The following table presents the solubilities of several
gases in water at 25 °C under a total pressure of gas and
water vapor of 1 atm. (a) What volume of CH4(g) under
standard conditions of temperature and pressure is contained
in 4.0 L of a saturated solution at 25 °C? (b) The
solubilities (in water) of the hydrocarbons are as follows:
methane < ethane < ethylene. Is this because ethylene
is the most polar molecule? (c) What intermolecular
interactions can these hydrocarbons have with water?
(d) Draw the Lewis dot structures for the three hydrocarbons.
Which of these hydrocarbons possess p bonds?
Based on their solubilities, would you say π bonds are
more or less polarizable than s bonds? (e) Explain why
NO is more soluble in water than either N2 or O2. (f) H2
S is more water-soluble than almost all the other gases
in table. What intermolecular forces is H2S likely to have
with water? (g) SO2 is by far the most water-soluble gas
in table. What intermolecular forces is SO2 likely to have
with water?
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