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When N2 gas is passed through water at 2...

When `N_2` gas is passed through water at 293 K, how many moles of ` 1N_2` would dissolve in one litre water ? Assume that `N_2` exert a partial pressure of 0.987 bar. `K_H` for `N_2` at 293 K is 76.48 kilobar.

Text Solution

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The solubility of a gas in a liquid is related to the mole fraction by Henry.s law as `p= K_(H) chi`.
`chi_(("Nitrogen"))= (p_(("Nitrogen")))/(K_(H))= (0.98 "bar")/(76480 "bar")=1.29 xx 10^(-5)`
Number of moles of water in 2.5L of water =2500/18=138.89
Let n be the number of moles of `N_(2)` in solution
`chi_(("Nitrogen"))=(n mol)/(n mol +138.89 mol)`
n in the denominator is neglected as it is `lt lt 55.5`
`1.29 xx 10^(-5)= (n mol)/(138.89 mol)`
`n=1.29 xx 0^(-5) xx 138.89= 1.792 xx 10^(-3)` mol
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