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 (also known as methylene chloride) and naphthalene to 60 degrees Celsius, collecting distillate until no further material is distilled, and then cooling the flask back to room temperature, we need to consider the properties of the involved substances and their boiling points.
Dichloromethane has a boiling point of 40 degrees Celsius, while naphthalene has a higher boiling point of 218 degrees Celsius. When a mixture is heated, substances with lower boiling points tend to vaporize and form distillate first. In this case, dichloromethane will likely vaporize and distill as it reaches its boiling point of 40 degrees Celsius.
At 60 degrees Celsius, dichloromethane is certainly in its vapor phase, resulting in its significant evaporation from the mixture. The collected distillate would predominantly consist of dichloromethane molecules.
As the process continues, the temperature remains at 60 degrees Celsius until there is no more dichloromethane left in the mixture. At that point, the distillation process would stop since the boiling point of naphthalene has not been reached.
Once the distillation process is complete, if the flask is cooled back to room temperature, both the distillate and the remaining mixture inside the flask will return to their original liquid states. The distillate collected should solely contain dichloromethane, while the original mixture in the flask would contain naphthalene, as it did not boil and distill during the heating process.
In conclusion, heating a mixture of dichloromethane and naphthalene to 60 degrees Celsius and collecting distillate until no further material is distilled would result in the separation of the dichloromethane from the mixture. The distillate collected would consist of pure dichloromethane, while the remaining mixture in the flask would still contain naphthalene. Cooling the flask back to room temperature would not change the composition of the substances, but they would return to their liquid states.