If `N_2` gas is bubbled through water at 293 K. how many millimoles of N, gas would dissolve in 1 litre of water. Assume `N_2` exerts a partial pressure of 0.987 bar. Given that Henry's law constant for `N_2` at 293 K is 76.45 bar.

Explanation

According to Henry.s law,
`{:(P_(N_(2)), K_H , , X_(N_(2))),("(partial pressure of nitrogen)",="(Henry.s law constant" ,xx, "(""mole fraction of" N_2")"):}`
`X_(N_(2)) =P_(N_2)/K_H`If.n. moles of `N_2` are present in 1 litre of `H_2 O`
(i.e., 55.5 moles),
`X_(N_(2))`=`n/(n+55.5)`
=`n/(55.5) (n lt lt 55.5)`
`therefore n/(55.5)=1.29 xx 10^(-5) xx 55.5`
= `71.595xx 10` moles