Henry's law constant for `CO_(2)` in water is `1.67xx10^(8)` Pa at 298 K. Calculate the quantity of `CO_(2)` in 500 mL of soda water when packed under 2.5 atm `CO_(2)` pressure at 298 K.

The quantity of CO_(2) in 500 mL of soda water when packed under 3.34 bar CO_(2) pressure at 298 K in g is

Henry' s law constant for CO_(2) in water is 1.67 K bar at 25^(@)C. The quantity of CO_(2) in 1000 mL of soda water when packed under 5 bar CO_(2) pressure at 23^(@)C is

The quantity of CO_2 in 500ml of soda water when packed under 2.5 atm CO_2 pressure at 298 k is....... gm (Henry's law constant 1.67 xx 10^8 pa at 298K)

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 constant for solubility of N_(2) gas in water at 298K 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 pressure is :

The acid formed when CO_2 is dissolved in water-

If CO_(2) gas having a partial pressure of 1.67 bar is bubbled through 1 L water at 298 K the amount of CO_(2) dissolved in water in g L^(-1) is approximately. (Henry's law constant of CO_(2) is 1.67 K bar at 298 K )

Henry's law constant for nitrogen at 20^@C is 76.48 k bar. Assuming the partial pressure as 0.987 bar, calculate mass of nitrogen dissovled in one litre water at 20^@C .