The beginning of chem was fun, because we watched Steven Colbert singing "Friday" for some fundraising thing. And then we talked about weird stuff like farms.
But then we learned. Like scientifical stuff.
First was equilbrium. Basically it occurs when a reaction is going forward at the same rate its reverse reaction is going. So if we have a reaction A --> B, we would reach equilibrium if A's were changing into B's at the same rate that B's were changing into A's. Thus we can determine, that once we reach equilibrium, the total number of A's and B's, or their concentration, will not change, though they may not necessarily be equal.
Ok. so that was easy.
This part is shaky for me.
So for the equation: aA + bB < - > cC + dD, where the little letters are coefficients and the big letters are gases, we can get this equation:
Ok, so that's kinda not really simple. why is my font bigger. Ok, now it's too small. That bothers me.
So the PA-D 's represent the pressures of each of the gases. Then they are raised to the power of their respective coefficients. And from there it's pretty straight forward.
We also get this other equation:
Kc = [C]c[D]d/[A]a[B]b
The brackets here around the letters mean "the concentration of". So [C] means the concentration of gas C. It is essentially the same equation as before, only we use concentration instead of pressure.
Now we have an equilibrium pressure constant, and an equilibrium concentration constant, so now we relate them with yet another equation.
Kp = Kc(RT)^∆n
These should be familiar, we have the constants and the universal gas constant (.0821 L*atm/mol*K) and the change in moles of gas.
I am pretty sure the moles referred to is the total number of moles (moles of products - moles of reactants) but I could be wrong).
We have a WA due tomorrow. So get some sleep. and do it during lunch. and watch this:
Umm scribing tomorrow will be.. MOLLIE McAWESOME
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