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I received a few questions about the ICE table problems I did at the
end of lecture,<br>
particularly the one where I ignored the "x". I've added two links
to the "Notes"<br>
link on my web page. The first three links go along with what we
covered on<br>
Thursday.<br>
<br>
The first link shows why when you add reactions to get another
reaction you<br>
multiply the equil. constants. This was an existing link.<br>
<br>
<a
href="https://www.asc.ohio-state.edu/zellmer.1/chem1220/notes/ch15_adding_eqns_K.pdf"><b>Chapter
15 - Chem. Equil. - Equil. Constant when Adding Eqns - Proof</b></a><br>
<br>
The 2nd link is the first example I did where I ignored the "x".
I've made a video<br>
using my notes working through the example while explaining things.
There's<br>
three pages. This is a new link.<br>
<br>
<a
href="https://www.asc.ohio-state.edu/zellmer.1/chem1220/notes/ch15_ice_notes_ex1/ice_ex1_video.htm"><b>Chapter
15 - Chem. Equil. - ICE Table Example 1 from Notes </b></a><br>
<br>
The 3rd link is the second example I did where the reaction was
going in the<br>
reverse direction, with the "-" signs on the right-hand side of the
ICE table.<br>
I did it both ways, going right to left and then reversing it and
going left to<br>
right. You'll see you get the same answer doing it either way.<br>
<br>
<a
href="https://www.asc.ohio-state.edu/zellmer.1/chem1220/notes/ch15_ice_notes_ex2.pdf"><b>Chapter
15 - Chem. Equil. - ICE Table Example 2 from Notes</b></a><br>
<br>
We haven't covered the material for the 4th link yet.<br>
<br>
Dr. Zellmer<br>
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