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Rate of Reaction Lab
Hydrogen Peroxide Lab
Balance Chemical Reaction:
Effect of Temperature on Rate of Reaction
Directions (Procedures)
1. Turn on the Hot plate on the bench. One Hot plate per bench.
1. Obtain a "Bubble-O-meter"
2. Using scale on side of "Bubble-O-meter", add 10ml of hydrogen peroxide solution.
3. Using stopwatch, record (in data table below) the number of bubbles you see in 60.seconds @room temperature
Room temperature can be found on the barometer in the corner of the room.
4. Place the "Bubble-O-meter" on the hot plate (one plate per bench). Wait a few minutes for solution to heat up.
5. Using stopwatch, record (in data table) the number of bubbles you see in 60.seconds.
6. Take off Hot plate and let it cool back down to room temperature (wait 1-2 minute).
Effect of Catalysts on Rate of Reaction
Directions (Procedures)
1. Use the results of room temperature trial from the above procedures as you "room temp" trial. Record in data table below.
2. Using a pipette, add 1 ml (volume of the skinny part, not the bulb part) of potassium iodide (KI) solution to the hydrogen peroxide solution.
3. Using a stopwatch, record (in the data table below), the number of bubbles you see in 60.seconds.
| Temperature vs. Reaction Rate |
| Temperature |
Rxn Rate (bubbles/60.sec) |
| ______________ |
_____________________ |
| ______________ |
_____________________ |
| Presence of Catalyst vs. Reaction Rate |
| Catalyst(Y/N) |
Rxn Rate (bubbles/60.sec) |
| ______________ |
______________ |
| ______________ |
______________ |
Questions: Answer on separate sheet of paper (not in space between questions)
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).
2. Did your observations support your answer in Question 1 (simple yes or no answer)
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).
4. Did your observations support your answer in Question 3 (simple yes or no answer)
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.