My confusion part is that why the partial pressure of the low solubility gas in gaseous phase and liquid phase are still the same even though the concentration of that gas in liquid phase is lower than that in the gaseous phase. Is that when it reach equilibrium rate, so the partial pressure is the same between the two phases? But why different concentration of gases in the two phases do not affect the partial pressure?
Because of equilibrium.. Be it low or high solubility, once the system reaches equilibrium, the amount of molecules entering and exiting would be equal isnt it?
Finally understood why Caisson's disease occurs too now. Thank you so much for your amazing videos integrating physics and medicine!
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Thanks Again :)
Thank you so much sir. Crystal clear 🙏🙏🙏❤
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Thank you so much!
Oh wow that nice, good work prof
Thank you! Cheers!
thank you so much! Your video was very helpful.
Doesn't the partial pressure of o2 & CO2 drop after reaching equilibrium? Why is it still at 100mmHg?
yes ig because volume goes up
My confusion part is that why the partial pressure of the low solubility gas in gaseous phase and liquid phase are still the same even though the concentration of that gas in liquid phase is lower than that in the gaseous phase. Is that when it reach equilibrium rate, so the partial pressure is the same between the two phases? But why different concentration of gases in the two phases do not affect the partial pressure?
Because of equilibrium.. Be it low or high solubility, once the system reaches equilibrium, the amount of molecules entering and exiting would be equal isnt it?
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