Hi I need some help understanding reaction kinetics, and I’m trying to get an overview, so I’d really appreciate some help. I have 3 individual/quite unrelated questions, if you have time to answer one that would be very much appreciated.(adsbygoogle = window.adsbygoogle || []).push({});

1. In what situations dos the Definition of the reaction rate for a general reaction Hold true?

aA + Bb --> pP+qQ

-(1/a)*(d[A]/dt)= -(1/b)*(d/dt) = -(1/p)*(d[P]/dt) = -(1/q)*(d[Q]/dt)

I would assume this definition only holds true when all the rates are equal, so this does not apply for reactions where the rate of A is different from the rate of B (if this is possible)

2. If the rate of A is slower than the Rate of B, would they then not be comsumed at the same RATE because A would be the limiting factor, the equation -(1/a)*(d[A]/dt)= -(1/b)*(d/dt) holds true for all reactions?

3. Is it true that if the rate law for A + B --> C +D is givn by -d[A]/dt = k[A]^n^m with respect to A, then it might be different with repsect to B? So -d/dt might be different (slower or faster) than -d[A]/dt, so the -d[A]/dt=-d/dt = k[A]^n*^m only holds true for elementary reactions, while for complex reactions the rate law for -d[A]/dt could be equal to k[A]raised to a first order while -d/dt could be equalt to k[A]^2^1 (something different?)

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# 3 Questions regarding reaction kinetics- please help me out.

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