Purification Technology Edition: Daily Question [2017-10-23]
Thread Content
What is the specific content of Henry’s law? Answer: 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 is a proportionality constant known as the Henry coefficient.
At a certain temperature, the equilibrium partial pressure of volatile substances in the gas phase in a dilute solution is proportional to their molar fraction in the solution.
At 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.
Henry’s law: “At constant temperature and pressure, the solubility of a volatile solute (usually a gas) in a solution is directly 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.
At a certain temperature and pressure, the solubility of a gas in a liquid is proportional to its equilibrium pressure
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 constant temperature and pressure, the solubility of a gas in a solution is proportional to the equilibrium pressure of that gas above the liquid surface.
At a constant temperature, the solubility of a gas in a liquid is directly proportional to its partial pressure in the gas phase; this law is known as Henry’s law. Its expression is as follows: P = E • x, where x is the molar fraction of the gas in the liquid phase ； P — vapor pressure of the component at equilibrium ； E — Henry’s constant of the component
In a sealed container at a constant temperature, the partial pressure of a gas is proportional to its molar concentration in the solution
In a sealed container at a constant temperature, the partial pressure of a gas is proportional to its molar concentration in the solution