Converting concentration to partial pressure  [ENDORSED]


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abby hyman
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Joined: Thu Jul 25, 2019 12:16 am

Converting concentration to partial pressure

Postby abby hyman » Mon Jan 04, 2021 2:10 pm

Can someone explain to me how you would be able to figure out the partial pressure of a gas if you are not given the temperature?

Marley Magee 3A
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Re: Converting concentration to partial pressure

Postby Marley Magee 3A » Mon Jan 04, 2021 2:18 pm

The only way we have been shown to convert between concentration and partial pressure in class is using PV=nRT. So if you don't have temperature, based on what we know for this class so far, I don't think you can find partial pressure. But maybe it'll be covered in class later!

Chem_Mod
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Re: Converting concentration to partial pressure  [ENDORSED]

Postby Chem_Mod » Mon Jan 04, 2021 2:25 pm

In Wednesday's class I'll cover this.

Karl Yost 1L
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Re: Converting concentration to partial pressure

Postby Karl Yost 1L » Mon Jan 04, 2021 10:29 pm

The total pressure of a system is the sum of all of the partial pressures. If you want to find the partial pressure of a specific gas within the system, you multiply the total pressure (exerted by all of the gases) by the mole fraction of the specific gas whose partial pressure you want to calculate. To find the mole fraction of a given gas, you divide the moles of the given gas by the total number of moles in the system.


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