How to Leverage off Henry’s Law to Get the Information You Are Looking for – Part 1

Henry's law, a gas law, states that the amount of dissolved gas in a liquid is directly proportional at equilibrium to its partial pressure above the liquid.


The depth-dependent dissolution of Oxygen and Nitrogen in the blood of underwater divers which changes during decompression, possibly causing decompression sickness if the decompression occurs too fast, is an application of Henry’s law.

Once the bottle of a carbonated soft drink is opened, almost pure Carbon dioxide above the liquid in the container at a pressure higher than the atmospheric pressure escapes decreasing the pressure above the liquid, resulting in fast degassing as the dissolved gas is liberated from the solution. This is an everyday example of Henry’s law.

Question:

KH values for some gases at the same temperature are given:

Gas

KH/k bar

Ar

40.3

CO2

1.67

HCHO

1.83 x 10-5

CH4

0.413

where KH is Henry’s law constant in water. What is the order of their solubilities in water?

Solution: 



Click/tap to enlarge the image

C = Solubility of a gas in a liquid, P = Partial pressure of the gas above the liquid

Hesitant about the Henry's law related problems❓ Let Chemaficionado know in the comments below or at mychemistryhomework@gmail.com❗

References:

(1)    Wikipedia Contributors. Henry’s law. Wikipedia. https://en.wikipedia.org/wiki/Henry%27s_law.

‌‌(2)    Henry's Law

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