<p>Name:______Date:______Review Sheet 1. Use the Heating Curve below to answer each of the following. a. How does an increase in temperature during part A of the heating curve affect the average kinetic energy of the molecules in this system? ______b. At segment D, the temperature of the system remains constant, but heat energy continues to be added. Where does this energy go? Explain using the particle behavior. ______c. The molar heat of vaporization (energy required to turn a liquid into a gas) is usually much larger than the molar heat of fusion (energy required to turn a solid into a liquid). Explain this observation using molecular structure. ______2. Which of the following molecules would have the highest boiling point? Explain using Intermolecular Forces.</p><p>NH3 GeO2 H2Se CCl4 ______3. Describe the difference between solutions that are saturated and unsaturated. ______</p><p>4. Below are two ions in solutions. If water is introduced to the ions, how will the particles interact? Complete the picture by drawing in some water molecules. Hint: Water is polar. 5. Use the solubility curve shown to answer each of the following.</p><p> a. What mass of KNO3 will produce a saturated solution in 100 g of water at 40oC? b. A solution contains 60 g of KCl and 100 g of water at 80oC. Is this saturated (S) or unsaturated (U)?</p><p> c. A solution contains 70 g of NH4Cl in 100 g of water. What temperature does it need to be to be saturated?</p><p>Use the Phase Diagram shown below to answer questions 6 – 11. </p><p>6. Label the above diagram with S for solid, L for liquid and G for gas. 7. Label the melting point and boiling point at 1 atm. 8. Label the triple point and critical point. 9. Draw arrows to represent the following phase changes: condensation, deposition, and melting. 10. What is the approximate boiling point of this substance when the pressure is 0.6 atm? ______11. What phase would this substance most likely be in at 50oC and 1.0 atm? ______</p><p>Answer the following questions about the above heating curve:</p><p>12. What is the melting temperature of the above substance? _____</p><p>13. What is the freezing temperature of the above substance? _____</p><p>14. What is the boiling temperature of the above substance? _____ 15. The part of the graph labeled “e” represents temperatures at which gas is being heated. Describe what is happening for each of the other lettered sections of the graph:</p><p> a. ______b. ______c. ______d. ______16. In which section of the graph are atoms moving the least? ______17. In which section of the graph is this substance all liquid? ______18. On your graph, draw an arrow to and label each of the following: “melting begins”, “melting complete”, and “boiling begins”. </p><p>19. Use IMFs to explain the following differences in boiling points: a. HF (20 °C) and HCl (-85 °C)</p><p> b. Br2 (59 °C) and ICl (97 °C)</p><p>20. Which of the following would be expected to have the highest boiling point? Explain your choice. CO2 Ar CF4 LiCl SiF4</p>