# Problem: A gaseous mixture of O2 and N2 contains 40.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 605 mmHg?Express you answer numerically in millimeters of mercury.Dalton's law states that the total pressure, Ptotal, of a mixture of gases in a container equals the sum of the pressures of each individual gas:Ptotal=P1+P2+P3+...The partial pressure of the first component, P1, is equal to the mole fraction of this component, X1, times the total pressure of the mixture:P1=X1×PtotalThe mole fraction, X, represents the concentration of the component in the gas mixture, soX1=moles of component 1total moles in mixture

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A gaseous mixture of O2 and N2 contains 40.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 605 mmHg?

Express you answer numerically in millimeters of mercury.

Dalton's law states that the total pressure, Ptotal, of a mixture of gases in a container equals the sum of the pressures of each individual gas:

${\mathbf{P}}_{\mathbf{total}}\mathbf{=}{\mathbf{P}}_{\mathbf{1}}\mathbf{+}{\mathbf{P}}_{\mathbf{2}}\mathbf{+}{\mathbf{P}}_{\mathbf{3}}\mathbf{+}\mathbf{.}\mathbf{.}\mathbf{.}$

The partial pressure of the first component, P1, is equal to the mole fraction of this component, X1, times the total pressure of the mixture:

${\mathbf{P}}_{\mathbf{1}}\mathbf{=}{\mathbf{X}}_{\mathbf{1}}\mathbf{×}{\mathbf{P}}_{\mathbf{total}}$

The mole fraction, X, represents the concentration of the component in the gas mixture, so