The partial pressures of CH4, N2, and O2 in a sample of gas were found to be 135 mmHg, 508 mmHg, and 571 mmHg, respectively. Calculate the mole fraction of nitrogen.

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

= 0.4

Therefore, mole fraction of N₂ is 0.4

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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