Henry's law constant for molality of `CH_(4)` in benzene at `298K` is `3.8times10^(3)mm` of `Hg` . Calculate solubility of `CH_(4)` in benzene at `760` mm of Hg?

Henry's law constant for the molality of methane in benzene at 298K is 4.27xx10^(5)mm Hg . Calculate the solubility of methane in benzene at 298 K under 760 mm Hg .

Henry's law constant for the molality of methane in benzene at 298 K is 4.27xx10^(5)mm Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.

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

Henry's law constan for the solubility of methane in benzene is 4.27 xx 10^(-5) mm^(-1) Hg mol dm^(-3) at constant temperature .Calculate the solubility of methane at 760 mm Hg pressure at same temperature .

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

Henry's law constant for CO_(2) in water is 1.6times10^(8)Pa at 298K . The quantity of CO_(2) in 500g of soda water when packed under 3.2 bar pressure at 298K is

Henry's law constant for CO_(2) in water is 2.5xx10^(8)Pa at 298K . Calculate mmole of CO_(2) dissolved in 14g water at 2.5atm pressure at 298K . [Take 1atm=10^(5)N//m^(2) or Pa ]