A sample of oxygen is collected over water at 22°C and 762 torr. What is the partial pressure of the dry oxygen? The vapor pressure of water at 22°C is 19.8 torr.
Dalton's law of partial pressures applies.
762torr = pressuredryO2+watervaporpressure.
To find the partial pressure of the dry oxygen, we need to subtract the vapor pressure of water from the total pressure.
Given:
Total pressure (Ptotal) = 762 torr
Vapor pressure of water (Pwater) = 19.8 torr
The partial pressure of dry oxygen (Pdry oxygen) can be calculated as follows:
Pdry oxygen = Ptotal - Pwater
Pdry oxygen = 762 torr - 19.8 torr
Pdry oxygen = 742.2 torr
So, the partial pressure of the dry oxygen is 742.2 torr.
To find the partial pressure of the dry oxygen, we need to subtract the vapor pressure of water from the total pressure.
Given:
Temperature (T) = 22°C = 295 K
Total pressure (P_total) = 762 torr
Vapor pressure of water (P_water) = 19.8 torr
Partial pressure of dry oxygen (P_oxygen) = P_total - P_water
Substituting the given values:
P_oxygen = 762 torr - 19.8 torr
P_oxygen = 742.2 torr
Therefore, the partial pressure of the dry oxygen is 742.2 torr.