Why does the Equilibrium Law multiply the concentrations of products and reactants raised to the coefficient instead of just adding them?

For example, let’s say there’s a reaction aA + bB <–> cC + dD.

Why do they use this:



Instead of this much simpler and far more meaningful ratio:

c[C] + d[D]

a[A] + b[b]

To find an equilibrium constant? It seems pretty stupid to use the first ratio, so there has to be a very convincing reason to do it.

I think I’ve figured it out anyway. THANKS PIERSON.

No problem!

<.< >.> <.< FREE POST!!


They both are.

The second equation also happens to be a ratio of the forward and reverse rate constants though, so it’s more useful. I guess it’s also easier to cancel out the concentrations of solids and liquids, since they have no effect on equilibrium anyway.

LMAO! Best emoticon ever.
makes it AIM buddy icon

Pierson wins this thread.

I can’t see it. :frowning:

Okay, I’m pretty sure we made this clear a while ago, but I guess some people don’t understand the concept of not making idiotic free posts. If you want to enlarge your post count, at least take the four seconds to think of something else to write. God damn.

I don’t give a fuck who makes the thread, if someone asks a question like this, if you have nothing to add except banal, assinine useless spam to the thread, shut the fuck up. Jesus fucking christ.