Temperature Dependence of Henry's Law Constant

chemical species

acetylene

Henry's law was originally formulated by William Henry in 1803. This law describes the solubility of gases in liquids. Henry's law states that at constant temperature, the mole fraction of a given gas dissolved in the liquid

x

is directly proportional to the partial pressure of that gas (i.e.,

Py=Hx

, where

P

is the total pressure,

H

is the Henry's law constant, and

y

is the vapor-phase mole fraction).

The constant in Henry's law changes with the system's temperature

T

. This is why it is preferable to name it Henry's coefficient. Multiple equations take into account the effect of temperature on this constant. Here, the following relationship is adopted[1]:

H=1/exp(A+B/T+Cln(T)+DT)

, where

T

is in Kelvin, and

A

,

B

,

C

, and

D

are constants that depend on the chemical species considered.

The present Demonstration plots

H(T)

for different gaseous species in water (

H

is expressed in atm).

References

[1] R. H. Perry, Perry’s Chemical Engineers’ Handbook, 4th ed., New York: McGraw–Hill, 1963.

Permanent Citation

Housam Binous, Ahmed Bellagi

"Temperature Dependence of Henry's Law Constant"
http://demonstrations.wolfram.com/TemperatureDependenceOfHenrysLawConstant/
Wolfram Demonstrations Project
Published: June 9, 2015