## When to use PV=nRT

Shanzey
Posts: 120
Joined: Wed Sep 18, 2019 12:20 am

### When to use PV=nRT

How do we know when to use the PV=nRT equation? Do we just use it to calculate initial concentration for pressure before creating our ICE table? Were there any homework questions that showed us an example of when/how to use it? Also, do the units for pressure (bars vs. atm) matter when using this equation, or can we use either?

Ariana Iranmahboub1G
Posts: 114
Joined: Fri Aug 09, 2019 12:17 am

### Re: When to use PV=nRT

It’s often used to convert partial pressure to the molarity or vice versa. It can also be used to understand the effect volume, moles, and temperature will be affected by a change in pressure. In terms of whether to use arm or bar, you units should be the same units you are using for your R constant.
Last edited by Ariana Iranmahboub1G on Sun Jan 19, 2020 10:18 pm, edited 1 time in total.

Janet Nguy 2C
Posts: 115
Joined: Sat Aug 24, 2019 12:17 am

### Re: When to use PV=nRT

pV = nRT is used to convert between concentrations and partial pressures. Basically it means that you can express K for gases as either their molar concentrations or their partial pressures.

CalvinTNguyen2D
Posts: 102
Joined: Thu Jul 25, 2019 12:16 am

### Re: When to use PV=nRT

Ideal gas law is used to convert individual concentrations into partial pressures, and vise-versa. It's useful for expressing K in either Kc (concentration) or Kp (partial pressure).

Kimberly Koo 2I
Posts: 99
Joined: Sat Aug 17, 2019 12:17 am

### Re: When to use PV=nRT

Since PV=nRT can be converted into the equation P=(n/V)RT and R is a constant, we can convert from partial pressures to concentration to find K and vice versa

Ruth Glauber 1C
Posts: 100
Joined: Wed Sep 18, 2019 12:20 am

### Re: When to use PV=nRT

Does anyone have an example they could walk through?