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So, what's your point? :Ssee, look at this site http://www.newton.dep.anl.gov/askasci/chem03/chem03747.htm, at the end u will see that when the pressure is altered the
system is nolongerin equilibrium. "hanges in concentrations or pressures result in a perturbation of the equilibrium such that the system is momentarily not at
equilibrium."
IF we consider the system to NOT be in equilibrium it fails your Kp argument too (which was not a real argument to begin with...).
Any how, I think you need to pay closer attention to what the link says: 'However, the Le Chatelier Principle expresses the system will reacquire equilibrium. This means that, in this case, there will be an increase in the forward rate of reaction so that more product will be formed. This will continue until the pressures are such that the ratio is once again equal to Kp.'
I think what you don't realize here is that the reactants don't necessarily have to increase for the Kp to remain constant. Remember, we're using partial pressures and not the moles themselves.