## Rate laws vs average rate

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

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### Rate laws vs average rate

Hi can someone explain to me the difference between the average rate of a reaction and the rate laws? when should I use each equation?

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### Re: Rate laws vs average rate

Remember that rate is change in concentration over time (M/s). The average rate of a reaction is the change in concentration of reactants over a certain time interval. So it would be rate=-Δ[R]/Δt. The rate law, on the other hand, is setting rate (M/s) equal to rate constant k times concentration of reactants. So it would be rate=k[R]x.

905022356
Posts: 48
Joined: Mon Oct 02, 2017 7:19 am

### Re: Rate laws vs average rate

Thank you! That helped a lot :)

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