errata 24303

modules/m68817/index.cnxml

@@ -78,7 +78,7 @@ Consider the system shown in <link target-id="CNX_Chem_16_03_Energy"/>. What is
 <caption>Entropy increases as the temperature of a substance is raised, which corresponds to the greater spread of kinetic energies. When a substance undergoes a phase transition, its entropy changes significantly.</caption>
 </figure>
 <note id="fs-idm189737360" class="chemistry link-to-learning">
-<para id="fs-idm305735232">Try this <link url="http://openstax.org/l/16freemotion">simulator</link> with interactive visualization of the dependence of particle location and freedom of motion on physical state and temperature.</para>
+<para id="fs-idm305735232">Use <link url="http://openstax.org/l/16freemotion">interactive simulator</link> to visualize the dependence of particle location and freedom of motion on physical state and temperature for several different atoms and molecules.</para>
 </note>
 <para id="fs-idm135226880">The entropy of a substance is influenced by the structure of the particles (atoms or molecules) that comprise the substance. With regard to atomic substances, heavier atoms possess greater entropy at a given temperature than lighter atoms, which is a consequence of the relation between a particle’s mass and the spacing of quantized translational energy levels (a topic beyond the scope of this text). For molecules, greater numbers of atoms increase the number of ways in which the molecules can vibrate and thus the number of possible microstates and the entropy of the system.</para><para id="fs-idm96833856">Finally, variations in the types of particles affects the entropy of a system. Compared to a pure substance, in which all particles are identical, the entropy of a mixture of two or more different particle types is greater. This is because of the additional orientations and interactions that are possible in a system comprised of nonidentical components. For example, when a solid dissolves in a liquid, the particles of the solid experience both a greater freedom of motion and additional interactions with the solvent particles. This corresponds to a more uniform dispersal of matter and energy and a greater number of microstates. The process of dissolution therefore involves an increase in entropy, Δ<emphasis effect="italics">S</emphasis> > 0.</para>
 <para id="fs-idm224301776">Considering the various factors that affect entropy allows us to make informed predictions of the sign of Δ<emphasis effect="italics">S</emphasis> for various chemical and physical processes as illustrated in <link target-id="fs-idm151499136"/>.</para>