## 5J.13 and Ideal Gas Law

$PV=nRT$

Alice Chang 2H
Posts: 101
Joined: Fri Aug 30, 2019 12:18 am

### 5J.13 and Ideal Gas Law

I'm having a bit of trouble trying to figure problem 5J.13 out. I'm trying to work backwards with the given answer for this question, but I'm still getting stuck.

In the problem, the concentration can be worked out, and the temperature is given, so the partial pressures (?) of each molecule can be worked out (or at least I'm assuming by the given units of bar). Yet when I use P=(n/V)RT, I still can't get the numbers the answer got for the conversion from concentration to bars. What am I doing wrong? Am I using the wrong formula?

Daniel Honeychurch1C
Posts: 109
Joined: Thu Jul 11, 2019 12:15 am

### Re: 5J.13 and Ideal Gas Law

You don't need to do any calculations, just look at the equilibrium constants for 600 K and 700 K. The Keq is smaller at the higher temperature, so increasing the temperature will increase the concentration of the reactants. Therefore, the concentration of NH3 will decrease.

cassidysong 1K
Posts: 100
Joined: Fri Aug 30, 2019 12:15 am

### Re: 5J.13 and Ideal Gas Law

There is no need to calculate anything; just compare the two different K values.

Posts: 97
Joined: Wed Sep 30, 2020 9:36 pm

### Re: 5J.13 and Ideal Gas Law

Yes, you don’t have to calculate anything in this problem. All you have to do is look at the two K values and use Le Chatelier’s Principle. When the equilibrium mixture is heated, the K value decreases, so that means there’s more reactants than products and there will be less ammonia present since it’s a product.

Natalie Do 3F
Posts: 114
Joined: Wed Sep 30, 2020 10:03 pm

### Re: 5J.13 and Ideal Gas Law

Raising temperature favors reactants
This means there will be less ammonia at higher temperatures

All of this is assuming no other changes are occurring