- #1
Roshan Patel
- 3
- 1
I'm an anaesthetist... I have exams coming up... I use lots of gases and vapours and need to appreciate the associated physics.
My question relates to saturated vapour pressure and ambient pressure...
SVP increases with temperature - more molecules have sufficient energy to escape the surface/increased temp increases rate of endothermic reactions.
When a substance is below its SVP it behaves more or less as an ideal gas such that reducing volume/increasing pressure increases the partial pressure of the vapour within the mixture in accordance to Dalton's law.
What I do not understand is why at SVP pressure has no effect. I have seen this time and again but no explanation is given..
I would kindly appreciate clarification on this.
Thanks
My question relates to saturated vapour pressure and ambient pressure...
SVP increases with temperature - more molecules have sufficient energy to escape the surface/increased temp increases rate of endothermic reactions.
When a substance is below its SVP it behaves more or less as an ideal gas such that reducing volume/increasing pressure increases the partial pressure of the vapour within the mixture in accordance to Dalton's law.
What I do not understand is why at SVP pressure has no effect. I have seen this time and again but no explanation is given..
I would kindly appreciate clarification on this.
Thanks