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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.

Respuesta :

Answer:

174.402 Torr is the partial pressure of oxygen gas.

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.

[tex]P_T=p_{1}+p_{2}+p_{3}...p_{n}[/tex]

where,

[tex]P_T[/tex] = Total pressure

[tex]p_{1}[/tex] = partial pressure of gas-1

[tex]p_{2}[/tex] = partial pressure of gas-2

[tex]p_{3}[/tex] = partial pressure of gas-3

[tex]p_{n}[/tex] = partial pressure of nth gas in the mixture

We have:

[tex]P_T= 1 atm = 760 Torr[/tex]

[tex]p_{CO_2}=0.285 Torr[/tex]

[tex]p_{N_2}=585.313 Torr[/tex]

[tex]p_{O_2}=?[/tex]

Now put all the given values is expression, we get the partial pressure of the [tex]O_2[/tex] gas.

[tex]P_T=p_{CO_2}+p_{N_2}+p_{O_2}[/tex]

[tex]760 Torr=0.285 Torr+585.313 Torr+p_{O_2}[/tex]

[tex]p_{O_2}=174.402 Torr [/tex]

174.402 Torr is the partial pressure of oxygen gas.

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