Answer:
0.4
Explanation:
The total pressure of the mixture is the sum of the pressures of all the gases;
Let the total pressure be PT
PT = 135 mmHg + 508 mmHg + 571 mmHg = 1214 mmHg
Partial pressure = mole fraction * total pressure
mole fraction = partial pressure/total pressure
partial pressure of nitrogen = 508 mmHg
mole fraction = 508 mmHg/1214 mmHg
mole fraction = 0.4
The proportion of the moles present in the whole amount of moles in a mixture is called a mole fraction.
In a gaseous mix, the partial pressure of single gas will be equal to the product of mole fraction and partial pressure of the particular gas.
The mole fraction of Nitrogen will be 0.4.
This can be calculated by:
The total pressure will be:
= 135 mmHg + 508 mmHg + 571 mmHg
= 1214 mmHg
[tex]\text{Partial pressure} & = \text{Mole fraction} \times \text{Total Pressure}[/tex]
[tex]\text{Mole fraction} = \dfrac{\text{Partial pressure}} {\text{Total pressure}}[/tex]
[tex]\text{Mole fraction} = \dfrac{\text{508 mm Hg}} {\text{1214 mm Hg}}[/tex]
= 0.4
Therefore, mole fraction of N₂ is 0.4
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