Hydrogen peroxide reacts with thiosulfate ion in slightly acidic solution as follows.
H2O2 + 2S2O3^2- + 2H+ -- 2H2O + S4O6^2-
This reaction rate is independent of the hydrogen-ion concentration in the pH range 4 to 6.
The following data were obtained at 25 °C and pH 5.0. Initial concentrations: [H2O2] = 0.036 molL-1; [S2O3^2-] = 0.02040 mol L-1
t/ min: 16, 36, 43, 52.
[S2O32-]/ (10^-3 mol L-1): 10.30, 5.18, 4.16, 3.13
(a) What is the order of the reaction? (b) What is the rate constant?
for better view of the question, go to this webpage http://edelsteincenter.files.wordpress.com/2010/

Question

Hydrogen peroxide reacts with thiosulfate ion in slightly acidic solution as follows.
H2O2 + 2S2O3^2- + 2H+ --> 2H2O + S4O6^2-
This reaction rate is independent of the hydrogen-ion concentration in the pH range 4 to 6.
The following data were obtained at 25 °C and pH 5.0. Initial concentrations: [H2O2] = 0.036 molL-1; [S2O3^2-] = 0.02040 mol L-1
t/ min: 16, 36, 43, 52.
[S2O32-]/ (10^-3 mol L-1): 10.30, 5.18, 4.16, 3.13
(a) What is the order of the reaction? (b) What is the rate constant?
for better view of the question, go to this webpage http://edelsteincenter.files.wordpress.com/2010/

anonymous · Answer

http://edelsteincenter.files.wordpress.com/2010/07/kinetics-problems-2-alberty.pdf

callisto · Answer

which question in the file?

callisto · Answer

The reaction is a second order reaction as the half life becomes longer as the reaction proceeds.
rate = k [H2O2][S2O3^2-]
can't help for the following steps

anonymous · Answer

what should i do to show that it is a second order reaction? plot graph of what variable against what?