I want to know how to draw the graph and the answer to these following questions for part 1 by what rate your [ ] decrease when you halfed the [kio3]? Why this occurred
b) what does the slope of the graph gives you
For part 2
Graph, and answerto the following for every 10C increase rate of rxn double is this statement true about your reaction

The thing is that I don't understand what you are saying.


what rate your [ ] decrease when you halfed the [kio3]? why this occured

What does that mean? What reaction occurred? What are you investigating?:confused:

i want to know how to draw the graph and the answer to these following questions for part 1 by what rate your [ ] decrease when you halfed the [kio3]? why this occured
b) what does the slope of the graph gives you
for part 2
graph, and answerto the following for every 10C increase rate of rxn double is thsi statement true about your reaction

There are several "iodine clock" reactions. '

Iodine clock reaction - Wikipedia, the free encyclopedia (http://en.wikipedia.org/wiki/Iodine_clock_reaction)

You must be doing the "Iodate" version

In this protocol, iodide ion is generated by the following slow reaction between the iodate and bisulfite:

IO_3^- + 3HSO_3^- \rightarrow I^- + 3HSO_4^-

IO_3^- + 5I^- + 6H^+ \rightarrow 3I_2 + 3H_2O

I_2 + HSO3^- + H_2O \rightarrow 2I^- + HSO4^- + 2H^+

The first reaction is the rate-determining step, therefore the kinetics are determined by that reaction. I think that this would, therefore, be the rate equation, but I don't have time to verify it.

K = \frac {[IO_3^-][HSO_3^-]^3}{[I^-][HSO_4^-]^3}

Here's a link on the kinetics.

Landolt Reaction - Iodine Clock Kinetics (http://www.chemie.uni-regensburg.de/Organische_Chemie/Didaktik/Keusch/D-Landolt-e.htm)


Please explain your questions. You need to specify what graph you are talking about.

What is th epurpose of idodin clock reaction

Well, it can be used to determine the order of reaction with respect to the reactants used.