## Partial Pressure

Kennedi2J
Posts: 101
Joined: Wed Sep 18, 2019 12:20 am

### Partial Pressure

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

KDang_1D
Posts: 127
Joined: Fri Aug 30, 2019 12:15 am
Been upvoted: 1 time

### Re: Partial Pressure

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
Posts: 99
Joined: Thu Jul 25, 2019 12:17 am

### Re: Partial Pressure

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
Posts: 132
Joined: Thu Jul 11, 2019 12:15 am

### Re: Partial Pressure

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

Jaci Glassick 2G
Posts: 104
Joined: Sat Jul 20, 2019 12:16 am

### Re: Partial Pressure

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