Question

Question 1: Show your calculations from Experiment 1: Ideal Gas Law - Finding Percent H2O2 with Yeast to determine the theoretical number of moles of O2 if the hydrogen peroxide were a 100% solution. NOTE: All work must be shown. Skipping steps or lack of clarity in steps will result in loss of points. All units must be properly labeled.

QUESTION 2: Using the actual moles of O2 you determined from your experiment (n) and the theoretical moles of O2 you just calculated, show your calculations from Experiment 1: Ideal Gas Law - Finding Percent H2O2 with Yeast to determine the percentage of hydrogen peroxide in your experimental sample. NOTE: All work must be shown. Skipping steps or lack of clarity in steps will result in loss of points. All units must be properly labeled.

QUESTION 3: The bottle of hydrogen peroxide you used in Experiment 1: Ideal Gas Law - Finding Percent H2O2 is labeled as a 3% solution (the same as store-bought hydrogen peroxide). Do your experimental results support this (with consideration given to experimental error)? Show your calculations for your percent error of your results. NOTE: All work must be shown. Skipping steps or lack of clarity in steps will result in loss of points. All units must be properly labeled.

BELOW ARE MY CALCULATIONS AND RESULTS FROM EXPERIMENT 1, I JUST NEED YOU TO FIND THE 3 ABOVE ANSWERS.

To determine percentage, you need to first determine how many moles of hydrogen peroxide are present. Rearrange PV=nRT to solve for n, then plug in your known values for P, V, R, and T. Show all your calculations from Experiment 1 for converting your temperature (T) to Kelvin. ANSWER: 21°C= 294 K

Show your calculations from Experiment 1 for converting your pressure (P) to atm. (If you obtained the pressure originally in atm without converting, then convert atm to mmHg to demonstrate you know how to do this conversion.) . ANSWER: 1 atm= 760 mmHg

Show your calculations from Experiment 1 for converting your volume (V) from milliliters (mL) to liters (L). ANSWER: 42ml= 0.042 L

Show your rearrangement of the ideal gas law equation from Experiment 1 to solve for n. Then plug in your P, V, R, and T values (using proper units) and solve. ANSWER:??

Answer 1