- #1
johndoe3344
- 29
- 0
Homework Statement
Not really a textbook question, but I've read from numerous sources that changing the concentration of the reactants/products won't change the equilibrium constant. Why isn't this contradictory?
Assume the reaction:
xX + yY <---> zZ
where x,y,z are the coefficients of X,Y,Z
Keq = [Z]^z/[X]^x[Y]^y
So if I change the concentration of say, X, then won't Keq change by definition?