At 25 °C the liquids 1-propanol (CH₃CH₂CH₂OH) and carbon tetrachloride (CCl₄) each have measurable vapor pressures. The dipole moments are 1.68 D for 1-propanol and 0.00 D for CCl₄. A student combines 10.0 mL of each liquid in a test tube, shakes vigorously, and observes the formation of a single transparent phase.
A second student instead combines 10.0 mL of 1-propanol with 10.0 mL of hexane (C₆H₁₄, dipole moment 0.00 D) under identical conditions and observes two distinct liquid layers at equilibrium.
Respond to the following.
(a) Using the information provided, determine whether 1-propanol is miscible with CCl₄, with hexane, with both, or with neither. Clearly state your conclusion for EACH pairing.
(b) For EACH pairing, explain how the dominant intermolecular forces present in the pure liquids account for the miscibility outcome you stated in part (a). In your explanation, reference at least two different types of intermolecular forces.
(c) The first student claims that the large difference in molar mass between 1-propanol (60 g mol⁻¹) and CCl₄ (154 g mol⁻¹) should prevent miscibility. Evaluate this claim and provide chemical reasoning to support or refute it.
(d) Predict how raising the temperature to 60 °C would affect the miscibility of each pair. Justify your predictions qualitatively in terms of changes to kinetic energy and the relative importance of intermolecular attractions.