Why does gas solubility increase at higher pressure?
From Henry's law (at least, this version),
where:
That mathematically tells you that the solubility increases in the solution for higher pressures.
A more conceptual way of explaining this is that higher pressures means greater force of collision between gas particles above the solution (pressure is force per unit area). Therefore, their average kinetic energy is greater, and their average speeds are greater.
As a result, they are more likely to knock some of the particles down into the solution, thereby dissolving them.
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Gas solubility increases at higher pressure due to the increase in the number of gas molecules that can dissolve in the solvent. This is because higher pressure forces more gas molecules into the solvent, leading to a higher concentration of dissolved gas particles.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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