles or transitioning from an ordered to a less ordered phase, result in an increase in entropy, while processes that decrease the number of configurations lead to a decrease in entropy.

Phase Changes

Phase transitions, such as melting, solidification, condensation, and vaporization, are key processes that involve changes in entropy. Typically, moving from a more ordered phase (like a solid) to a less ordered phase (like a liquid or gas) increases entropy, whereas the reverse transition decreases entropy. The physical state of matter plays a crucial role in the evaluation of entropy changes in any process.

Molecular Dissociation

Molecular dissociation refers to the breaking apart of molecules into smaller entities such as atoms or radicals. This process generally increases entropy because it increases the number of particles in the system and therefore the number of possible microstates. The increased freedom of movement and interactions of the individual particles contributes to a higher level of disorder.

Chemical Precipitation

Chemical precipitation involves the formation of a solid from a solution, typically when dissolved ions combine to form an insoluble compound. This process often results in a decrease in entropy because the ions, which were once randomly dispersed in solution, become locked into a well-ordered solid lattice, reducing the overall randomness or disorder of the system.

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