Henry's Law for Oxygen and Carbon Dioxide

volume (L)

0

moles

0

solute

O

2

CO

2

liquid volume (L)	vapor pressure (atm)	solubility (mol solute/L solution)	moles in solution	mass dissolved (g)
0.	0.	0.	0.	0.

key
	molecular weight (g/mol)	boiling point (K)	temperature (K)
solute: carbon dioxide	44.	194.5	298
solute: oxygen	32.	90.	298
solvent: water	18.	373	298

This Demonstration considers the solubility of two different gases,

CO

2

and

O

2

, in water. The "volume (L)" slider changes the amount of water in the cylinder, while the "moles" slider changes the number of moles of gas in the cylinder, roughly modeled by the number of blue spheres. By Henry's law,

s

, the solubility of a gas, is proportional to

P

, its partial pressure above the solution:

s=

K

H

P

. At 298 K, the Henry's law constant

K

H

equals

1.317×

-3

10

mol/Latm

for

O

2

and

3.344×

-2

10

mol/Latm

for

CO

2

.