Question

Three of the primary components of air are

carbon dioxide, nitrogen, and oxygen. In a
sample containing a mixture of only these
gases at exactly one atmosphere pressure, the
partial pressures of carbon dioxide and nitrogen are given as PCO2 = 0.285 torr and
PN2 = 585.313 torr. What is the partial pressure of oxygen?
Answer in units of torr.

Answer 1

174.402 Torr is the partial pressure of oxygen gas.

Step-by-step explanation:

According to the Dalton's law, the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gasses.

`P_T=p_(1)+p_(2)+p_(3)...p_(n)`

where,

`P_T` = Total pressure

`p_(1)` = partial pressure of gas-1

`p_(2)` = partial pressure of gas-2

`p_(3)` = partial pressure of gas-3

`p_(n)` = partial pressure of nth gas in the mixture

We have:

`P_T= 1 atm = 760 Torr`

`p_(CO_2)=0.285 Torr`

`p_(N_2)=585.313 Torr`

`p_(O_2)=?`

Now put all the given values is expression, we get the partial pressure of the
`O_2` gas.

`P_T=p_(CO_2)+p_(N_2)+p_(O_2)`

`760 Torr=0.285 Torr+585.313 Torr+p_(O_2)`

`p_(O_2)=174.402 Torr`

174.402 Torr is the partial pressure of oxygen gas.