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Yes, by altering the concentrations of either reactants or products or both while the reaction is at equilibrium, it will be temporarily thrown out of balance. However, Le Chatelier's principle states that a reaction thrown out of equilibrium will try to minimize the effect of changing the concentration, so give the reaction some time, and eventually it goes back to its equilibrium state.
Cole 1J wrote:If the concentration of a product or reactant is changed while a reaction is in equilibrium, will the reaction then be temporarily shifted out of equilibrium?
yes, changing the concentration of the reactant or products will temporarily offset the equilibrium making it shift to the right or left because when a reaction is at equilibrium the concentrations are not changing. The reaction will not be altered to much from equilibrium though and it will quickly make its way back to equilibria due to Le Chatelier's Principle that states "chemical reactions adjust so as to minimize the effect of any changes". This is explained clearly in Lavelle's modules posted on his website about Chemical Equilibria, I believe it's part 2 of the two chemical equilibria modules
Yes, any change in the concentration of either the reactants and product will shift the equilibrium towards either the left or the right for a temporary period of time. Since both the forward and reverse reactions are happening simultaneously the equilibrium will shift back and after some time equilibrium will be restored. You can also think of this in terms of the reaction quotient and K.
Furthermore, if the concentrations of reactants are increased, the equilibrium will shift to the right and create more product to compensate, and if the concentrations of products are increased, the equilibrium will shift to the left and create more reactants to compensate. As stated above, this is due to Le Chatlier's Principle.
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