Temperature of Tap Water ( ° C) Room (or regional) Pressure (atm) Initial Volume
ID: 1045411 • Letter: T
Question
Temperature of Tap Water (°C)
Room (or regional) Pressure (atm)
Initial Volume
of Air (mL)
Final Volume of Air
(after reaction) (mL)
Volume of O2 Collected
(Final Volume - Initial Volume)
22
0.9986
54
57
3
Table 3: Reaction Time Data
Time Reaction Started
Time Reaction Ended
Total Reaction Time
7:03
7:09
6:00
POST-LAB QUESTIONS
1. What would happen if you added more than 5 mL of yeast solution to the H2O2?
2. What would happen if you added more than 5 mL of H2O2 to the 5 mL of yeast solution?
3. What was going on in the graduated cylinder as the H2O was pushed out?
4. How would the number of moles (n) of O2 change if the atmospheric pressure doubled but all other variables stayed the same?
5. Using the Ideal Gas Law (PV = nRT), calculate the grams of O2 produced in the reaction. (Hint: solve for n, and then convert moles to grams. Don’t forget to convert your temperature from Celsius to Kelvin.) Show your work.
Temperature of Tap Water (°C)
Room (or regional) Pressure (atm)
Initial Volume
of Air (mL)
Final Volume of Air
(after reaction) (mL)
Volume of O2 Collected
(Final Volume - Initial Volume)
22
0.9986
54
57
3
Explanation / Answer
1) Since hydrogen peroxide forms oxygen gas when it decomposes, we can use the Ideal Gas Law to observe this decomposition reaction,however the natural reaction is very slow and could take weeks,we would use a catalyst. H2O2(aq) ? 2 H2O + O2(g). Catalyst increase the rate of reaction.
2) Yeast cells contain a catalyst called catalase. Catalase speeds up the decomposition of hydrogen peroxide to form water and oxygen.
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