A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 101.4kPa if P (He) = 68.7kPa and P (CO2) = 1.4kPa?

Question

Nola Boone

Chemistry

21 November, 09:28

A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 101.4kPa if P (He) = 68.7kPa and P (CO2) = 1.4kPa?

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Jordin Riddle · Answer 1

Answer is: pressure of oxygen is 31,3 kPa.

The total pressure of an ideal gas mixture is the sum of the partial pressures of the gases in the mixture.

p (mixture) = p (helium) + p (oxygen) + p (carbon dioxide).

p (oxygen) = p (mixture) - (p (helium) + p (carbon dioxide)).

p (oxygen) = 101,4 kPa - (68,7 kPa + 1,4 kPa).

p (oxygen) = 101,4 kPa - 70,1 kPa.

p (oxygen) = 31,3 kPa.