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Chapter 17: Problem 36

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 the entropy of the system are: melting of a solid (a), sublimation (b), mixing (d), and boiling (f). These processes increase the randomness or disorder of the system.

Step by step solution

01

a. Melting of a solid

During the melting of a solid, the solid changes to a liquid state. In the liquid state, the particles have more freedom to move around when compared to a solid state. This leads to an increase in the disorder or randomness of the system. Therefore, melting of a solid involves an increase in the entropy of the system.
02

b. Sublimation

Sublimation is the process in which a solid changes directly to a gas without passing through the liquid state. In the gaseous state, particles have even more freedom to move around compared to a solid state. This causes the system to become more disordered and random. Thus, sublimation involves an increase in the entropy of the system.
03

c. Freezing

In the freezing process, a liquid changes to a solid state. This leads to particles having less freedom to move around compared to the liquid state. The system becomes more ordered, which means the entropy of the system decreases. Therefore, freezing does not involve an increase in the entropy of the system.
04

d. Mixing

When two substances are mixed, the particles of both substances are spread out and intermingle randomly, leading to a more disordered and random system. Consequently, mixing involves an increase in the entropy of the system.
05

e. Separation

In separation, particles are sorted and isolated from each other, leading to a more ordered and less random system. As a result, separation does not involve an increase in the entropy of the system but rather a decrease in entropy.
06

f. Boiling

Boiling is the process in which a liquid changes to a gaseous state. In the gaseous state, particles have more freedom to move around compared to the liquid state, which results in an increase in the disorder or randomness of the system. Therefore, boiling involves an increase in the entropy of the system. To summarize, the processes that involve an increase in the entropy of the system are: - Melting of a solid (a) - Sublimation (b) - Mixing (d) - Boiling (f)

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Most popular questions from this chapter

Some nonelectrolyte solute (molar mass \(=142 \mathrm{g} / \mathrm{mol} )\) was dissolved in \(150 . \mathrm{mL}\) of a solvent (density \(=0.879 \mathrm{g} / \mathrm{cm}^{3} )\) The elevated boiling point of the solution was 355.4 \(\mathrm{K}\) . What mass of solute was dissolved in the solvent? For the solvent, the enthalpy of vaporization is 33.90 \(\mathrm{kJ} / \mathrm{mol}\) , the entropy of vaporization is 95.95 \(\mathrm{J} / \mathrm{K} \cdot\) mol, and the boiling- point elevation constant is 2.5 \(\mathrm{K} \cdot \mathrm{kg} / \mathrm{mol}\) .

Consider the dissociation of a weak acid \(\mathrm{HA}\left(K_{\mathrm{a}}=4.5 \times 10^{-3}\right)\) in water: $$\mathrm{HA}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{A}^{-}(a q)$$ Calculate \(\Delta G^{\circ}\) for this reaction at \(25^{\circ} \mathrm{C}\)

The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 \(\mathrm{K}\) to 350.0 \(\mathrm{K}\) . Calculate the standard change in enthalpy \(\left(\Delta H^{\circ}\right)\) for this reaction (assuming \(\Delta H^{\circ}\) is temperature-independent).

Acrylonitrile is the starting material used in the manufacture of acrylic fibers (U.S. annual production capacity is more than two million pounds). Three industrial processes for the production of acrylonitrile are given below. Using data from Appendix 4, calculate \(\Delta S^{\circ}, \Delta H^{p},\) and \(\Delta G^{\circ}\) for each process. For part a, assume that \(T=25^{\circ} \mathrm{C} ;\) for part \(\mathrm{b}, T=70 .^{\circ} \mathrm{C} ;\) and for part \(\mathrm{c}, T=700 .^{\circ} \mathrm{C}\) Assume that \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) do not depend on temperature.

Predict the sign of \(\Delta S\) for each of the following and explain. a. the evaporation of alcohol b. the freezing of water c. compressing an ideal gas at constant temperature d. dissolving NaCl in water
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