I’ve attached all the info you may need, I need help with solving: 1. The Data a

Question

I’ve attached all the info you may need, I need help with solving: 1. The Data analysis table 2. Questions 1, 2, 3 Thanks in advance! LabQuest 12 The Decomposition of Hydrogen Peroxide The decomposition of hydrogen peroxide in aqueous solution proceeds very slowly. A bottle of 3% hydrogen peroxide sitting on a grocery store shelf is stable for a long period of time. The decomposition takes place according to the reaction below A number of catalysts can be used to speed up this reaction, including potassium iodide, manganese (IV) oxide, and the enzyme catalase. If you conduct the catalyzed decomposition of hydrogen peroxide in a closed vessel, you will be able to determine the reaction rate as a function of the the vessel that is caused by the production of oxygen gas. If you vary the initial molar concentration of the HO2 solution, the rate law for the reaction can also be determined. Finally, by conducting the reaction at different temperatures, the activation energy, E can be calculated. pressure increase in OBJECTIVES In this experiment, you will Conduct the catalyzed decomposition of hydrogen peroxide under various conditions. Calculate the rate constant for the reaction. Determine the rate law expression for the reaction. .Calculate the activation energy for the reaction. MATERIALS LabQuest LabQuest App Vernier Gas Pressure Sensor Temperature Probe two-hole #5 rubber stopper with stems tubing with two Luer-lock utility clamp 3% hydrogen peroxide. .., solution 0.5 M potassium iodide, KI, solution distilled water two 25 ml graduated cylinders 50 mL graduated cylinder magnetic stirrer and stir bar cold water bath 125 mL. Erlenmeyer flask

Explanation / Answer

Answer 1 :-

k = rate/([H2O2]^x [KI]^y)

rate1 = k[H2O2]^x [KI]^y

rate2 = k[H2O2]^x [KI]^y

rate1/rate2 = (k[H2O2]^x [KI]^y)/(k[H2O2]^x [KI]^y)
(1.15 X 10^-5)/((2.66 X 10^-6)) = (k/k)*((0.704/0.704)^x)*((0.1/0.5)^y)
4.3 = 2^y
y 2 (to the nearest integer)

Answer 2 :-

the machanism of the reaction is correct. The second step of the reaction is the slowest step so this step is the rate determining step.

Answer 3 :-

Ea =      R ln k2 / k1

             1/T1 – 1/T2

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