- #1

ContrapuntoBrowniano

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- TL;DR Summary
- Why does pressure and volume seem unnaffected for temperature changes in a heated cooking pot filled with water?

Hi! I wanted to do some basic calculations for temperature T on a water-filled pot. I noticed something strange on my calculations, and couldn’t figure out what was wrong...

So here it is:

The ideal gas formula:

k=PV

The actual formula Relates equally the product PV with the a constant associated with temperature. So, i never saw any flaws in this relationship for fluids...until today! You’ll see... If we vary the pressure or the volume leaving the other one constant, then the temperature will also vary accordingly, however, if we vary the temperature, the pressure and volume migth stay the same! This is the case of the heated water pot:

If water is an uncompressible fluid, the pressure changes appear insignificant to it, and since the only thing i’m doing is heating water, the volume stays the same...but “T” IS rising. Is there something I’m not considering?

So here it is:

The ideal gas formula:

k=PV

The actual formula Relates equally the product PV with the a constant associated with temperature. So, i never saw any flaws in this relationship for fluids...until today! You’ll see... If we vary the pressure or the volume leaving the other one constant, then the temperature will also vary accordingly, however, if we vary the temperature, the pressure and volume migth stay the same! This is the case of the heated water pot:

If water is an uncompressible fluid, the pressure changes appear insignificant to it, and since the only thing i’m doing is heating water, the volume stays the same...but “T” IS rising. Is there something I’m not considering?