the table above shows the structural formulas and molar masses for three different compounds. which of the…

the table above shows the structural formulas and molar masses for three different compounds. which of the following is a list of the compounds in order of increasing boiling points?\n(a) butane < 1 - propanol < acetone\n(b) butane < acetone < 1 - propanol\n(c) 1 - propanol < acetone < butane\n(d) acetone = butane < 1 - propanol

the table above shows the structural formulas and molar masses for three different compounds. which of the following is a list of the compounds in order of increasing boiling points?\n(a) butane < 1 - propanol < acetone\n(b) butane < acetone < 1 - propanol\n(c) 1 - propanol < acetone < butane\n(d) acetone = butane < 1 - propanol

Answer

Explanation:

Step1: Analyze intermolecular forces

  • Butane: Only has weak London dispersion forces.
  • Acetone: Has dipole - dipole forces in addition to London dispersion forces.
  • 1 - propanol: Has hydrogen bonding (strongest intermolecular force among the three) along with London dispersion and dipole - dipole forces.

Step2: Relate intermolecular forces to boiling point

  • The stronger the intermolecular forces, the higher the boiling point.
  • Since London dispersion forces < dipole - dipole forces < hydrogen bonding.
  • So, butane (weakest intermolecular forces) has the lowest boiling point, followed by acetone, and 1 - propanol (strongest intermolecular forces) has the highest boiling point.

Answer:

B. Butane < acetone < 1 - propanol