Differential Rate Law

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

Erik Buetow 1F
Posts: 96
Joined: Fri Aug 30, 2019 12:15 am

Differential Rate Law

why is "k" in the differential rate law (kR^n) dependent on activation energy? And what does this mean?

Kate Osborne 1H
Posts: 102
Joined: Fri Aug 30, 2019 12:16 am

Re: Differential Rate Law

k is the rate constant and is what allows for different rates when there is the same concentration of reactants and products

Frank He 4G
Posts: 50
Joined: Tue Nov 12, 2019 12:19 am

Re: Differential Rate Law

Activation energy is essentially the energy input needed to break the bonds of a reactant so that new bonds can form to create the product, so if the activation energy, or energy required to make the reaction happen, is high, then naturally it would take longer for a reaction to happen, which means that the number that tells us how fast the reaction happens, k, would be affected.

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