- #1
rocketboy
- 243
- 1
Ok, I have been going through my chemistry notes on molecular geometry...and I don't understand the following:
In my notes it says that
-"as pressure goes up, so does the boiling point"
-"High vapour pressure means weak attractive force between the molecules and low vapour pressure means strong attractive force".
-"as temperature goes up, so does vapour pressure"
So my question is:
If when the pressure of a system increases, why does the boiling point? When pressure increases, the attractive force is weaker...so why does the temperature have to be greater in order for the substance to boil? If the bonds are weaker less energy is needed to break them, which to me indicates the boiling point should decrease.
I know I'm wrong, could somebody please help me?
Thanks,
-Jon
In my notes it says that
-"as pressure goes up, so does the boiling point"
-"High vapour pressure means weak attractive force between the molecules and low vapour pressure means strong attractive force".
-"as temperature goes up, so does vapour pressure"
So my question is:
If when the pressure of a system increases, why does the boiling point? When pressure increases, the attractive force is weaker...so why does the temperature have to be greater in order for the substance to boil? If the bonds are weaker less energy is needed to break them, which to me indicates the boiling point should decrease.
I know I'm wrong, could somebody please help me?
Thanks,
-Jon