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?

Question

5006 views around the world

You can reuse this answer
Creative Commons License

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#