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State Henry’s law and mention some important applications.
By BYJU'S Exam Prep
Updated on: September 25th, 2023
Henry’s law states that the solubility of the gas is directly proportional to the pressure of the gas at a constant temperature. It is used in soft drink bottles to increase solubility and deep sea drivers with less soluble Helium gas. According to Henry’s law, a gas’s solubility at a given temperature is exactly proportional to its pressure.
This implies that the gas is more soluble the higher the gas pressure increases. Additionally, if the gas has low pressure, we can infer that it is less or not soluble. The mathematical form is P = KH x x, where P = the partial pressure of the gas, KH = Henry’s constant, and x = mole fraction of the gas.
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Applications of Henry’s Law
- Soft drink bottles are sealed under high pressure to increase the solubility of carbon dioxide (CO2).
- This is why when we open a bottle of soft drink, some gas escapes.
- Less soluble Helium gas is used to spread the oxygen that is given to deep sea divers.
- This is done to lessen the unpleasant effects of the greater levels of soluble Nitrogen (N2) gas in the blood.
Summary:
State Henry’s law and mention some important applications.
According to Henry’s law, a gas’s solubility at a given temperature is exactly proportional to its pressure. With less soluble Helium gas, it is employed in deep sea drives and soft drink bottles to boost solubility.
