i don't understand the part b]
2.(b) Given
rate= k[H2O2]a[I-]b[H+]ca represents the order of reaction with respect to [H
2O
2].
b represents the order of reaction with respect to [I
-].
c represents the order of reaction with respect to [H
+].
NOTE : 1. The slowest step is the rate determining step.
2. The number of moles of a reactant in the rate determining step gives the order with respect to that of the reactant.
When step 1 is slowest overall :
a=1, b=1 and c=0This is because in step 1, the number of moles of H
2O
2 is 1 and so is I
-. However H
+ is not present in this equation which means it has order zero.(Reaction is independent of H
+)
When step 2 is slowest overall:
a=1, b=1 and c=1IO
- is formed from H
2O
2 and I
-. Replace the first equation in the second and you'll get :
H
2O
2 + I
- + H
+ ---> HOI + H
2O
From this equation, note the number of moles of the respective reactants.
When step 3 is slowest overall :
a=1, b=2 and c=2.Replace the new equation found above in this third step and you'll get :
H
2O
2 +
2I
- +
2H
+ ---> I
2 + 2H
2O
From this equation, note the number of moles of the respective reactants.
I sincerely hope my explanations are clear enough for you to understand.
