These exercises, which make use of the unique features of your student CD-Rom, Central Science Live, can also be found at the end of the chapter in your book, Chemistry: The Central Science, 8th Edition. If you've installed Central Science Live on your computer, you will be able to do these exercises by going to the referenced eChapter on the student CD-ROM.
(Note: It is best if you are using the browser installed with Central Science Live, as it has been correctly configured to display the contents of Central Science Live.)
| 11.103 | The Changes of State movie (eChapter 11.4) shows the heating curve of a substance that melts and then vaporizes. (a) Using the information in Figure 11.25(b), sketch the heating curve of carbon dioxide at atmospheric pressure, starting at -100°C and ending at 30°C. (b) Sketch the same heating curve as it would appear at a pressure of 10 atm. (c) Under what conditions would the heating curve of water resemble the one you sketched for part (a)? |
| 11.104 | Using the Equilibrium Vapor Pressure simulation (eChapter 11.5), compare the vapor pressures of methanol, ethanol, acetic acid, water, and benzene. (a) Which compound appears to have the strongest intermolecular forces at 100°C? (b) If one compound has a higher equilibrium vapor pressure than another at a particular temperature, will it necessarily have a higher equilibrium vapor pressure at all temperatures? If not, give an example of two compounds whose vapor pressure curves cross, and at what temperature they have roughly the same vapor pressure. |
| 11.105 | Ethanol and acetic acid have very similar molar masses and both exhibit hydrogen bonding. In which of these two compounds is hydrogen bonding a more significant component of the overall intermolecular forces? Support your answer using data from the Equilibrium Vapor Pressure simulation (eChapter 11.5). |
| 11.106 | Water is a substance with some very unusual properties. (a) Based on a comparison of the water molecule and the structure of ice (eChapter 11.8), explain why ice is less dense than water, and (b) why increasing pressure, within a certain temperature range, causes ice to melt. (c) Why is it not possible to convert ice to liquid water by applying pressure at very low temperatures? |
| 11.107 | Compare the structure of ice (eChapter 11.8) with the structure of diamond (eChapter 11.8). If you rotate the structures just right, you will see distinct similarities, namely sp3 hybridization (of oxygen and carbon, respectively) and the hexagonal arrangement of atoms. Given this similarity, explain why ice can be melted by applying pressure whereas diamond cannot. |
