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Chapter 4: Problem 140

Which of the following process/es proceed towards more disordered state? a. sublimation of dry ice b. crystallization of salt from solution c. dissolution of sugar in water d. stretching of the rubber

Short Answer

Expert verified
Processes a (sublimation) and c (dissolution) increase disorder.

Step by step solution

01

Analyze Sublimation of Dry Ice

When dry ice (solid carbon dioxide) sublimates, it changes directly from a solid to a gas. In a solid, the molecules are in an ordered structure. In the gaseous state, molecules move freely and are more disordered. Thus, sublimation increases disorder.
02

Analyze Crystallization of Salt

Crystallization involves dissolved ions coming together to form a regular, repeating crystal lattice. This transition from a disordered state (in solution) to an ordered solid decreases disorder.
03

Analyze Dissolution of Sugar

When sugar dissolves in water, its molecules disperse uniformly throughout the solution from an initially ordered solid state. This dispersion increases disorder.
04

Analyze Stretching Rubber

Stretching rubber involves aligning polymer chains from a more disordered to a somewhat ordered arrangement, thereby decreasing disorder.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sublimation Process
Sublimation is a fascinating phase transition where a substance goes directly from a solid to a gas. This process fundamentally involves an increase in entropy, which is a measure of disorder. In the solid state, molecules are tightly packed in a structured arrangement. As sublimation occurs, these molecules gain energy, break free from their fixed positions, and scatter into the air as gas. This change from an ordered state to a more chaotic state significantly increases molecular disorder. For example, when dry ice (solid carbon dioxide) sublimates, the transition results in a higher entropy state due to increased freedom of movement for the gas molecules.
Dissolution Processes
Dissolution is the process where a solute, like sugar, dissolves in a solvent, like water. When sugar crystals are added to water, the structured lattice of sugar molecules begins to disperse. The individual sugar molecules spread out and intermingle with water molecules, moving from a more ordered solid form to a disordered liquid form. This transition results in a net increase in molecular disorder or entropy. It's fascinating to note that even though the sugar molecules distribute uniformly throughout the water, the overall randomness of their arrangement increases.
Crystallization Concepts
Crystallization is the process by which a solid forms from a liquid or solution form, leading to a decrease in disorder. When a solution is supersaturated, ions or molecules come together to form a crystal lattice, which is a highly structured and orderly arrangement. During crystallization, the initially disordered molecules or ions in the solution lose their freedom of motion as they become part of a solid structure. Hence, the entropy decreases because the molecules transition from a more random state to one that is highly ordered. This process starkly contrasts with dissolution, where disorder tends to increase.
Molecular Disorder
Molecular disorder refers to the randomness or chaos in the arrangement of particles within a system. High disorder means atoms or molecules are not in a fixed, predictable arrangement, which is typical in gases and solutions. On the other hand, in solids, like crystals, particles are arranged in a fixed and repeating pattern resulting in low disorder. The concept of molecular disorder is central to understanding entropy in thermodynamics, which describes how energy disperses and spreads out in a system. Processes like sublimation and dissolution both enhance molecular disorder and thus increase the system's entropy.

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Most popular questions from this chapter

Which of the following statement is/are correct? a. From the following reaction $$ \mathrm{CO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}), \Delta \mathrm{H}=\mathrm{q}_{1} $$ Heat of formation of \(\mathrm{CO}_{2}(\mathrm{~g})\) is \(\mathrm{q}_{1}\) b. From the following reaction $$ \mathrm{C} \text { (graphite) }+1 / 2 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}(\mathrm{g}), \Delta \mathrm{H}=\mathrm{q}_{2} $$ Heat of combustion of carbon is \(\mathrm{q}_{2}\). c. From the above reaction, heat of combustion of \(\mathrm{CO}(\mathrm{g})\) is \(\mathrm{q}_{1}\) and that of carbon is \(\mathrm{q}_{1}+\mathrm{q}_{2}\). d. From the above reaction, heat of formation of \(\mathrm{CO}_{2}\) is \(\mathrm{q}_{1}+\mathrm{q}_{2}\)

Which of the following reaction is exothermic? a. \(\mathrm{C}\) (diamond) \(\rightarrow \mathrm{C}\) (graphite) b. \(\mathrm{C}_{2} \mathrm{H}_{6} \rightarrow \mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2}\) c. \(\mathrm{C}_{2} \mathrm{H}_{6}+7 / 2 \mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2}+3 \mathrm{H}_{2} \mathrm{O}\) (I) d. \(2 \mathrm{NaOH}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow\) $$ \mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O} \text { (l) } $$

The signs of \(\Delta \mathrm{G}, \Delta \mathrm{H}\) and \(\Delta \mathrm{S}\) at \(25^{\circ} \mathrm{C}\) are shown below for three reactions. Reaction \(\Delta \mathrm{G}\) \(\Delta \mathrm{H} \quad \Delta \mathrm{S}\) I. \(+\quad+\) II. \(+\) III. - - - Which reaction could go in the reverse direction at high temperature? a. II only b. III only c. I and II d. II and III

The value of \(\log _{10} \mathrm{k}_{\mathrm{eq}}\) (equilibrium constant) can be given as a. \(\frac{\Delta \mathrm{G}^{\circ}}{\mathrm{RT}}\) b. \(\frac{\mathrm{T} \Delta \mathrm{S}^{\circ}-\Delta \mathrm{H}^{\circ}}{2.303 \mathrm{RT}}\) c. \(\frac{\Delta \mathrm{H}^{\circ}-\mathrm{T} \Delta \mathrm{S}^{\circ}}{2.303 \mathrm{RT}}\) d. \(\frac{2.303 \mathrm{RT}}{\mathrm{T} \Delta \mathrm{S}^{\mathrm{o}}-\Delta \mathrm{H}^{\circ}}\)

Match the following: List I List II A. \(\Delta \mathrm{S}\) gas for isothermal of an ideal (p) \(\mathrm{nR} \ln \left(\frac{\mathrm{P}_{1}}{\mathrm{P}_{2}}\right)\) gas B. Work done in reversible isothermal (q) \(-\mathrm{nFE}\) ideal gas expansion C. \(\Delta \mathrm{G}\) for reversible isothermal expan- (r) \(\mathrm{nRT} \ln \left(\frac{\mathrm{P}_{2}}{\mathrm{P}_{1}}\right)\) sion of an ideal gas D. \(\left(\Delta \mathrm{G}_{\text {system }}\right) \mathrm{T}, \mathrm{P}\) (s) \(\mathrm{nR} \ln \left(\frac{\mathrm{V}_{2}}{\mathrm{~V}_{\mathrm{1}}}\right)\)
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