olecular forces are what cause molecules to âstick together" in liquid and solid states. In bonds (intermolecular attractions between a hydrogen atom bonded to an electrone in an egative atom like nitrogen, oxygen or fluorine in one molecule and the N, O, or F atom other molecule) are stronger than simple dipole forces (between polar molecules) and, of rse, the more hydrogen bonds, the stronger the intermolecular forces Put a drop of ethanol, distilled water, and acetone onto three different temperature probes simultaneously. Then, compare the difference in behavior, particularly noting the rate of mperature changes. Compare the data taken at same time. Results 1. Describe the graph including data points. 2. Complete the Table helow Heat of vaporization Initial Final Temp. Rate Rate H-bond Exothermic / temp. temp.changeC/s) ranking strengthEndothermie Solvent ranking* 2A. Water 25 20.9 037 30 |B. Ethanol | asy .4-ä¸ä¸12. 2lo C. Acetone 23 67 Final temp. should be taken at the time when acetone reaches to minimum temp. **Rank the H-bond strength in the three solvents used in this experiment, 1 being the strongest and 3 being the weakest. Discussion Questions y how intermolecular forces affect heat of vaporization and rate of 1. Explain briefl vaporization? Using data from the lab show the correlations between rate of vaporization and intermolecular force strength. in with data why the temperature decreases with time for all three solvents? What 2. Expla was your expectation and does it agree?