00:01
So let's say we want to get the reaction below by summing up two other chemical reactions.
00:09
Well, if we know those reactions and how we can add them together or multiply values or flip their equations in order to get the reaction at the bottom, we can then figure out what happens to their equilibrium constants to find the equilibrium constant of this reaction shown on the screen.
00:28
So from two chemical reactions to get this reaction at the bottom, we could have two ch4s in equilibrium with c2h6 and h2.
00:50
And we can find that the equilibrium constant for this reaction is 9 .5 times 10 to the minus 13.
01:04
Now, if we had a second equation, and if we had that equation where ch4 and water are in equilibrium with ch3oh and h2, if we reverse that reaction and multiply it by two, we would get 2ch3oh plus 2h2 is in equilibrium with 2c8.
01:44
H4 and 2h2o.
01:54
Now, if we were told that that original equilibrium constant was 2 .8 times 10 to the minus 21, when we flip the reaction, we have to wind up flipping the equilibrium constant.
02:13
We have to, instead of an irregular he has as low where we would make it negative, here, remember, when we reverse a reaction, the products become the reactants and the reactants become the products.
02:26
So it would be the reciprocal of that equilibrium constant.
02:32
And then we also wind up squaring it.
02:35
So our new equilibrium constant here is going to be one over our 2 .8 times 10 to the minus 21, which was the original equilibrium.
02:50
Equilibrium constant.
02:52
It's inverse because we flip the reaction...