Assignment:
Q1. Describe the intermolecular force that must be overcome in converting each of the following from a liquid to a gas:
A. Liquid O2
B. Mercury
C. CH3I (methyl iodide)
D. CH3CH2OH (ethanol)
Q2. Rank the following in order of increasing strength of intermolecular forces in the pure substances. Which do you think might exist as gasses at 25"C and 1 atm: Ne, CH2, CO, and CCl4?
Q3. Explain why the boiling point of H2S is lower than that of water?
Q4. Which of the following compounds would be expected to form intermolecular hydrogen bonds in the liquid state?
A. CH3OCH3 (dimethyl either)
B. CH4
C. HF
D. CH3CO2H (acetic acid)
E. Br2
F. CH3OH (methanol)
Q5. The enthalpy of vaporization of liquid mercury is 59.11 kj/mol. What quantity of heat is required to vaporize 0.500 mL of mercury at 357'C, its normal boiling point? (The density of mercury is 13.6 g/mL.)
Q6. Assume you seal 0.1 g of diethyl ether in an evacuated 100.-mL flask. There are no molecules of any other gas in the flask. If the flask is held at 30'C, what is the approximate gas pressure in the flask? If the flask is place in an ice bath, does additional liquid ether evaporate of does some ether condense to a liquid?
Q7. Rank the following substances in order of increasing strength of intermolecular forces:
A. Ar
B. CH3Oh
C. CO2
D. CaO
Q8. If you place 1.0 of ethanol in a room that is 3.0 m long, 2.5 wide, and 2.5 high, does all the alcohol evaporate? If some liquid remains, how much remains? The vapor pressure of ethanol at 25'C is 59 mm Hg, and the density of the liquid at this temp is 0.785 g/cm3.
Provide complete and step by step solution for the question and show calculations and use formulas.