Respuesta :

P = 2.95 atm, total pressure
N = 0.220 + 0.350 + 0.640 = 1.21 moles, total moles

According to Dalton's Law, the partial pressure of H₂ is
(0.350/1.21)*(2.95 atm) = 0.8533 atm

Answer: 0.853 atm

Answer :  The partial pressure of [tex]H_2[/tex] is, 0.853 atm

Solution :

First we have to calculate the mole fraction of [tex]H_2[/tex] in the mixture.

Formula used :

[tex]X_{H_2}=\frac{n_{H_2}}{n_{H_2}+n_{CO}+n_{He}}[/tex]

Now put all the given values in this formula, we get

[tex]X_{H_2}=\frac{0.35}{0.22+0.35+0.64}=0.289[/tex]

Now we have to calculate the partial pressure of [tex]H_2[/tex]

Formula used :

[tex]p_{H_2}=X_{H_2}\times P_T[/tex]

where,

[tex]P_T[/tex] = total pressure = 2.95 atm

[tex]p_{H_2}[/tex] = partial pressure of nitrogen gas = ?

[tex]X_{H_2}[/tex] = mole fraction of nitrogen gas = 0.289

Now put all the given values in the above formula, we get

[tex]p_{H_2}=0.289\times 2.95atm[/tex]

[tex]p_{H_2}=0.853atm[/tex]

Therefore, the partial pressure of [tex]H_2[/tex] is, 0.853 atm

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