A sample of O2(g) is saturated with water vapor at 27 C. The total pressure of the mixture is 772 torr, and the vapor pressure of water is 26.7 torr at 27 C. What is the partial pressure of the O2?
jhcv
Well, it seems like O2 is feeling a little under pressure in this situation. But don't worry, I'm here to help bring some clarity to the situation!
To find the partial pressure of O2, we need to subtract the vapor pressure of water from the total pressure of the mixture.
So, let's do some math:
Total pressure - Vapor pressure of water = Partial pressure of O2
772 torr - 26.7 torr = Partial pressure of O2
Now let me calculate that for you (humming the Jeopardy music)...
*beep boop beep boop*
Partial pressure of O2 = 745.3 torr
There you go! The partial pressure of O2 in this mixture is 745.3 torr. O2 can breathe a little easier now!
To find the partial pressure of O2 in the mixture, we need to subtract the vapor pressure of water from the total pressure.
Partial pressure of O2 = Total pressure - Vapor pressure of water
Partial pressure of O2 = 772 torr - 26.7 torr
Partial pressure of O2 = 745.3 torr
Therefore, the partial pressure of O2 in the mixture is 745.3 torr.
To find the partial pressure of O2 in the mixture, we need to subtract the vapor pressure of water from the total pressure.
Partial pressure of O2 = Total pressure - Vapor pressure of water
Partial pressure of O2 = 772 torr - 26.7 torr
Partial pressure of O2 = 745.3 torr
Therefore, the partial pressure of O2 in the mixture is 745.3 torr.
The total pressure is 772 torr and the water vapor is 26.7 torr so 772 - 26.7 = 754.3 torr
So partial pressure = 754.3