Assuming that the air is essentially a mixture of nitrogen and oxygen in mole ratio of `4:1` by volume . Calculate the partial pressures of `N_(2)` and `O_(2)` on a day when the atmospheric pressure is 750 mm of Hg . Neglect the pressure of other gases.

Explanation

From Dalton's Law of partial pressure, we have
Partial pressure of nitrogen `= p_(N_(2)) = chi_(N_(2))xxP` and Partial pressure of oxygen `= p_(O_(2)) = chi_(O_(2) xxP`
Now, `chi_(N_(2)) = 4//5`, and `chi_(O_(2)) = 1//5`
`rArr p_(N_(2) ) = ( 4)/( 5) xx 750 = 600 `mm of Hg and `p_(O_(2)) = (1)/( 5) xx750 = 150 ` mm of Hg