Part IV Decompose 3% H2O2 solution with 0.5 M KI solution at-30°C 20. Conduct Pa

Question

Part IV Decompose 3% H2O2 solution with 0.5 M KI solution at-30°C 20. Conduct Part IV identically to the procedure in Part I, with one exception: set the water bath at 30°C. Use warm tap water adjusted to -30°C (record precise temperature) 21. Click on "Options" on the tope menu then choose "Graph Options" Type "Decomposition of H202" in the title box. Click on "Done." Save your data to your flor disk and name it with a descriptive file name. DATA TABLE TemperatureInitial rate 123.0031 | 23.10 Part Reactants (kPa/s) 4mL 3.0% H2O2 + 1 mL 0.5 M KI 4 mL 3.0% H2O2 + 1 mL 0.25 M KI 4mL1.5% H2O2 + 1 mL 0.5 M Kl mL 0.5 M KI ct.oosl 14mL 3.0% H2O2 + 1 | 30.9"Clou, 1 | . IV DATA ANALYSIS Initial rate (mol/L-s) [H202] after mixing Rate constant Part after mixing Determine the order of the reaction in H202 and KI. Explain how you arrived at your answer Calculate the rate constant, k, and write the rate law expression for the catalyzed decomposition of hydrogen peroxide. To convert the rate from kPa/s to M/s use the ideal gas equation, M = P/RT where R, is the gas constant-8.314 LkPaeK'l. mol-1 te

Explanation / Answer

2. Here we have to explain which step is the rate determining step.

The following mechanisms are given,

H2O2 + I- --> IO- + H2O

H2O2 + IO---> I- + H2O + O2

Both the given mechanisms are correct. It represent the decomposition of H2O2 with iodine (I).

The rate expression can be written as ,

The following mechanisms are given,

H2O2 + I- --> IO- + H2O Rate (1) = K1 [H2O2] [I-] Slow reaction

H2O2 + IO---> I- + H2O + O2 Rate (2) = K2 [H2O2] [IO-] Fast reaction

----------------------------------------------------------------------------

2H2O2 ---> 2H2O + O2 Rate =  [H2O2] [I] (Overall reaction)

It is known that the slow reaction is consider as the rate determining step.

Hence the 1st step which involve the formation of the intermediate is the rate determining step.

3. Here we have to the given Arrhenious equation to determine the activation energy Ea.

Step-1

The given Arrhenious equation is, ln K1/K2 = Ea/R (1/T2 - 1/T1)

Ea = Activation energy

R= Gas constant

T= Kelvin temperature

By solving this expression, the activation energy can be written as,

R ln K2/K1

Ea = ---------------

1/T1 - 1/T2

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---