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One way to help determine is the the number of molecules needed to combine. So more often than not, a bimolecular reaction will be slower than a unimolecular. Then termolecular being slower than bimolecular. THIS IS NOT FOOL PROOF OR ANY KIND OF LAW TO USE 100% OF THE TIME, just something to consider. Also, look at the Activation energies.
Clarissa Molina 1D wrote:Do you always ignore the reverse of the slow step? Why?
Well the idea is that when it comes to the slow step, the reaction produces products slowly in comparison to the other reactions so that the slow reaction can only proceed forward for a significant amount of time since there is not a significant enough amount of product to proceed with the reverse rxn. It reaches equilibrium so slowly that we can negate the reverse k for the slow reaction.
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