Abreathing mixture used by deep sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 1 atmosphere if P He- 609.5 mm Hg and P $CO_2$ = 0.5 mm Hg?

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Answer 1 · 2017-01-12T10:12:59

The sum of the partial pressure are $1*atm$

$p_(O_2)~=0.20*atm$

$Sigmap_i=1*atm$ , where $p_i$ are the individual partial pressures.

And thus $p_(CO_2)+p_(O_2)+p_(He)=760*mm*Hg$

And thus, $p_(O_2)={760-p_(CO_2)-p_(He)}*mm*Hg$

$p_(O_2)={760-0.5-609.5}*mm*Hg$

$p_(O_2)=150*mm*Hg$

And we convert $p_(O_2)$ to atmospheres, knowing that $1*atm-=760*mm*Hg$ .

$p_(O_2)=(150*mm*Hg)/(760*mm*Hg*atm^-1)=??atm$

Abreathing mixture used by deep sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 1 atmosphere if P He- 609.5 mm Hg and P CO_2CO_2 = 0.5 mm Hg?