Topic_8_Experimental_Procedure_Fall_2011

Topic_8_Experimental_Procedure_Fall_2011 - Topic 8 Topic 8...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
Topic 8 Topic 8 Experiment The Decomposition of Hydrogen Peroxide Introduction Since the decomposition of hydrogen peroxide produces oxygen gas as one of the products, the rate of gas formation can be used to measure the rate of the reaction. Experimentally, you will measure the gas by monitoring the pressure of gas within a sealed reaction vessel as a function of time. To accomplish this, you will set-up a plastic reaction bottle and attach a tube to a gas pressure sensor (and a temperature sensor). The sensors are connected to a computer and the data will be displayed as shown in the figure below. From the pressure change of gas per second,the rate of the reaction can be obtained. Reaction rates are usually given in units of molarity per second, and these are the units that should be used when reporting your final results. As explained in case study, you will first explore several different catalysts that are known to be effective at promoting the rate of the decomposition reactions. Aqueous iodide will be used as an example of a homogeneous catalyst, manganese(IV) oxide will be used as a heterogeneous catalyst, and catalase will be used as a biocatalyst. In addition, you will investigate if copper(II) ion can be used to inhibit the effectiveness of catalase as a catalyst.
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Topic 8 Experimental Procedure Your TA will help you to setup the apparatus and make sure that you are able to make measurement after that the rest is up to you. Calibration Measure 25 mL of water into the plastic bottle, add a magnetic stir bar, and stopper the bottle with the stopper that is attached to the pressure sensor. To launch the program select My Computer Shared 412 Gas Kinetics. Once the LoggerPro program displays, record the room pressure and temperature in your notebook. Use your data to calculate the number of moles of gas in 20. mL under these conditions. Obtain the equivalent solution concentration in units of molarity by dividing the moles of air by the volume of the water used. Open the stopcock on the stopper and start the data acquisition by clicking on the
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 10/11/2011 for the course CHEM 012 taught by Professor Mounaamaalouf,reneescole, during the Spring '11 term at Iowa State.

Page1 / 4

Topic_8_Experimental_Procedure_Fall_2011 - Topic 8 Topic 8...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online