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The pre-equilibrium approach says that the intermediate is formed and sustained in a rapid formation reaction and its reverse, and you assume it reaches a sort of equilibrium. Instead, the steady state approach assumes that concentrations of the intermediates are low and don't change. As you don't want intermediates in the overall rate law, you can substitute out for the intermediate if they are present in the slow step. This is b/c the slow step is the rate-determining step.
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