Question

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. 1.02 g/mL * 5 mL = 5.1g / 34 g = 0.15 mol 4. Was the calculated percentage of hydrogen peroxide close to the same as the percentage on the label (3%)? Calculate percent error of your value.

Answer 1

Answer:

1. 0.05moles of H₂O₂ is consumed in the reaction

2. the number of unreactive H₂O₂ is 0.20 moles

3. the percentage of H₂O₂ is 0.18%

4. no, not similar to 3% H₂O₂

5. percentage error = 0.94 = 94%

Explanation: