what would be the result if we heated a mixture of dicholoromethane and naphalene to 60 degrees celcius, collected distillate until no further material is distilled, and then cooled the flask back to room temperature?
To determine the result of heating a mixture of dichloromethane (DCM) and naphthalene, and subsequently cooling it back to room temperature, we need to understand the boiling points of these substances.
Dichloromethane (DCM) has a boiling point of 40 degrees Celsius, while naphthalene has a boiling point of 218 degrees Celsius. This means that dichloromethane will vaporize and distill at a much lower temperature compared to naphthalene.
Given that the mixture is heated to 60 degrees Celsius, we can conclude that dichloromethane will readily vaporize, while naphthalene will not. As a result, the distillate collected during this process will primarily contain dichloromethane, with minimal to no naphthalene present.
When the flask is subsequently cooled back to room temperature, the dichloromethane in the distillate will condense back into its liquid state, while naphthalene will remain in the original flask as a solid since it did not vaporize. Thus, the end result will be a mixture containing solid naphthalene and liquid dichloromethane.
It's worth noting that this process assumes that all the naphthalene remained in the flask and didn't volatilize or react with any other substances present in the mixture.