What does it mean if we increase the temperature we increase the vapor pressure? I understand...

What does it mean if we increase the temperature we increase the vapor pressure?

I understand if we increase their KE energy more particles will possess enough energy to escape from the liquid surface.

But vapor pressure is measured in an isolated system, where no heat and mass are escaping.

So, assuming we increase the temperature of our sample by 10 degree celcius, does that mean we would expect more concentration of particles at equilibrium in the gas phase?

Expert Solution

Even for an isolated system, there will be equlibrium between liquid and vapour phase.

Suppose, you prepared a solution in volumetric flask and it is pefectly closed.There will be generation of vapour above the liquid which will change the concentration of the solution if it is left for a long time.

If you increase the temperature, the equlibrium will be disturbed since the chemical potential in liquid phase will be greater than vapour phase because it is a function of temperature and pressure.So, the escaping tendency will be more towards the vapour phase to equalise the chemical potential in the two phases and consequently will be chnaged accordingly.

queen_honey_blossom answered 2 years ago

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