The Henry's law constant for the solubility of N2 gas in water at 298 K is atm

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Problem

The Henry's law constant for the solubility of N₂ gas in water at 298 K is

1.0 \times 10^5

atm. The mole fraction of N₂ in air is 0.8. The number of mole of N₂ from air dissolved in 10 mole of water at 298 K and 5 atm pressure is: (1)

4.0 \times 10^{-4}

(2)

4.0 \times 10^{-5}

(3)

5.0 \times 10^{-4}

(4)

4.0 \times 10^{-6}