Because the presence of impurities will block more molecules to jump to gaseous state so the vapore pressure will decrease, hence more energy is needed to elevate vapore pressure to environment pressure and higher boiling point is resulted.Borek said:
Brwahussen said:
But everyone has to start somewhere.Thanks!Borek said:OK
It is not exactly about energy (although in a way you are right, you need energy to heat up the mixture), more like you need a higher temperature so that the partial pressure of the solvent becomes equal to the external pressure. But in general you are on the right track. Note that is pretty easy to show using Raoult's law (try!).
Yes.
Actually it is not just bad, it is atrocious
Brwahussen said:
A volatile impurity is a substance that can easily evaporate or vaporize at room temperature. It is typically a liquid or gas that has a low boiling point.
A volatile impurity can lower the boiling point of a liquid. This is because the impurity molecules can mix with the liquid molecules, making it easier for the liquid to overcome the intermolecular forces and turn into a gas.
No, a volatile impurity can only lower the boiling point of a liquid. This is because the impurity molecules do not have strong intermolecular forces and therefore do not contribute to the boiling point of the liquid.
The higher the concentration of a volatile impurity, the lower the boiling point of the liquid will be. This is because there are more impurity molecules present to disrupt the intermolecular forces of the liquid molecules.
Yes, a volatile impurity can affect the boiling point of all liquids. However, the magnitude of the effect may vary depending on the strength of the intermolecular forces in the liquid and the concentration of the impurity.