What is the total gas pressure in a sealed flask that contains oxygen at a partial pressure of 0.41 atm and a water vapor at a partial pressure of 0.58 atm?

1 Answer
May 15, 2014

According to Dalton's Law of Partial Pressures

#P_(Total) = P_1 + P_2 + P_3 …#

According to Dalton's Law, in a mixture of non-reacting gasses, the total pressure exerted is the sum of the partial pressures of the component gasses. In more complicated circumstances, equilibrium states come into effect, but fortunately for us, oxygen is non-reactive with water vapor.

This being the case we wold simply add the partial pressure of the gas and the water vapor.

#P_(Total) = P_(O_2) + P_(H_2O)#

#P_(Total) = 0.41 atm + 0.58 atm#

#P_(Total) = 0.99 atm#

I hope this was beneficial.