What Is The Rate Equation For The Catalyzed Decomposition Of Hydrogen Peroxide

Chemical Kinetics of Hydrogen Peroxide Decomposition

Purpose
The purpose of this experiment was to determine the rate equation for the catalyzed decomposition of hydrogen peroxide H2O2.

Procedure
The procedure for this lab can be found on pages 36 - 40 in “General Chemistry CHE111L Laboratory Manual Spring 2014.”

Data Tables
Carbon copies of data tables and the graph have been attached to the back of this lab report.

Calculations

30 mL of solution  0.03L

Molarity of 3% H2O: x x = 0.882 M

Initial Molarity of H2O2:

Exp. 1: 5ml H2O2 x = 0.0041mol, = 0.147 M

Exp. 2: 10mL H2O2 x

Exp. 3: 5ml H2O2 x = 0.0041mol, = 0.147 M

Initial Molarity of KI:

Exp. 1: 10 ml KI x = 0.001 mol, = 0.033 M

Exp. 2: 10mL KI x

Exp. 3: 20 ml KI x = 0.002mol, = 0.067

Rate = k [H2O2]x [ KI]y

Order of KI:

y = 1

Order of H2O2 :

x=1

K1 : .089 =k (0.147)(0.033)  k1= 18.542

K2: .180= k (0.294)(0.033)  k2=13.469

K3: .132= k(0.147)(0.067)  k3= 18.557

K average: 16.856

Summary of Results

Exp. #
[H2O2]0
[KI]0
Initial Rate of O2, mm Hg/s
Specific rate constant, k
1
0.147
0.033
0.089
18.542
2
0.294
0.033
0.180
18.557
3
0.147
0.033
The initial rate of O2 was found to be 0.089mmHg/s and the specific rate constant was found to be 18.542. In the second experiment the initial molarity of H2O2 and of KI in the solution were found to be 0.294 and 0.033 respectively. The initial rate of O2 was found to be 0.180 mmHg/s and the specific rate constant was found to be 18.557. In the third experiment the initial molarity of H2O2 and of KI in the solution were found to be 0.147 and 0.067 respectively. The initial rate of O2 was found to be 0.132 mmHg/s and the specific rate constant was found to be