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Chapter 16: 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: melting of a solid (a), sublimation (b), mixing (d), and boiling (f). These processes result in an increase in randomness or disorder within the system.

Step by step solution

01

a. Melting of a solid

Melting involves a solid turning into a liquid. During this process, the particles in the solid gain kinetic energy, causing them to move more freely. Therefore, the randomness of the system increases. Thus, melting of a solid results in an increase in entropy.
02

b. Sublimation

Sublimation is the process in which a solid transitions directly into a gas, bypassing the liquid state. In this process, the particles in the solid break their bonds and move independently as a gas. The randomness of the system increases during this transition. Thus, sublimation involves an increase in entropy.
03

c. Freezing

Freezing is the process of a liquid becoming a solid. As the liquid particles lose kinetic energy, they become more ordered, forming the rigid structure of a solid. Therefore, the randomness in the system decreases. Thus, freezing does not involve an increase in entropy.
04

d. Mixing

During the mixing process, two or more substances are combined into a mixture. The particles of different substances are distributed randomly, increasing the disorder in the system. Mixing, therefore, involves an increase in entropy.
05

e. Separation

Separation is the process of separating two or more substances from a mixture. This process results in a more ordered system, as the particles of different substances are arranged separately. Therefore, separation does not involve an increase in entropy.
06

f. Boiling

Boiling involves a liquid transitioning into a gas. In this process, the particles in the liquid gain enough kinetic energy to break their bonds and move freely as a gas. The randomness of the system increases during boiling. Thus, boiling involves an increase in entropy. In conclusion, the processes that involve an increase in entropy are: melting of a solid (a), sublimation (b), mixing (d), and boiling (f).

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Most popular questions from this chapter

The value of \(\Delta G^{\circ}\) for the reaction $$2 \mathrm{C}_{4} \mathrm{H}_{10}(g)+13 \mathrm{O}_{2}(g) \longrightarrow 8 \mathrm{CO}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(l)$$ is \(-5490 .\) kJ. Use this value and data from Appendix 4 to calculate the standard free energy of formation for \(\mathrm{C}_{4} \mathrm{H}_{10}(g).\)

List three different ways to calculate the standard free energy change, \(\Delta G^{\circ},\) for a reaction at \(25^{\circ} \mathrm{C} .\) How is \(\Delta G^{\circ}\) estimated at temperatures other than \(25^{\circ} \mathrm{C} ?\) What assumptions are made?

Consider two perfectly insulated vessels. Vessel 1 initially contains an ice cube at \(0^{\circ} \mathrm{C}\) and water at \(0^{\circ} \mathrm{C}\). Vessel 2 initially contains an ice cube at \(0^{\circ} \mathrm{C}\) and a saltwater solution at \(0^{\circ} \mathrm{C}\). Consider the process \(\mathrm{H}_{2} \mathrm{O}(s) \rightarrow \mathrm{H}_{2} \mathrm{O}(l).\) a. Determine the sign of \(\Delta S, \Delta S_{\text {sur, }}\) and \(\Delta S_{\text {univ }}\) for the process in vessel 1. b. Determine the sign of \(\Delta S, \Delta S_{\text {sur, }}\) and \(\Delta S_{\text {univ }}\) for the process in vessel 2. (Hint: Think about the effect that a salt has on the freezing point of a solvent.)

The third law of thermodynamics states that the entropy of a perfect crystal at \(0 \mathrm{K}\) is zero. In Appendix \(4, \mathrm{F}^{-}(a q), \mathrm{OH}^{-}(a q)\) and \(\mathrm{S}^{2-}(a q)\) all have negative standard entropy values. How can \(S^{\circ}\) values be less than zero?

Cells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be written as $$\mathrm{ATP}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{ADP}(a q)+\mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q)$$ where ADP represents adenosine diphosphate. For this reaction, \(\Delta G^{\circ}=-30.5 \mathrm{kJ} / \mathrm{mol}.\) a. Calculate \(K\) at \(25^{\circ} \mathrm{C}\) b. If all the free energy from the metabolism of glucose $$\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)$$ goes into forming ATP from ADP, how many ATP molecules can be produced for every molecule of glucose? $$\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)$$ goes into forming ATP from ADP, how many ATP molecules can be produced for every molecule of glucose?
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