Question

Deep-sea divers must use special gas mixtures in their tanks, rather than compressed air, to avoid serious problems. One such breathing mixture contains helium, oxygen, and carbon dioxide. Determine the partial pressure of oxygen when the total pressure in the tank is 201.4 kPa if PHe = 125.4 kPa and PCO2= 18.2 kPa? Must show all work that leads to answer for credit

Answer 1

Answer: The partial pressure of oxygen gas is 57.8 kPa

Step-by-step explanation:

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the partial pressure of oxygen gas, we use the law given by Dalton, which is:

`P_T=p_(He)+p_(O_2)+p_(CO_2)`

We are given:

Total pressure of the tank,
`P_T` = 201.4 kPa

Vapor pressure of helium,
`p_(He)` = 125.4 kPa

Vapor pressure of carbon dioxide,
`p_(CO_2)` = 18.2 kPa

Putting values in above equation, we get:

`201.4=125.4+p_(O_2)+18.2\\\\p_(O_2)=201.4-[125.4+18.2]=57.8kPa`

Hence, the partial pressure of oxygen gas is 57.8 kPa