The total pressure in a vessel containing hydrogen collected over water at 25degrees Celsius was 0.8atm. the vapor pressure of water at the temperature is 23.8torr. What was the pressure of the oxygen in torr?
Ptotal = pO2 + pH2O
You want p in atm?
Convert 23.8 torr to atm.
0.8 atm = pO2 + (23.8/760)
Solve for pO2.
You want p in torr?
Convert 0.8 atm to torr
0.8*760 = pO2 + 23.8
Solve for pO2.
p in atm?
0.8atm = pO2 +0.031
0.8-0.031 = pO2
0.769atm = pO2
p in torr?
608 = pO2 + 23.8
608-23.8 = pO2
584.2 torr = pO2
To find the pressure of oxygen in torr, we need to consider Dalton's Law of Partial Pressures. According to Dalton's Law, the total pressure of a gas mixture is equal to the sum of the partial pressures of each gas in the mixture.
In this case, we have hydrogen and oxygen gases in the vessel. Let's denote the partial pressure of hydrogen as PH2 and the partial pressure of oxygen as PO2.
Given information:
Total pressure (Ptotal) = 0.8 atm
Vapor pressure of water (Pwater) = 23.8 torr
To determine the pressure of oxygen (PO2) in torr, we need to subtract the vapor pressure of water (Pwater) from the total pressure (Ptotal). However, we need to make sure that both pressures are in the same unit.
First, we need to convert the total pressure from atm to torr:
Ptotal = 0.8 atm x 760 torr/atm (since 1 atm = 760 torr)
Ptotal = 608 torr
Now, subtract the vapor pressure of water from the total pressure:
Partial pressure of oxygen (PO2) = Ptotal - Pwater
PO2 = 608 torr - 23.8 torr
PO2 = 584.2 torr
Therefore, the pressure of oxygen in torr is 584.2 torr.