Materials & Reagents Required:

1. Conical Fluxes (250 mL)
2. Measuring Cylinder (25 mL)
3. Volumetric Fluxes (100mL)
4. Stopwatch
5. Glass Rod

Procedure in laboratory (diagram)

Procedure in laboratory



Sample Data and Analysis

Table – 1



Table – 2



Table – 3



Analysis

Plot of log[Rate] vs log[H2O2]:

Here, the order of the reaction with respect to H2O2 = 1 (nearest possible integer of 0.98)

Plot of log[Rate] vs log[KI]:



Here the order of the reaction with respect to KI = 1 (nearest possible integer of 1.02)
The rate law equation can be expressed as,

Rate = k [I–] [H2O2] , where ‘k’ is the rate constant.

Now, Rate=-(∆[H_2 O_2])/∆t , ∆[H_2 O_2]= 0.5× Moles of S2O32- consumed = 0.5× 10 mL × 0.05 M × 0.001 mL-1 = 2.5 × 10-4 M

Rate=-(2.5 × 〖10〗^(-4) M)/(80 s) = 3.125 × 10-6 M.s-1

Rate constant, k = Rate/([I^-] [H_2 O_2]) = (3.125 × 〖10〗^(-6) M.s^(-1) )/(0.062 M×0.005 M) = 0.01 M-1 s-1