Open the to answer the following questions:(a) Select the Solid, Liquid, Gas tab. Explore by selecting different substances, heating and cooling the systems, and changing the state.
What similarities do you notice between the four substances for each phase (solid, liquid, gas)? What differences do you notice?(b) For each substance, select each of the states and record the given temperatures. How do the given temperatures for each state correlate with the strengths of their intermolecular attractions?
Explain.(c) Select the Interaction Potential tab, and use the default neon atoms. Move the Ne atom on the right and observe how the potential energy changes. Select the Total Force button, and move the Ne atom as before. When is the total force on each atom attractive and large enough to matter? Then select the Component Forces button, and move the Ne atom. When do the attractive (van der Waals) and repulsive (electron overlap) forces balance? How does this relate to the potential energy versus the distance between atoms graph?
Elemental carbon has one gas phase, one liquid phase, and two different solid phases, as shown in the phase diagram:(a) On the phase diagram, label the gas and liquid regions.(b) Graphite is the most stable phase of carbon at normal conditions. On the phase diagram, label the graphite phase.(c) If graphite at normal conditions is heated to 2500 K while the pressure is increased to 10 10 Pa, it is converted into diamond. Label the diamond phase.(d) Circle each triple point on the phase diagram.(e) In what phase does carbon exist at 5000 K and 10 8 Pa?(f) If the temperature of a sample of carbon increases from 3000 K to 5000 K at a constant pressure of 10 6 Pa, which phase transition occurs, if any? 10.5 The Solid State of Matter.
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