Table 1: Temperature, Pressure, and Volume
Data
Temperature of Distilled H2O: 21.4 c
Room (or regional) Pressure (atm): .99328 atm
Initial Volume of Air (mL) 10 ml
Final Volume of Air (after reaction) (mL) 62 ml
Volume of O2 Collected (Final Volume - Initial Volume) 62-10=52 ml
Table 2: Reaction Time Data
Time Reaction Started 0:00
Time Reaction Ended 2:00
Total Reaction Time 2 mins
Required 10 mL of 3% hydrogen peroxide, 5mL yeast.
1.A.) 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.
1.B.) 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.
1.C.) Determine the percentage of hydrogen peroxide in your solution.