At 1002 k keq 156e00 for the reactionibrg 12 i2g 12 br2gwhat...

At 1002 K, Keq = 1.56e+00 for the reaction IBr(g) 1/2 I2(g) + 1/2 Br2(g). What is the value of Keq for the reaction I2(g) + Br2(g) 2 IBr(g) at this temperature? a) For the second reaction at this temperature, Keq = 4.09e-01. b) For the second reaction at this temperature, Keq = 8.01e-01. c) For the second reaction at this temperature, Keq = 2.45e+00. d) For the second reaction at this temperature, Keq = 1.25e+00. e) For the second reaction at this temperature, Keq = 6.41e-01.

Transcript

00:01 Hello.

00:02 I've written out the first equation that we have the k4, which is 1 .56.

00:06 And then we have the second one.

00:10 All right.

00:11 Now, the idea here is that we must have done something to the first equation.

00:15 We changed it in some way, and we're trying to find what its k value is too.

00:19 So what we need to do is figure out what's happened.

00:23 And first off, it looks like we flipped the reactants in the products, where we had ibr on the left.

00:31 Hand side in the first one.

00:33 Now it's on the right hand side.

00:36 And the same with the i2 and the br2.

00:38 We have flip flopped.

00:41 So just doing the flip then would have created, let's see, we would have had one half i2 plus one half br2 going to ibr.

00:57 So that's just from flipping the equation backwards.

01:01 Now, when you flip an equation backwards, your equation, your k value in inverts.

01:11 So instead of 1 .56, instead, the k for that is now 1 divided by 1 .56.

01:22 All right.

01:23 And i'm doing this step by step.

01:25 There's going to be one more step we got to do.

01:27 We're not completely finished yet, but this is the first bit as we flip the equation backwards.

01:34 So as of right now, with just having it flip backwards, our k value is 0 .641.

01:43 All right.

01:45 Now we need to look at the equation and see, well, there's something else that was done.

01:51 So look at your numbers for a second...

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