Henry 's law constant for the solubility of `N_(2)` gas in water at `298 K` is `1.0 xx 10^(5) atm`.

Henry 's law constant for the solubility of N_(2) gas in water at 298 K is 1.0 xx 10^(5) atm . The mole fraction of N_(2) in air is 0.6 . The number of moles of N_(2) from air dissolved in 10 moles of water at 298 K and 5 atm pressure is a. 3.0 xx 10^(-4) b. 4.0 xx 10^(-5) c. 5.0 xx 10^(-4) d. 6.0 xx 10^(-6)

The Henry's law constant for the solubility of N_(2) gas in water at 298 K is 1.0 xx 10^(5) atm . The mole fraction of N_(2) in air is 0.8 . The number of moles of N_(2) from air dissolved in 10 moles of water at 298 K and 5 atm . Pressure is:

The Henry's law constant for the solubility of N_(2) gas in water at 298K is 1.0 xx 10^(5) atm. The mole fraction of N_(2) in air is 0.8 . The number of moles of N_(2) from air dissolved in 10 moles of water at 298K and 5 atm pressure is

The Henry's law constant fo the solubility of N_(2) gas in water at 298 K is 1.0xx10^(5) atm. The mole fraction of N_(2) in air is 0.8. The number of moles of N_(2) from air dissolved in 10 moles of water at 298K and 5 atm pressue is

The Henry's law constant for the solubility of N_(2) gas in water at 298 K is 1xx10^(-5)" atm" . The mole fraction of N_(2) in air in 0.8. If the number of moles of N_(2) of air dissolved in 10 moles of water at 298 K and 5 atm x. 10^(-4) . Find the value of x.

Henry's law constant for the solubility of nitrogen gas in water at 298 K is 1.0 xx 10^(-5) atm . The mole fraction of nitrogen in air is 0.8 .The number of moles of nitrogen from air dissolved in 10 mol of water at 298 K and 5 atm pressure is