Partial Pressure

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Partial Pressure

Postby Kennedi2J » Sun Jan 19, 2020 11:23 pm

For test 1, will we need to know how to calculate the partial pressure of a gas if it isn't given?

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Re: Partial Pressure

Postby KDang_1D » Sun Jan 19, 2020 11:30 pm

Dr. Lavelle went over it in lecture, so I believe it would be a fair question.

You would need to apply the ideal gas equation: PV=nRT. Divide V over to get P = (n/V)RT. (n/V) is concentration, which should be given, and RT are constant so just solve for P, your partial pressure

Rohit Ghosh 4F
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Re: Partial Pressure

Postby Rohit Ghosh 4F » Thu Jan 23, 2020 12:33 pm

Although the ideal gas equation isn't completely right for modeling gases in the real world it is useful for introductory chemistry.

Kishan Shah 2G
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Re: Partial Pressure

Postby Kishan Shah 2G » Thu Jan 23, 2020 9:07 pm

A very simple way to convert from concentration to pressure is (Pressure = Concentration * RT)

Jaci Glassick 2G
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Re: Partial Pressure

Postby Jaci Glassick 2G » Thu Jan 23, 2020 9:10 pm

You would have to use the ideal gas law (PV=nRT) to calculate P using the other given values.

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