In each of the following groups of substances, pick the one that has the given property. Justify your answer. a. highest boiling point: HBr, Kr, or Cl2 b. highest freezing point: H2O, NaCl, or HF c. lowest vapor pressure at 25C: Cl2, Br2, or I2 d. lowest freezing point: N2, CO, or CO2 e. lowest boiling point: CH4, CH3CH3, or CH3CH2CH3 f. highest boiling point: HF, HCl, or HBr g.

5-86 Using the phase diagram of water (Figure 5-20), describe the process by which you can sublime 1 g of ice at-10°C and at 1 atm pressure to water vapor at the same temperature.

For each of the following pairs, choose the member with the lower boiling point. Explain your reason in each case. (a) NaCl or PCl3 (b) NH3 or AsH3 (c) C3H7OH or C2H5OCH3 (d) HI(g) or HCl(g)

(a) How do the structures of these molecules account for these differences in boiling point? Provide a full account of the structures and their influence on the differences in this physical property. Name Boiling Point methane -161.6 °C methanol 64.7 °C propane -42 °C propan-1-ol 97 °C

Which compound has a higher boiling point: butane, C4 H10, or hexane, C6H4?

The boiling points of noble gases (Groups 8A elements) increase going from top to bottom of the column. True or False?

3) Which of the following compounds has the higher boiling point Justify your answer. INclude drawings where appropriate. CHICHỊCH CENT CH3 11 CH₂ CN(CH₂)₂

The following compounds, represented with ball-and-stick models, have the same molecular formulas (C5H12). Which would you expect to have a higher boiling point? Select the single best answer. ×

Which molecule ( CH3OH or CH4 ) has a greater vapor pressure and why?