What is the total gas pressure in a sealed flask that contains oxygen at a partial pressure of 0.39 atm and water vapor at a partial pressure of 0.47 atm?
Add the partial pressures to get the total pressure.
It must be a hot flask to have a water vapor partial pressure that high.
To find the total gas pressure in the sealed flask, we need to use Dalton's Law of Partial Pressure. According to this law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas component.
In this case, we have two gas components: oxygen and water vapor. The partial pressure of oxygen is given as 0.39 atm, and the partial pressure of water vapor is given as 0.47 atm.
To find the total gas pressure, we simply add the partial pressures together:
Total gas pressure = partial pressure of oxygen + partial pressure of water vapor
Total gas pressure = 0.39 atm + 0.47 atm
Total gas pressure = 0.86 atm
Therefore, the total gas pressure in the sealed flask is 0.86 atm.