One Question per Day: Methanol Technology Exchange Edition 20180423
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Learn from the advanced practices of the *Brothers section; there are prizes for correct answers – every response earns a reward, allowing us to grow and mature through these Q&A sessions. Brief answer: There are two important laws for studying gas-liquid phase equilibrium, namely Raoult’s law and Henry’s law.
Raoult’s law and Henry’s law are the two most fundamental empirical laws in solutions, both of which describe the proportional relationship between the partial pressure of a component and its concentration. The difference between them is: (1) Raoult’s law applies to the solvent in dilute solutions and to ideal solutions, whereas Henry’s law applies to the solute ； (2) The proportionality constant in Raoult’s law is the vapor pressure of the pure solvent and is independent of the solute, whereas the proportionality constant in Henry’s law is determined experimentally and depends on both the solute and the solvent ； (3) The concentration in Henry’s law can be expressed in various units, as long as the value of k is consistent with that unit, whereas in Raoult’s law the concentration can only be expressed as a mole fraction.
Raoult’s law and Henry’s law are the two most fundamental empirical laws in solutions, both of which describe the proportional relationship between the partial pressure of a component and its concentration. The difference between them is: (1) Raoult’s law applies to the solvent in dilute solutions and to ideal solutions, whereas Henry’s law applies to the solute ； (2) The proportionality constant in Raoult’s law is the vapor pressure of the pure solvent and is independent of the solute, whereas the proportionality constant in Henry’s law is determined experimentally and depends on both the solute and the solvent ； (3) The concentration in Henry’s law can be expressed in various units, as long as the value of k is consistent with that unit, whereas in Raoult’s law the concentration can only be expressed as a mole fraction.
Raoult’s law and Henry’s law are the two most fundamental empirical laws in solutions, both of which describe the proportional relationship between the partial pressure of a component and its concentration. The difference between them is: (1) Raoult’s law applies to the solvent in dilute solutions and to ideal solutions, whereas Henry’s law applies to the solute ； (2) The proportionality constant in Raoult’s law is the vapor pressure of the pure solvent and is independent of the solute, whereas the proportionality constant in Henry’s law is determined experimentally and depends on both the solute and the solvent ； (3) The concentration in Henry’s law can be expressed in various units, as long as the value of k is consistent with that unit, whereas in Raoult’s law the concentration can only be expressed as a mole fraction.
There are two important laws for studying gas-liquid phase equilibrium, namely: Raoult’s law and Henry’s law. (v)
Raoult’s law and Henry’s law are the two most fundamental empirical laws in solutions, both of which describe the proportional relationship between the partial pressure of a component and its concentration. The difference between them is: (1) Raoult’s law applies to the solvent in dilute solutions and to ideal solutions, whereas Henry’s law applies to the solute ； (2) The proportionality constant in Raoult’s law is the vapor pressure of the pure solvent and is independent of the solute, whereas the proportionality constant in Henry’s law is determined experimentally and depends on both the solute and the solvent ； (3) The concentration in Henry’s law can be expressed in various units, as long as the value of k is consistent with that unit, whereas in Raoult’s law the concentration can only be expressed as a mole fraction.