How does boiling point evolve with decreasing pressure?
And first off, I should define
So if we reduce the ambient pressure, by means of a vacuum pump or water aspirator, we should substantially reduce the boiling point of the liquid, as less heat has to be pumped into the system in order that the vapour pressure of the liquid becomes equal to the (reduced!) ambient pressure. This underlies the principle of
I take it you are at A-level or 1st year university. If you are, you should definitely take this definition of boiling point on board. It is a fact that when we boil water in a kettle, the vapour pressure of the liquid is at
If you lived in Denver, Colorado (elevation 1610 m above sea level), what would you expect the temperature of boiling water to be? Why?