Fundamentals of Purification (9)
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What is the specific content of Henry’s law? At a certain temperature, when the gas and liquid phases are in equilibrium, the molar fraction XA of the soluble gas in the liquid phase is proportional to its equilibrium partial pressure PA in the gas phase; this is Henry’s law. That is, PA = E × XA. Here, XA is the molar fraction of the solute in the liquid phase, PA is the equilibrium partial pressure of the solute in the gas phase, and E is a proportionality constant known as the Henry coefficient.
At a certain temperature, when the gas and liquid phases are in equilibrium, the molar fraction XA of the soluble gas in the liquid phase is proportional to its equilibrium partial pressure PA in the gas phase; this is Henry’s law. That is, PA = E × XA. Here, XA is the molar fraction of the solute in the liquid phase, PA is the equilibrium partial pressure of the solute in the gas phase, and E is a proportionality constant known as the Henry coefficient.
Henry’s law is one of the fundamental laws in physical chemistry; it states that \"in a sealed container at a constant temperature, the partial pressure of a gas is directly proportional to its molar concentration in the solution.\"
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Henry’s law states that, at a constant temperature and when there is equilibrium between a liquid and a gas, the amount of gas dissolved per unit volume is proportional to the partial pressure of that gas above the liquid surface. If the partial pressure of a certain gas above the water surface can be reduced to zero, thereby eliminating that gas from the water surface entirely, then that gas dissolved in the water can also be completely removed.
At a constant temperature, when the gas and liquid phases are in equilibrium, the molar fraction XA of the soluble gas in the liquid phase is proportional to its equilibrium partial pressure PA in the gas phase; this is Henry’s law. That is, PA = E × XA. Here, XA refers to the molar fraction of the solute in the liquid phase, PA refers to the equilibrium partial pressure of the solute in the gas phase, and E is a proportionality constant known as the Henry coefficient.
At a certain temperature, when the gas and liquid phases are in equilibrium, the molar fraction XA of the soluble gas in the liquid phase is proportional to its equilibrium partial pressure PA in the gas phase; this is Henry’s law. That is, PA = E × XA. Here, XA refers to the molar fraction of the solute in the liquid phase, PA refers to the equilibrium partial pressure of the solute in the gas phase, and E is a proportionality constant known as the Henry coefficient.
At a certain temperature, when the gas and liquid phases are in equilibrium, the molar fraction XA of the soluble gas in the liquid phase is proportional to its equilibrium partial pressure PA in the gas phase; this is Henry’s law. That is, PA = E × XA. Here, XA refers to the molar fraction of the solute in the liquid phase, PA refers to the equilibrium partial pressure of the solute in the gas phase, and E refers to the proportionality constant.
“At a certain temperature and pressure, the solubility of a gas in a liquid is proportional to its equilibrium pressure. This law applies under the conditions that the equilibrium partial pressure of the gas is not high, and the gas does not react with the solvent in the solution (or it may react to a small extent, but with very little ionization). The amount of gas dissolved can be expressed in terms of different concentrations. The mathematical expression for Henry’s law can take the following forms: PB = kB(x)xB, PB = kB(m)mB, PB = kB(c)cB. Here, xB is the mole fraction of solute B; mB is the mass molar concentration of solute B, with units of mol·kg-1; cB is the molar concentration of solute B, with units of mol·dm-3. KB(x), KB(m), and KB(c) are all referred to as Henry’s constants, and they are related to each other as follows: ρ is the density of the solution, and Mr(A) is the relative molecular mass of solvent A. The Henry constant can also be expressed in terms of the volume of gas dissolved per unit volume.
At a constant temperature, when the gas and liquid phases are in equilibrium, the molar fraction XA of the soluble gas in the liquid phase is proportional to its equilibrium partial pressure PA in the gas phase; this is Henry’s law. That is, PA = E × XA. Here, XA refers to the molar fraction of the solute in the liquid phase, PA refers to the equilibrium partial pressure of the solute in the gas phase, and E is a proportionality constant known as the Henry coefficient.
Henry’s law, one of the fundamental laws in physical chemistry, was discovered by the British scientist Henry in 1803 while studying the laws governing the solubility of gases in liquids. It can be expressed as follows: \"Under constant temperature and pressure, the solubility of a volatile solute (usually a gas) in a solution is proportional to the equilibrium pressure of that solute above the liquid surface.\" ”Its formula is Pg = Hx, where H is the Henry constant, x is the molar fraction of solubility of the gas, and Pg is the partial pressure of the gas. H can effectively represent the amount of gas dissolved, but Henry’s law is only applicable to systems with very low solubility. Strictly speaking, Henry’s law is merely an approximate rule and cannot be used in systems under high pressure. In this sense, the Henry constant is merely a function of temperature and is independent of pressure.