What Happens to Pressure During a Temperature Decrease?

[Junkwisch]

The question is in the attachment... "this is an old past exam question"

for i) I assume that the pressure will remain constant (I'm not sure) since volume is likely to increase proportion to the decrease in temperature. (Is this correct?)

Best Regards

 

[Simon Bridge]

for i) I assume that the pressure will remain constant (I'm not sure) since volume is likely to increase proportion to the decrease in temperature. (Is this correct?)

What leads you to believe that the volume increases when temperature decreases?
Do you know an equation that relates volume to temperature for a gas?

The graph shows how the saturation vapor pressure varies with temperature for "a parcel of air".

You notice that the initial state vapor pressure is lower than the saturation vapor pressure - is it possible for the vapor pressure to be higher than the saturation pressure? i.e. what does "saturation vapor pressure" mean?

 

[Junkwisch]

What leads you to believe that the volume increases when temperature decreases?
Do you know an equation that relates volume to temperature for a gas?

The graph shows how the saturation vapor pressure varies with temperature for "a parcel of air".

You notice that the initial state vapor pressure is lower than the saturation vapor pressure - is it possible for the vapor pressure to be higher than the saturation pressure? i.e. what does "saturation vapor pressure" mean?

Since it is a parcel of air, the volume is constant? thus the only that that will change is pressure? Can I use the ideal gas law in this case? "PV=nRT"

I think it is nott possible for vapour pressure to be higher than saturated vapour pressure since it will precipitate (I'm not certain)

 

[Simon Bridge]

Since it is a parcel of air, the volume is constant?

Well you just said that the volume increases as temperature decreases - now you are saying the volume stays the same?

Can I use the ideal gas law in this case? "PV=nRT"

Lets pretend that you can use the ideal gas equation - what does that equation tell you happens to the pressure (at constant volume) as the temperature decreases or the volume (at constant pressure) for that matter?
Compare with what you wrote in post #1.

However - the question is talking about vapor pressure - is this different from the gas pressure?
Do you know any definitions for vapor pressure?

I think it is nott possible for vapour pressure to be higher than saturated vapour pressure since it will precipitate (I'm not certain)

... then this is something you need to check. It looks like you need to revise your work on vapor pressure.

Looking at the graph, if the temperature dropped, but the vapor pressure stayed the same, would the vapor pressure be above or below the saturation pressure?

You may find useful:
http://nicholas.duke.edu/people/faculty/katul/ENV234_Lecture_2.pdf
http://www.ldeo.columbia.edu/~martins/hydro/lectures/evap_precip.htm

 

[Junkwisch]

thank you for your help Simon, I have been going through much of my lecture note and recording in the recent days. It seems that the ideal gas law has nothing to do with this case. by using this equation saturation vapour pressure = 0.6108exp(17.27*T/T+237.
3), I got saturation vapour pressure to be equal to 1.23 kPa. (This is correct right?) It seems like this poinrt (10, 1.23) is above the blue line, thus precipitation will occurJunks

 

[Simon Bridge]

That's better ;)