## PV=nRT

$PV=nRT$

Alison Trinh 1E
Posts: 104
Joined: Thu Jul 25, 2019 12:16 am

### PV=nRT

When would we use this equation in relation to chemical equilibrium?

805383532
Posts: 53
Joined: Thu Jul 11, 2019 12:16 am

### Re: PV=nRT

It could possibly be used to find the partial pressure of a molecule if you are looking for Kp.

Jielena_Bragasin2G
Posts: 104
Joined: Sat Aug 24, 2019 12:18 am
Been upvoted: 1 time

### Re: PV=nRT

n/V is concentration, therefore this equation can also be seen as P=(concentration)RT or P/RT=(concentration). This allows us to convert from concentration to pressure or pressure to concentration in case a problem gives us some equilibrium information as pressure or some as concentration.

Manav Govil 1B
Posts: 104
Joined: Sat Sep 07, 2019 12:19 am

### Re: PV=nRT

We can use the equation to relate the values before and after the reaction, like comparing pressure, volume, and concentration.

Dan M -3E
Posts: 101
Joined: Wed Sep 18, 2019 12:19 am

### Re: PV=nRT

I think the most important way we can use this formula in this class is to convert between partial pressure and concentration when we need to. Other than that it is used more for physics than chemistry.

Eesha Sohail 1D
Posts: 100
Joined: Sat Aug 17, 2019 12:16 am

### Re: PV=nRT

As far as I've seen, the ideal gas law is taught in high school chemistry classes more than physics classes, but that's a bit of a moot point. That said, could we possibly use other variants of the law to figure things out as well, such as P(mm) = dRT (where mm = molar mass and d = density)?

kendal mccarthy
Posts: 109
Joined: Wed Nov 14, 2018 12:22 am

### Re: PV=nRT

you can use this equation to gain information such as converting from concentration to pressure and vice versa.

SVajragiri_1C
Posts: 115
Joined: Thu Jul 11, 2019 12:16 am

### Re: PV=nRT

You can use this equation to find partial pressures of the components of the reaction (P) if you know the volume, temperature and molar concentration. Then you could find the equilibrium constant Kp by plugging in the partial pressures into the formula for Kp.

Ian Morris 3C
Posts: 101
Joined: Wed Sep 18, 2019 12:18 am

### Re: PV=nRT

In this class, we will mainly focus on the use of PV=nRT to find concentration or pressure.

saigorijavolu2k
Posts: 108
Joined: Sat Sep 28, 2019 12:15 am

### Re: PV=nRT

If we are tested on this, we will be asked to find the pressure or even concentration and from there calculate the equilibrium constant.

Angela Wu-2H
Posts: 50
Joined: Fri Aug 30, 2019 12:16 am

### Re: PV=nRT

You can use the ideal gas law (PV=nRT) with concentration as well because Molarity is mol/liter, which is also what n/v is (if you divide V over to the right side).

PV=nRT --> P= (n/v)RT

ValerieChavarin 4F
Posts: 99
Joined: Wed Sep 18, 2019 12:18 am

### Re: PV=nRT

This in relation to concentration (n/V). It's used mainly to calculate for the unknown variable.

Jasmine Vallarta 2L
Posts: 102
Joined: Sat Aug 17, 2019 12:18 am

### Re: PV=nRT

P = (n/V)RT = (concentration)RT

Gurmukhi Bevli 4G
Posts: 49
Joined: Wed Nov 14, 2018 12:20 am

### Re: PV=nRT

It can be used to convert between partial pressure and concentration, since n/v (mol/L) is equal to concentration, for pv=nRT, n/v=P/RT.