[pnblwzrd]

Im having a lot of trouble with this question:
4.  The decomposition of hydrogen peroxide is catalyzed by iodide ion.  The
   Catalyzed reaction is thought to proceed by a two-step mechanism:
H2O2(aq)   +   I-(aq)   →   H2O(l)   +   IO-(aq)                   (slow)
IO-(aq)   +   H2O2(aq)   →   H2O(l)   +   O2(g)   +   I-(aq)     (fast)
   (a)  Write the rate law for each of the elementary reactions of the mechanism.
   (b)  Write the chemical equation for the overall reaction.                                
   (c)  Identify the intermediate, if any, in the mechanism 
   (d)  Assuming that the first step of the mechanism is rate determining, predict the
           rate law for the overall process. 
I know the overall reaction is 2 H2O2 -> 2 H2O + O2 (or at least i think I know) but other than that I don't really know what to do or how to identify and intermediate.
Any help?

[nj_bartel]

Do you know what a catalyst is?  What are the components of a catalyzed reaction?  How did you find the overall reaction?

[pnblwzrd]

thats all the information

[nj_bartel]

I know that's all the information directly associated with the problem.  My question refer to background knowledge you should have in order to be able to solve that problem.

[pnblwzrd]

you aren't really helping by asking me questions.

[nj_bartel]

The answer to A, B, C, and D are all 72 K 

[Astrokel]

Im having a lot of trouble with this question:
4.  The decomposition of hydrogen peroxide is catalyzed by iodide ion.  The
   Catalyzed reaction is thought to proceed by a two-step mechanism:
H2O2(aq)   +   I-(aq)   →   H2O(l)   +   IO-(aq)                   (slow)
IO-(aq)   +   H2O2(aq)   →   H2O(l)   +   O2(g)   +   I-(aq)     (fast)
   (a)  Write the rate law for each of the elementary reactions of the mechanism.
   (b)  Write the chemical equation for the overall reaction.                                
   (c)  Identify the intermediate, if any, in the mechanism 
   (d)  Assuming that the first step of the mechanism is rate determining, predict the
           rate law for the overall process. 
I know the overall reaction is 2 H2O2 -> 2 H2O + O2 (or at least i think I know) but other than that I don't really know what to do or how to identify and intermediate.
Any help?

a) r= k[reactant]^n
b) right
c) Substances generated by one step and used for the succeeding step are considered intermediates.
d) The order of the concentration of the reactant in the overall rate law is the stoichiometric coefficient of the particular reactant in the rate determing step.

For example, rate determing step:  2A + B --> C
                                 
Therefore, the overall rate law is r = k[A]^2[B ]