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Chapter 17: Problem 1

Explain what is meant by a spontaneous process. Give two examples each of spontaneous and nonspontaneous processes.

Short Answer

Expert verified
A spontaneous process is one that occurs naturally without external influence and tends towards equilibrium, such as the melting of ice at room temperature or a gas spreading out in a container. A nonspontaneous process requires continuous external influence to proceed, like charging a battery or compressing a gas into a smaller volume.

Step by step solution

01

Definition of a Spontaneous Process

A spontaneous process is a natural occurrence that, once started, proceeds on its own without any external intervention. It will continue to take place under a specific set of conditions till it reaches equilibrium - say, the system state of lowest potential energy. However, the rate at which the process happens can be fast or slow.
02

Examples of Spontaneous Processes

Now let's provide two examples of spontaneous processes: 1. The melting of ice at room temperature: This process is spontaneous because ice naturally transforms to water at temperatures above its freezing point, without any external influence. This happens until all ice has melted, and the system reaches an equilibrium. 2. A gas spreading out in a container: After the lid from the container is removed, the gas molecules naturally spread out or disperse to fill the entire container due to their kinetic energy, without the need for external force.
03

Definition of Nonspontaneous Processes

A nonspontaneous process, in contrast, does not happen naturally under a given set of conditions and requires constant external influence to proceed.
04

Examples of Nonspontaneous Processes

Now let's provide two examples of nonspontaneous processes: 1. Charging a battery: This process is nonspontaneous because it requires a source of electrical energy to proceed. Without this external supply, the battery does not charge on its own. 2. Compressing a gas into a smaller volume: Naturally, gases tend to spread out to fill the entire space available to them. So compressing them into a smaller volume requires continuous external pressure.

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Most popular questions from this chapter

Consider the reaction \(\mathrm{A} \longrightarrow \mathrm{B}+\mathrm{C}\) at \(298 \mathrm{~K}\). Given that the forward rate constant \(\left(k_{f}\right)\) is \(0.46 \mathrm{~s}^{-1}\) and the reverse rate constant \(\left(k_{r}\right)\) is \(1.5 \times 10^{-2} / M \cdot \mathrm{s},\) calculate \(\Delta G^{\circ}\) of the reaction.

Consider the following facts: Water freezes spontaneously at \(-5^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm},\) and ice has a more ordered structure than liquid water. Explain how a spontaneous process can lead to a decrease in entropy.

Consider the following reaction at \(25^{\circ} \mathrm{C}\) : $$ \mathrm{Fe}(\mathrm{OH})_{2}(s) \rightleftharpoons \mathrm{Fe}^{2+}(a q)+2 \mathrm{OH}^{-}(a q) $$ Calculate \(\Delta G^{\circ}\) for the reaction. \(K_{\mathrm{sp}}\) for \(\mathrm{Fe}(\mathrm{OH})_{2}\) is \(1.6 \times 10^{-14}\)

For each pair of substances listed here, choose the one having the larger standard entropy value at \(25^{\circ} \mathrm{C}\). The same molar amount is used in the comparison. Explain the basis for your choice. (a) \(\mathrm{Li}(s)\) or \(\mathrm{Li}(l)\) (b) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)\) or \(\mathrm{CH}_{3} \mathrm{OCH}_{3}(l)\) (Hint: Which molecule can hydrogen-bond?); (c) \(\operatorname{Ar}(g)\) or \(\operatorname{Xe}(g) ;\) (d) \(\operatorname{CO}(g)\) or \(\mathrm{CO}_{2}(g)\) (e) \(\mathrm{O}_{2}(g)\) or \(\mathrm{O}_{3}(g) ;(\mathrm{f}) \mathrm{NO}_{2}(g)\) or \(\mathrm{N}_{2} \mathrm{O}_{4}(g)\)

Calculate \(\Delta G^{\circ}\) for the following reactions at \(25^{\circ} \mathrm{C}\) : (a) \(2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s)\) (b) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)\) (c) \(2 \mathrm{C}_{2} \mathrm{H}_{6}(g)+7 \mathrm{O}_{2}(g) \longrightarrow\) $$ 4 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) $$ See Appendix 2 for thermodynamic data.
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