Hello!
We have the following statement data:
Data:
[tex] P_{Total} = 800 mmHg[/tex]
[tex]P\% N_{2} = 60\%[/tex]
[tex]P\% O_{2} = 40\%[/tex]
[tex] P_{partial} = ? (mmHg)[/tex]
As the percentage is the mole fraction multiplied by 100:
[tex]P = X_{ O_{2} }*100[/tex]
The mole fraction will be the percentage divided by 100, thus:
What is the partial pressure of oxygen in this mixture?
[tex] X_{ O_{2} } = \frac{P}{100} [/tex]
[tex] X_{ O_{2}} = \frac{40}{100}[/tex]
[tex]\boxed{X_{ O_{2}} = 0.4}[/tex]
To calculate the partial pressure of the oxygen gas, it is enough to use the formula that involves the pressures (total and partial) and the fraction in quantity of matter:
In relation to [tex]O_{2}[/tex] :
[tex] \frac{P O_{2} }{P_{total}} = X_O_{2} [/tex]
[tex]\frac{P O_{2} }{800} = 0.4[/tex]
[tex]P_O_{2} = 0.4*800[/tex]
[tex]\boxed{\boxed{P_O_{2} = 320\:mmHg}}\end{array}}\qquad\quad\checkmark[/tex]
Answer:
b. 320.0 mm hg
