Calculate the total pressure in the flask after all of the oxygen has been removed from the air in the flask. Assume that the temperature is 25¡ÆC, the initial barometric pressure is 760 torr
and that air is 21% oxygen by volume.
pO2 = XO2*Ptotal
pO2 = 0.21*760 = approx 160 mm
Then pressure remaining is 760-approx160 = approx?
To calculate the total pressure in the flask after all of the oxygen has been removed from the air, you need to consider the partial pressure of oxygen and the partial pressure of the other gases in the air.
Here are the steps to calculate the total pressure:
1. Convert the barometric pressure from torr to atm. There are 760 torr in 1 atm, so the barometric pressure is 760 torr/760 = 1 atm.
2. Calculate the partial pressure of oxygen in the air. Since air is 21% oxygen by volume, the partial pressure of oxygen can be calculated as:
Partial pressure of oxygen = (21/100) * 1 atm
3. Subtract the partial pressure of oxygen from the barometric pressure to calculate the partial pressure of the other gases in the air.
Partial pressure of the other gases = barometric pressure - partial pressure of oxygen
4. The total pressure in the flask after all of the oxygen has been removed is the sum of the partial pressure of oxygen and the partial pressure of the other gases.
Total pressure = partial pressure of oxygen + partial pressure of the other gases
Let's calculate the total pressure using these steps:
Partial pressure of oxygen = (21/100) * 1 atm = 0.21 atm
Partial pressure of the other gases = 1 atm - 0.21 atm = 0.79 atm
Total pressure = 0.21 atm + 0.79 atm = 1 atm
Therefore, the total pressure in the flask after all of the oxygen has been removed from the air is 1 atm.