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Chapter 18: 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 can occur without any external influence once started, such as a ball rolling down a hill or ice melting at room temperature. A nonspontaneous process is one that requires input of energy and doesn't occur naturally under the set conditions, such as charging a battery or pumping water uphill.

Step by step solution

01

Define Spontaneous Process

A spontaneous process is a process that, once started, can proceed without any further external influence or input. It is a process that has the potential to occur naturally under a certain set of conditions. Examples include a ball rolling down a hill, ice melting at room temperature, etc._
02

Examples of Spontaneous Processes

1. The melting of ice at room temperature: This process is spontaneous because it can occur naturally without any further external influence, given the conditions are right (i.e., the temperature is above the freezing point of water).\n 2. An apple falling from a tree: This is spontaneous because once the apple is detached from the tree, it will fall to the ground under the influence of gravity without any need for additional energy.
03

Define Nonspontaneous Process

A nonspontaneous process is a process that cannot naturally occur without the input of some form of energy. These types of processes are generally not naturally occurring under the set conditions. Examples might include pumping water uphill, the charging of a battery, etc.
04

Examples of Nonspontaneous Processes

1. The charging of a battery: It requires an external source of electricity, and so it is a nonspontaneous process.\n 2. Pumping water uphill: This process requires an external force (usually provided by a pump) to overcome gravity, so it is nonspontaneous.

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Most popular questions from this chapter

State the second law of thermodynamics in words and express it mathematically.

State the third law of thermodynamics and explain its usefulness in calculating entropy values.

How does the entropy of a system change for each of the following processes? (a) A solid melts. (b) A liquid freezes. (c) A liquid boils. (d) A vapor is converted to a solid. (e) A vapor condenses to a liquid. (f) A solid sublimes. (g) Urea dissolves in water.

Use the following data to determine the normal boiling point, in kelvins, of mercury. What assumptions must you make in order to do the calculation? $$ \begin{aligned} \mathrm{Hg}(l): & \Delta H_{\mathrm{f}}^{\circ} &=0 \text { (by definition) } \\\ & S^{\circ} &=77.4 \mathrm{~J} / \mathrm{K} \cdot \mathrm{mol} \\ \mathrm{Hg}(g): & \Delta H_{\mathrm{f}}^{\circ} &=60.78 \mathrm{~kJ} / \mathrm{mol} \\ & S^{\circ} &=174.7 \mathrm{~J} / \mathrm{K} \cdot \mathrm{mol} \end{aligned} $$

The molar heat of vaporization of ethanol is \(39.3 \mathrm{~kJ} / \mathrm{mol}\) and the boiling point of ethanol is \(78.3^{\circ} \mathrm{C}\) Calculate \(\Delta S\) for the vaporization of \(0.50 \mathrm{~mol}\) ethanol.
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