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Chapter 10: Q10.3-41 E (page 587)
Use the information to estimate the boiling point of water in Denver when the atmospheric pressure is \(83.3\)kPa
The boiling point of water in Denver is\({\rm{9}}{{\rm{5}}^{\rm{^\circ }}}{\rm{C}}\).
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Dry ice, \({\rm{C}}{{\rm{O}}_{\rm{2}}}{\rm{(s)}}\), does not melt at atmospheric pressure. It sublimes at a temperature of \({\rm{ - 7}}{{\rm{8}}^{\rm{o}}}{\rm{C}}\). What is the lowest pressure at which \({\rm{C}}{{\rm{O}}_{\rm{2}}}{\rm{(s)}}\) will melt to give \({\rm{C}}{{\rm{O}}_{\rm{2}}}{\rm{(l)}}\)? At approximately what temperature will this occur? (See Figure \({\rm{10}}{\rm{.34}}\) for the phase diagram.)
Explain why a hydrogen bond between two water molecules is weaker than a hydrogen bond between two hydrogen fluoride molecules.
Open the PhET States of Matter Simulation (http://openstaxcollege.org/l/16phetvisual) 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 to 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? Explain.
Water rises in a glass capillary tube to a height of 8.4cm. What is the diameter of the capillarytube?
The molecular mass of butanol,\({C_4}{H_9}OH\), is\(74.14\); that of ethylene glycol, \({\rm{C}}{{\rm{H}}_{\rm{2}}}\left( {{\rm{OH}}} \right){\rm{C}}{{\rm{H}}_{\rm{2}}}{\rm{OH}}\), is 62.08, yet their boiling points are \({\bf{117}}.{\bf{2}}{\rm{ }}^\circ {\bf{C}}\) and \(174 ^\circ C,\)respectively. Explain the reason for the difference.
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