Henry's law constant of oxygen is `1.4 xx 10^(-3)` mol `"lit"^(-1) "atm"^(-1)` at 298 K. How much of oxygen is dissolved in 100 mL at 298 K when the partial pressure of oxygen is 0.5 atm?

Henry's law constant of oxygen 1.4xx10^-3 molL^-1 atm^-1 at 298K. How much of oxygen is dissolved in 100 mL at 298K when partial pressure of oxygen is 0.5 atm?

The Henry's Law constant for oxygen dissolved in water is 4.34 xx 10 ^(4)atm ( mol /L) at 25^(@) C . If the partial pressure of oxygen in air is 0.2 atm under ordinary atmospheric condition calculate the concentration (in mol/litre ) of dissolved oxygen in water equilibrium with air at 25^(@) C

Henry's law constant for CO_2 in water is 1.67xx10^(-8) Pa at 298 K. Calcuated the quantity of CO_2 in 500 mL of soda water when paked under 2.5 atm CO_2 pressure at 298K.

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

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

Henry law constant for oxygen dissolved in water is 4.34 xx 10^(4) atm at 25^(@) C . If the partial pressure of oxygen in air is 0.4 atm.Calculate the concentration ( in moles per litre) of the dissolved oxygen in equilbrium with air at 25^@C .

Henry law constant for oxygen dissolved in water is 4.34 xx 10^(4) atm at 25^(@) C . If the partial pressure of oxygen in air is 0.4 atm.Calculate the concentration ( in moles per litre) of the dissolved oxygen in equilbrium with air at 25^@C .