[ktschix]

I have no idea how to do this problem, please show me how.

Experiment    Initial Concentration of BrO3   Initial Concentration of Br
                   (mol/L)                                (mol/L)
1                  0.10                                   0.10
2                  0.20                                   0.10
3                  0.20                                   0.20
4                  0.10                                   0.10

Initial Concentration of H           Measured Initial Rate (mol/L x S)
(mol/L)
0.10                                      8.0 X 10^-4
0.10                                      1.6 X 10^-3
0.10                                      3.2 X 10^-3
0.20                                      3.2 X 10^-3

Determine the orders for all three reactants, the overall reaction order, and the value of the rate constant.

Thank you in advance for the replies

[opti384]

First you should show your attempts.

[ktschix]

I can't, that was all the information given for the problem, unless there is a way to get that from the problem then I am not sure

[JVC]

You are being asked to determine how changing the concentration of each of the three products changes the rate of the reaction.
For each species involved, try to identify a pair of values where the concentration of only that species is changed. Then compare the change in rate to the change in concentration.

This should give you an idea of the relationship between the concentration and the rate for each reactant (which is the order of the reaction with respect to that particular reactant).
The overall order would be the sum of the individual orders.
The rate constant can only be determined by the rate constant for the reaction:

Rate = k(rate constant) [BrO3]^x
^y[H+]^z
where x, y and z are the orders with respect to each of the species.
The rate and concentrations can be selected from any experiment.

Hope this helps.