Question

Each of the containers below hold 150 ml of the indicated solution at 20 ⁰C which one would have the lowest rate of vaporization?

A) CH₃C1
B) H₂O
C) CH₃CI
D) H₂O

Answer 1

C) CH₃CI. To determine which solution has the lowest rate of vaporization, one must consider the boiling points and intermolecular forces.

Step-by-step explanation:

The student's question is about determining which of the given containers with a 150 ml solution would have the lowest rate of vaporization at 20 °C. By evaluating the solutions listed (CH₃Cl and H₂O), we can deduce that the answer will depend on the vapor pressure and intermolecular forces of the compounds in question.

Assuming there is a typo in the list with CH₃Cl repeated, and that one instance should be another compound, without the name of this other compound, we cannot provide a definitive answer. However, we can state that between water (H₂O) and methyl chloride (CH₃Cl), methyl chloride would typically have a higher rate of vaporization than water due to its lower boiling point and weaker intermolecular forces compared to water's strong hydrogen bonding.

Methyl chloride (CH₃Cl) generally vaporizes faster than water (H₂O) due to weaker intermolecular forces and a lower boiling point.