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?
I suspect you will have a solution of napthalene dissolved in dichloromethane
To determine the result of heating a mixture of dichloromethane 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 boiling points and solubility of the substances involved.
First, let's look at the boiling points:
- Dichloromethane (also known as methylene chloride) has a boiling point of around 40 degrees Celsius.
- Naphthalene has a relatively higher boiling point of around 218 degrees Celsius.
Based on this information, when the mixture is heated to 60 degrees Celsius, dichloromethane will start to evaporate, while naphthalene will remain in liquid form.
As you collect distillate (the evaporated substances) until no further material is distilled, you will mainly collect the dichloromethane vapor. It will condense in a separate collection vessel since its boiling point is lower. On the other hand, naphthalene will remain in the original flask.
Once you cool the flask back to room temperature, both the collected dichloromethane and the remaining naphthalene will return to their respective states: dichloromethane will become a liquid again, and naphthalene will remain as a solid.
Therefore, the outcome of heating the mixture, collecting the distillate (dichloromethane vapor), and then cooling back to room temperature would be the separation of the two substances, with dichloromethane collected separately as a liquid and naphthalene remaining as a solid in the original flask.