## Help on 11.9: b and c

Joanna Pham - 2D
Posts: 113
Joined: Fri Apr 06, 2018 11:04 am

### Help on 11.9: b and c

For this question, we are asked to balance then write the equilibrium expression Kc for the reactions

For part b, the equation is $I_2 (g) + F_2 (g) -> IF_5$. I balanced the equation and got $I_2 (g) + 5F_2 (g) -> 2IF_5$. Then I used the equation in the book, $K = (RT)^(\Delta n_R)(Kc)$, inputted the corresponding elements and solved for Kc. I got
$K_C = (RT)^4([IF_5]^2 / [I_2][F_2]^5))$ for my answer, but in the back of the book, there's no (RT)^4 in front. Everything else was correct, but I am unsure why there's no RT in the answer. Is there another way I am supposed to solve this?

Thanks!

Neil Hsu 2A
Posts: 61
Joined: Fri Sep 28, 2018 12:16 am

### Re: Help on 11.9: b and c

I'm not sure where that equation came from, but I would just find the equilibrium expressions like how Lavelle taught us in class. Given a hypothetical chemical reaction aA + bB--> cC + dD, the equilibrium constant Kc = ([C]^c [D]^d) / ([A]^a [B]^b), or simply just Kc = [products] / [reactants]. So in the case of this question, you balanced the equation right, and Kc should equal [IF5]^2 / ( [F2]^5 [I2]).

Laura Gong 3H
Posts: 89
Joined: Fri Sep 28, 2018 12:26 am
Been upvoted: 1 time

### Re: Help on 11.9: b and c

When the question asks you to write the Kc expression, it is just looking for the form, Kc=[P]/[R].
The equation K=KcRT^delta(n) is the equation used to convert Kc to Kp (or the equilibrium constant using partial pressures).
For some reason, it appears the textbook does not include the subscript p.

kamalkolluri
Posts: 65
Joined: Fri Sep 28, 2018 12:17 am
Been upvoted: 1 time

### Re: Help on 11.9: b and c

I think we just need to use the general Kp and Kc. You don't need the complex equation, I'm pretty sure that's for later.

Kayla Vo 1B
Posts: 60
Joined: Fri Sep 28, 2018 12:26 am

### Re: Help on 11.9: b and c

That equation from the book is used when you want to write Kp in terms of Kc. For this problem you can just use the formula given in lecture to find the equilibrium constant.