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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

Consider the reaction: $$\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightarrow 2 \mathrm{NO}_{2}(g)$$ where \(P_{\mathrm{NO}_{2}}=0.29\) atm and $P_{\mathrm{N}_{2} \mathrm{O}_{4}}=1.6 \mathrm{atm} .$ For this reaction at these conditions, \(\Delta G=-1000 \mathrm{J}\) and \(\Delta G^{\circ}=6000 \mathrm{J}\) . Which of the following statements about this reaction is(are) true? a. The reverse reaction is spontaneous at these conditions. b. At equilibrium, \(P_{\mathrm{N}_{2} \mathrm{O}_{4}}\) will be greater than 1.6 \(\mathrm{atm}\) . c. The value of K for this reaction is greater than 1. d. The maximum amount of work this reaction can produce at these conditions is –6000 J. e. The reaction is endothermic.

For the sublimation of iodine at \(25^{\circ} \mathrm{C}\) $$\mathrm{I}_{2}(s) \rightarrow \mathrm{I}_{2}(g)$$ the values of \(\Delta H^{\circ}\) and \(\Delta G^{\circ}\) are, respectively, 62 \(\mathrm{kJ}\) and 19 \(\mathrm{kJ}\) . Estimate the temperature at which iodine sublimes. Assume \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) do not depend on temperature.

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).

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. $\Delta H=-10 . \mathrm{kJ}, \Delta S=-40 . \mathrm{J} / \mathrm{K}, T=200 . \mathrm{K}$

Choose the substance with the larger positional probability in each case. a. 1 mole of \(\mathrm{H}_{2}\) (at \(\mathrm{STP} )\) or 1 mole of $\mathrm{H}_{2}\left(\text { at } 100^{\circ} \mathrm{C}, 0.5 \mathrm{atm}\right)$ b. 1 mole of \(\mathrm{N}_{2}(\text { at } \mathrm{STP})\) or 1 mole of \(\mathrm{N}_{2}(\text { at } 100 \mathrm{K}, 2.0 \mathrm{atm})\) c. 1 mole of \(\mathrm{H}_{2} \mathrm{O}(s)\) (at \(0^{\circ} \mathrm{C} )\) or 1 \(\mathrm{mole}\) of $\mathrm{H}_{2} \mathrm{O}(l)\left(\mathrm{at} 20^{\circ} \mathrm{C}\right)$
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