【Daily Question】Chemical Engineering Principles 543: Henry’s Law (March 31)
Thread Content
The Chemical Engineering Theory section is launching the \"One Question per Day\" campaign starting today, aimed at helping everyone reinforce their basic knowledge in chemical engineering. Subsequent series will include those on \"Principles of Chemical Engineering,\" \"Mass Transfer and Separation,\" \"Thermodynamics in Chemical Engineering,\" and \"Chemical Process Engineering.\" We hope for your active support~~~ Replies to the \"One Question per Day\" campaign can be viewed directly at **; the topic will be closed after 1 day! ! To encourage continued participation from everyone this year! You get 3 wealth rewards just for participating, and an additional 4 wealth points for correct answers~~~ Short answer question: What is the definition of Henry’s law? At a temperature where the total pressure is not too high, it is the relationship between the equilibrium partial pressure of the solute component above a dilute solution and its concentration in the liquid phase.
In a sealed container at a constant temperature, the partial pressure of a gas is proportional to its molar concentration 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.
For non-ideal solutions, the deviation from Raoult’s law is significant; however, at low solution concentrations it can be concluded that when the concentration is below a certain value, the equilibrium pressure of the solute is proportional to its molar fraction in the solution. This is Henry’s law: Pe = HX.
That is, when the solution concentration is below a certain value, the equilibrium pressure of the solute is proportional to its molar fraction in the solution; this is Henry’s law: Pe = HX.
The mole fraction of a substance in a solution is directly proportional to its partial pressure in the gas phase.
At a certain temperature, the solubility of a gas in a liquid is proportional to its equilibrium partial pressure.
At a certain temperature, the solubility of a gas in a liquid is proportional to its equilibrium partial pressure.
At a certain temperature, the solubility of a gas in a liquid is proportional to its equilibrium partial pressure.
At a certain temperature, the solubility of a gas in a liquid is proportional to its equilibrium partial pressure.
At a certain temperature, the solubility of a gas in a liquid is proportional to its equilibrium partial pressure.