Editing revision 16 of Rate Of Reaction - Hydrogen Peroxide Lab
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<center><b>Rate of Reaction Lab</b></center> <center><b>Hydrogen Peroxide Lab</b></center> <i>Balance Chemical Reaction:</i> <br><br> <b>Effect of Temperature on Rate of Reaction</b><br> <b>Directions (Procedures)</b><br> 1. Turn on the Hot plate on the bench. One Hot plate per bench.<br> 2. Obtain a "Bubble-O-meter"<br> 3. Using scale on side of "Bubble-O-meter", add 20ml of hydrogen peroxide solution.<br> 4. Using stopwatch, record (in data table below) the number of bubbles you see in 3minutes <b>@room temperature</b><br> (Not seeing any bubbles is <nowiki>OK</nowiki>. It does not mean lab is wrong)<br> 5. Place the "Bubble-O-meter" on the hot plate (one plate per bench). Wait a few minutes for solution to heat up (wait until you see 1st bubble before starting stopwatch).<br> 6. Using stopwatch, record (in data table) the number of bubbles you see in 3minutes.<br> 7. When done, take "Bubble-O-meter" off Hot plate and let it cool back down to room temperature (wait 1-2 minute).<br> <br> <b>Effect of Catalysts on Rate of Reaction</b><br> <b>Directions (Procedures)</b><br> 1. Use the results of room temperature trial from the above procedures as you "room temp" trial. Record in data table below.<br> 2. You can use the same solution as the step above. Once "Bubble-O-meter" has cooled for a 1-2 minute (Step7), add 5-6 drops of potassium iodide (KI) solution to the hydrogen peroxide solution. Make sure that you put the top of "Bubble-O-meter" back on and that there is enough water.<br> 3. You need to wait until the catalyst (KI) starts working before you start counting drops. Count the number (& record in the data table below), the number of bubbles you see in 3minutes. <br> 4. Rinse out all parts of the "Bubble-O-meter" and put them away to dry. <br> <table bgcolor=beige border=2> <tr> <th colspan=8 align=center>Temperature vs. Reaction Rate</th> <tr> <tr> <th>Temperature</th> <th>Rxn Rate (bubbles/60.sec)</th> <tr> <tr> <th>______________</th> <th>_____________________</th> <tr> <tr> <th>______________</th> <th>_____________________</th> <tr> </table> <br> <table bgcolor=beige border=2> <tr> <th colspan=8 align=center>Presence of Catalyst vs. Reaction Rate</th> <tr> <tr> <th>Catalyst(Y/N)</th> <th>Rxn Rate (bubbles/60.sec)</th> <tr> <tr> <th>______________</th> <th>______________</th> <tr> <tr> <th>______________</th> <th>______________</th> <tr> </table> <br> <br> <br> <br> -----<br> <br> <br> <b>Questions: Answer on separate sheet of paper (not in space between questions)</b><br> <br> <br> 1. Would you expect the rate of carbon dioxide formation in the above room temp solution to be greater, equal or less than with the room temp solution? Why? (make sure to use effective collisions in your discussion).<br> <br> 2. Did your observations support your answer in Question 1 (simple yes or no answer)<br> <br> 3. Would you expect the rate of carbon dioxide formation while stirring greater, equal or less than when not stirring the solid in the solution? Why? (make sure to use effective collisions in your discussion).<br> <br> 4. Did your observations support your answer in Question 3 (simple yes or no answer)<br> <br> 5. Have you seen another experiment that would be explained with the same reasoning as in Question 3? You can not use any example of a solid in a solution.
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