The relationship between the solubility of a gas and its pressure is a linear one, and can be described by Henry's law.
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As you increase the pressure of a gas, the collision frequency increases and thus the solubility goes up, as you decrease the pressure, the solubility goes down..
Would this mean that in a closed system a substance with a lower boiling point and higher vapor pressure would have an increased solubility
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When a gas phase molecule hits the surface of a liquid it may be deflected back into the gas or dissolved into the solution, in the latter case becoming a solute particle. If a dissolved molecule reaches the surface of the liquid, a fraction will have enough kinetic energy to escape, and so particles are being exchanged across the liquid/gas boundary all the time. When the rate at which the gas phase particles enter and leave are equal you have a dynamic equilibrium, where the concentration in each phase becomes a constant value. The solubility is a measure of the concentration of the dissolved gas particles in the liquid and is a function of the gas pressure. As you increase the pressure of a gas, the collision frequency increases and thus the solubility goes up, as you decrease the pressure, the solubility goes down..
Discribes areas effect on pressure, and shows how increasing pressure effects solubility
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Step 1: Separate particles of the solute from each other Step 2: Separate particles of the solvent from each other Step 3: Combine separated solute and solvent particles to make solution
Process of salvation
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Grams Solute per 100 g H2O (S)
This might be a stupid question but isn't this just percent by weight? How is this special in any way?
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For example, we used the concept of mole fraction to describe the partial pressure of a gas, where the partial pressure was the mole fraction times the total pressure, but that told you nothing about how close the molecules were to each other
I don't think I understand the mole fractions use, I assumed it would describe the moles of a substance compared to the other moles within a solution or compound. How exactly is this related to pressure?
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saturated solution it does not dissolve, typically falling to the bottom as a precipitate
I thought a percipient was caused when two valuable compounds form an insoluble solid within an aquias solution. Is a percipient any sold within an aquias solution?
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Phase diagram of
What is a metast liquid
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Figure 12.7
I think I am understanding the reason behind why a substance can only be gas or solid at low temperatures but I wanted to confirm with you. Due to the low temperatures they cant move or interact as normal so their particles are reliant on the pressure which is either pulling them apart with a vacuum so drastically that they become a gas or putting them under so much pressure that they get forced together to take up ass little room as possible.
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- Jan 2026
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Practice
on question 2 how do these numbers relate to the well.I understand the repulsion between nuclei and the attraction of electrons and nuclei and how this relates to equilibrium, but I do not understand how the numbers relate back to the model
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Intermolecular Force" is a misnomer, even though it is commonly used, as these are the forces between ions with molecules possessing a dipole moment, and ions do not have to be molecular
Do molecules always have to be multiple ions/atoms? Can a single atom ever be considered a molecule?
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Figure 11.2.1
What is the significance of the double ended arrow and the n above figure 11.2.1?
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