## Using PV=nRT

$PV=nRT$

Erik Buetow 1F
Posts: 96
Joined: Fri Aug 30, 2019 12:15 am

### Using PV=nRT

Will we need to use this equation for test 1? And if so, will we only use it to find pressure or concentration for the equilibrium equation?

Isabella Dal Porto 1H
Posts: 100
Joined: Fri Aug 30, 2019 12:16 am

### Re: Using PV=nRT

This equation will most likely show up on the test. It is used for finding the equilibrium pressure of a gas.

Kaylee Sepulveda 4G
Posts: 100
Joined: Thu Jul 11, 2019 12:16 am

### Re: Using PV=nRT

Everything that we have covered so far is fair game, so I would not be surprised if at least one question required this formula. However, if I remember correctly, it is on the equation sheet.

Jacey Yang 1F
Posts: 101
Joined: Fri Aug 09, 2019 12:17 am

### Re: Using PV=nRT

Yes, you would use the equation to convert between concentration and partial pressure, depending on what the problem asks for.

JesseAuLec1Dis1G
Posts: 52
Joined: Mon Jun 17, 2019 7:23 am

### Re: Using PV=nRT

You would need to use this equation if you needed to convert mols to pressure.

Martina
Posts: 111
Joined: Thu Jul 25, 2019 12:16 am

### Re: Using PV=nRT

Yes you can use it find find pressure if you have the molarity (n/V) or vice versa.

005206171
Posts: 107
Joined: Wed Sep 18, 2019 12:20 am

### Re: Using PV=nRT

If it does, it will be in the context of converting partial pressure to concentration or vice versa

Aarushi Solanki 4F
Posts: 107
Joined: Sat Jul 20, 2019 12:17 am

### Re: Using PV=nRT

It is on the equation sheet but you should understand the reasoning behind the derivation of this equation.