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 and naphthalene to 60 degrees Celsius and then cooling it back to room temperature, we need to understand the properties and behaviors of both chemicals.
Dichloromethane (also known as methylene chloride) is a volatile organic compound with a low boiling point of 40 degrees Celsius. On the other hand, naphthalene is a solid aromatic hydrocarbon that sublimes (turns directly from solid to gas) at temperatures above 80 degrees Celsius.
Based on this information, heating the mixture of dichloromethane and naphthalene to 60 degrees Celsius would cause the dichloromethane to vaporize since its boiling point is lower than the selected temperature. The naphthalene, however, will remain in its solid state since it requires a higher temperature to sublimate.
When you collect the distillate (the condensed vapors) until no further material is distilled, it is likely that the distillate will mostly consist of dichloromethane. This is because it has a lower boiling point and is more volatile compared to naphthalene.
Upon cooling the flask back to room temperature, the dichloromethane will condense and return to its liquid state. Naphthalene, being a solid, will remain unchanged since its sublimation temperature was not reached during heating.
So, the result of this process would be a mixture containing dichloromethane as a liquid and naphthalene as a solid, with most of the volatile dichloromethane having been distilled and then condensed back to a liquid state.