Temperature of Distilled H2O: Room (or regional) Pressure (atm): Initial Volume of Air (mL) Final Volume of Air (after r

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Temperature of Distilled H2O:
Room (or regional) Pressure (atm):
Initial Volume
of Air (mL)
Final Volume of Air
(after reaction) (mL)
Volume of O2Collected
(Final Volume - Initial Volume)
22C
1.00atm
27ml
77ml
61 ml
Time Reaction Started
Time Reaction Ended
Total Reaction Time
10:15
10:18
3 minutes
1. Calculate the number of moles of O2 produced using the ideal
gas law. Then, use this value to calculate the number of moles of
hydrogen peroxide you began the experiment with. Hint: Use the
balanced equation provided in the lab introduction.
2. Calculate the number of moles of hydrogen peroxide you would
have if you used 5 mL of a pure hydrogen peroxide solution. Hint:
The density of hydrogen peroxide is 1.02 g/mL.
3. Determine the percentage of hydrogen peroxide in your
solution.
4. Was the calculated percentage of hydrogen peroxide close to
the percentage on the label (3%)? Calculate percent error of your
value.