Question

Kinetics help!

Answer 1

I am doing a lab where I add reagents together and use the method of initial rates to calculate the reaction order and rate law. I need to construct a table giving the actual initial concentrations of the reactants.

For trial one, I made a 100 mL solution of .1 M KIO3, and used 5mL of that plus 5 mL of a solution that was originally .03M 100 mL solution of H3AsO3, 65 mL of a solution that was a buffer, and 25 mL of a .2M 500 mL solution of KI.

How do I construct a table giving the actual initial concentrations of the reactants.
Update: For example, would I say since I used 5 mL of a .1M KIO3 solution, then

((.005)(.1))/(100mL)

with the 100 mL meaning the total volume of trial 1 was 100 mL various chemicals?

Answer 2

well to calculate the rate, you would keep the concentration of one of your reactants constant and then measure the concentration of the other

Answer 3

I suggest organizing your table like this



where you give the concentration of each, element along with the initial rate.

A great example would be this below: