3 Questions regarding reaction kinetics- me out.

[christian0710]

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.

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?)

 

[Borek]

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)

It is not possible. I already told you somewhere else that we use stoichiometric coefficients to make sure rates of the reaction for all substances involved are identical.

 

[christian0710]

Hi borek, yes i was a bit confused on what question you were answering but now it seems more clear to me: What you are saying is that No matte what reaction we have (Zero order, first order, second order, complex) the equation -(1/a)*(d[A]/dt)= -(1/b)*(d/dt) = -(1/p)*(d[P]/dt) = -(1/q)*(d[Q]/dt) is true? and in some cases the rate of any of the reactants might display the following relationship = k[A]^m^n (for complex reactions) and in elementary reactions the orders of the reaction equals the koefficients of the reactants?

If this is a correct understanding, I'm really happy :)

 

[christian0710]

Ohh yes an just to make sure it's 100% clear for me:

If -(1/a)*d[A]/dt)=k[A]^m^n

Then This must also be true

-(1/b)*(d/dt)=k[A]^m^n

:)

 

[Borek]

No matte what reaction we have (Zero order, first order, second order, complex) the equation -(1/a)*(d[A]/dt)= -(1/b)*(d/dt) = -(1/p)*(d[P]/dt) = -(1/q)*(d[Q]/dt) is true?

and in some cases the rate of any of the reactants might display the following relationship = k[A]^m^n (for complex reactions) and in elementary reactions the orders of the reaction equals the koefficients of the reactants?

If -(1/a)*d[A]/dt)=k[A]^m^n

Then This must also be true

-(1/b)*(d/dt)=k[A]^m^n

Yes, yes, yes & yes.

 

[christian0710]

Thank you very much Borek - Now I'm really happy :D