Henry’s law states that the mass of a gas dissolving in a liquid is proportional to the pressure exerted on the gas, and inversely proportional to temperature. It is used to explain the behavior of gas in everyday objects, such as soft drinks, and in diving, where it can cause decompression sickness.
In the science of chemistry, Henry’s law is a gas law which states that the mass of a gas dissolving within a certain amount of liquid is equally proportional to the pressure exerted on the gas. Simply put, the higher the pressure, the more gas can dissolve and merge into the liquid. Henry’s gas law also states that the solubility of a gas is inversely proportional to the temperature. If there is an increase in temperature, the solubility of the gas decreases.
The establishment of Henry’s law is attributed to William Henry, who in 1800 experimented with the gases contained in water, using different temperatures and pressures. In formulaic terms, the gas law can be summarized as follows: p = khc, where “p” represents the partial pressure of the gas, and c is the concentration of the solute. The kh is the constant variable, depending on which gas is being analyzed. The formula can also be expressed in other inverse forms, such as kh,pc = p/c or kh,cp = c/p.
Henry’s law principle is most easily understood when applied in everyday objects, such as soft drinks, when the element of pressure is concerned. You may notice that a carbonated drink sizzles and bubbles when you remove the bottle cap and release the pressure, evidence that carbon gas is also being released. If the bottle cap remains on, the pressure inside somehow forces and presses on the carbon to dissolve into the sugary liquid, demonstrating that more pressure causes the gas to dissolve. This is why soft drinks don’t taste as delicious when they’re exposed to the air for too long, as a lot of carbon has already been released.
Henry’s Law can also be experienced by divers who usually feel heavier the further they descend into deeper water. This is because nitrogen is absorbed more by body tissues due to increased pressure under water. When divers swim, they experience a lighter sensation due to the release of gas, a very similar occurrence of carbons coming out of soda. Divers are advised, however, not to surface too quickly, as this can lead to decompression sickness, in which gases are released throughout the body and can cause severe pain, inflammation and even seizures.
The element of temperature in Henry’s law can also be seen in carbonated drinks, or any gas-containing liquid, for that matter. As mentioned earlier, the solubility of gas decreases with increasing temperature, as seen when water boils and gas bubbles form at the surface. This also explains why experienced divers do not immerse themselves in a hot bath immediately after the dive, because warm water produces less soluble nitrogen which is detached from the body, causing decompression sickness.
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