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What will happen to the following reaction if the initial concentrations of the reactants and products are as given? 3O2(g)2O3(g)K=1.83107[O2]0=0.419M[O3]0=0.000397M The equilibrium will shift to

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What will happen to the following reaction if the initial concentrations of the reactants and products are as given? 3O2(g)2O3(g)K=1.83107[O2]0=0.419M[O3]0=0.000397M The equilibrium will shift to the right because QK. Nothing because Q=K. The equilibrium will shift to the left because QK

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