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Chapter 17: Problem 32

Which of the following involve an increase in the entropy of the system? a. melting of a solid b. sublimation c. freezing d. mixing e. separation f. boiling

Short Answer

Expert verified
The processes that involve an increase in entropy are: a. Melting of a solid, as molecules become more disordered. b. Sublimation, as the substance transitions from solid to gas, increasing disorder. d. Mixing, as molecules become more dispersed and disordered. f. Boiling, as the substance changes from liquid to gas, increasing disorder.

Step by step solution

01

Option a: Melting of a solid

Melting is the process of a solid turning into a liquid. As the substance changes from a solid to a liquid, its molecules become more disordered, and the entropy increases. So, there is an increase in the entropy of the system.
02

Option b: Sublimation

Sublimation is the direct transformation of a substance from the solid phase to the gas phase, bypassing the liquid phase. In this process, the molecules become even more disordered compared to the solid state. Therefore, sublimation involves an increase in entropy.
03

Option c: Freezing

Freezing is the process of a liquid turning into a solid. The substance becomes more ordered as the molecules become more tightly packed in the solid state compared to the liquid state. Thus, freezing decreases entropy; there is no increase in the entropy of the system.
04

Option d: Mixing

When two substances mix together, their molecules become more dispersed and disordered. The overall entropy of the system increases due to this increase in disorder. Therefore, mixing involves an increase in entropy.
05

Option e: Separation

Separation is the process of taking a mixture apart and separating it into its component parts. This process increases the order in the system as the components are no longer mixed. As a result, separation leads to a decrease in entropy, not an increase.
06

Option f: Boiling

Boiling is the process of a liquid turning into a gas. As the substance changes from a liquid to a gas, its molecules become much more disordered and dispersed. This results in an increase in entropy. To summarize, the processes that involve an increase in entropy are: a. Melting of a solid b. Sublimation d. Mixing f. Boiling

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Most popular questions from this chapter

Given the values of \(\Delta H\) and \(\Delta S\), which of the following changes will be spontaneous at constant \(T\) and \(P\) ? a. \(\Delta H=+25 \mathrm{~kJ}, \Delta S=+5.0 \mathrm{~J} / \mathrm{K}, T=300 . \mathrm{K}\) b. \(\Delta H=+25 \mathrm{~kJ}, \Delta S=+100 . \mathrm{J} / \mathrm{K}, T=300 . \mathrm{K}\) c. \(\Delta H=-10 . \mathrm{kJ}, \Delta S=+5.0 \mathrm{~J} / \mathrm{K}, T=298 \mathrm{~K}\) d. \(\Delta H=-10 . \mathrm{kJ}, \Delta S=-40 . \mathrm{J} / \mathrm{K}, T=200 . \mathrm{K}\)

The Ostwald process for the commercial production of nitric acid involves three steps: $$ \begin{array}{l} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \underset{825^{\circ} \mathrm{C}}{\longrightarrow} 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \\\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \\ 3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(l)+\mathrm{NO}(g) \end{array} $$ a. Calculate \(\Delta H^{\circ}, \Delta S^{\circ}, \Delta G^{\circ}\), and \(K\) (at \(\left.298 \mathrm{~K}\right)\) for each of the three steps in the Ostwald process (see Appendix 4). b. Calculate the equilibrium constant for the first step at \(825^{\circ} \mathrm{C}\), assuming \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) do not depend on temperature. c. Is there a thermodynamic reason for the high temperature in the first step, assuming standard conditions?

You have a \(1.00\) - \(L\) sample of hot water \(\left(90.0^{\circ} \mathrm{C}\right)\) sitting open in a \(25.0^{\circ} \mathrm{C}\) room. Eventually the water cools to \(25.0^{\circ} \mathrm{C}\) while the temperature of the room remains unchanged. Calculate \(\Delta S_{\text {surr }}\) for this process. Assume the density of water is \(1.00 \mathrm{~g} / \mathrm{cm}^{3}\) over this temperature range, and the heat capacity of water is constant over this temperature range and equal to \(75.4 \mathrm{~J} / \mathrm{K} \cdot \mathrm{mol}\).

Consider the following energy levels, each capable of holding two particles: $$ \begin{array}{l} E=2 \mathrm{~kJ}\\\ \boldsymbol{E} \quad E=1 \mathrm{~kJ}\\\ E=0 \quad \quad X X \end{array} $$ Draw all the possible arrangements of the two identical particles (represented by \(X\) ) in the three energy levels. What total energy is most likely, that is, occurs the greatest number of times? Assume that the particles are indistinguishable from each other.

Hydrogen cyanide is produced industrially by the following exothermic reaction: Is the high temperature needed for thermodynamic or kinetic reasons?
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