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 1.67xx10^(8) Pa at 298 K . Calculate the quantity of CO_(2) in 500mL of soda water when packed under 2.5atm CO_(2) pressure at 298 K .

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 ]

henry's law constant for CO_(2) in water is 2.5xx10^(8) Pa at 298K calcualte mmole of CO_(2) dissolbed in 144 g water at 2.5 atm pressure at 298K. [take 1 atm =10^(6)(N)/(m^(2)) or Pa]

Henry's law constant of CO_2 in water at 298K is 5/3K bar. IF pressure of CO_2 is 0.01 bar, find its mole fraction.

Henry's law constant for CO_2 in water is 0.835x2x 10^3 bar.How many millimoles of CO_2 would dissolve in 0.9L water? Assume CO_2 gas exerts a partial pressure of 0.853bar

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?