Question

Please explain Whole Question Number 2.

Also some explanation On Rate of reaction

( please No Copy Paste)

Answer 1

http://www.xtremepapers.com/papers/CIE/Cambridge%20International%20A%20and%20AS%20Level/Chemistry%20(9701)/9701_w08_qp_4.pdf

Answer 2

okay, so starting with the basics,
a reaction may occur in a single step or a series of steps. one of those steps will be the lowest step and that will be the rate determining step. The other steps will not affect the rate of reaction.
now, as you know, as the reaction proceeds, the concentration of the reactants and the products change,
so the rate of reaction= change in concentration of substance/time take for the change.
The relationship between the rate of reaction and the active masses of the reacting substances is
that 'the rate of reaction is proportional to the active masses of the reactant or to the product of the active masses, if more than one reactants is involved in the reaction.'
aA + bB---> cC+dD
Rate if reaction=k [A]^a [B]^b
this is the rate equation

Answer 3

do you have any questions on this part?

Answer 4

this is just a primary part which i already know,

The main confusion lies in determining order of any reaction by comparing two reacting species.

I guess you did not look at the above question paper? did you?

Answer 5

I did look at the question paper,
That above was just a little summary on the rate of reaction.
You weren't really specific on what was confusing you.

Anyway, the order of the reactions as asked in the paper (b) are,
1- in the first equation we have 1 mole of H2O2 and 1 mole of iodine ion and no hydrogen ion in the reactants, it will be 1 1 0 in the table.
2- we have one mole of O and I- in together in OI- and we have 1 mole of H+, so it will be 1 1 1 in the table.
3- we have 1 O in HOI and 2H in HOI and H+ that form H2 in the product side, and 2I, one in HOI and the other as I- that form I2 in the product side.