HW 7.23

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

Gisela F Ramirez 2H
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HW 7.23

d) How would the rate law differ if the reactions were carried out in an organic solvent?

I am not sure how to answer this, can anyone explain? Thanks!

Chem_Mod
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Re: HW 7.23

If water is no longer the solvent then it is part of the equilibrium constant and therefore in the rate law.