CHEM 133 Week 9 Lab 9 Assignment

CHEM 133 Week 9 Lab 9 Assignment | American Public University System

Lab 9 Assignment

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Comment:Hi Suzy, Your Lab 9 assignment is graded. Message me if you have questions. -Gloria

Question 1 of 12

Please upload (in PDF format) a picture of your Gas Collection Apparatus (Step 2). To receive credit, your ring stand, graduated cylinder, beaker, all tubing, flask, etc. The oxygen bubbles must be clearly visible in the picture, as well as clear label with your name, the lab title (with Experiment number), and the date in clear view. This must be a single picture in a PDF file in order to receive credit.

NOTE: If your document is not clear, organized, and properly labeled, or any part of it is unclear to your instructor, you will not receive credit

Question 2 of 12

Please upload (in PDF format) a picture of your completed Table 1: Temperature, Pressure, and Volume Data and Table 2: Reaction Time Data (Step 3). To receive credit, these must be saved together in a single PDF file.

NOTE: If your tables are not clear, organized, and properly labeled (with units), or any part of it is unclear to your instructor, you will not receive credit.

Question 3 of 12

The goal for Experiment 1: Ideal Gas Law - Finding Percent H2O2 with Yeast is to find the percentage of hydrogen peroxide in the solution. 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.

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. Be sure to click on "Show/Hide Rich Text Editor" above your answer box so you can include subscripts, superscripts, etc. as needed. If your formatting is unclear, you will not receive credit.

Question 4 of 12

The goal for Experiment 1: Ideal Gas Law - Finding Percent H2O2 with Yeast is to find the percentage of hydrogen peroxide in the solution. 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 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.)

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. Be sure to click on "Show/Hide Rich Text Editor" above your answer box so you can include subscripts, superscripts, etc. as needed. If your formatting is unclear, you will not receive credit.

Question 5 of 12

The goal for Experiment 1: Ideal Gas Law - Finding Percent H2O2 with Yeast is to find the percentage of hydrogen peroxide in the solution. 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 your calculations from Experiment  1 for converting your volume (V) from milliliters (mL) to liters (L).

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. Be sure to click on "Show/Hide Rich Text Editor" above your answer box so you can include subscripts, superscripts, etc. as needed. If your formatting is unclear, you will not receive credit.

Question 6 of 12

The goal for Experiment 1: Ideal Gas Law - Finding Percent H2O2 with Yeast is to find the percentage of hydrogen peroxide in the solution. 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 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.

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. Be sure to click on "Show/Hide Rich Text Editor" above your answer box so you can include subscripts, superscripts, etc. as needed. If your formatting is unclear, you will not receive credit.

Question 7 of 12

Show your calculations from Experiment  1: Ideal Gas Law - Finding Percent H2O2 with Yeast for determining 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. Be sure to click on "Show/Hide Rich Text Editor" above your answer box so you can include subscripts, superscripts, etc. as needed. If your formatting is unclear, you will not receive credit.

Theoretical moles of 02=H2O2 volume x density x moles x (1 mol 02/2 mol H202) Volume =50 mL Density = 1.02g/mol Moles=0.0021 Moles of 02=50 x 1.02 x 0.0021 x 1/2 =0.00535 moles

Question 8 of 12

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 for determining the percent 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. Be sure to click on "Show/Hide Rich Text Editor" above your answer box so you can include subscripts, superscripts, etc. as needed. If your formatting is unclear, you will not receive credit.

Percent of H202=theoretical moles x 100=0.00535 x 100 =5.35%

Question 9 of 12

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. Be sure to click on "Show/Hide Rich Text Editor" above your answer box so you can include subscripts, superscripts, etc. as needed. If your formatting is unclear, you will not receive credit.

My calculations do not match with the 3% solution.

% of error = (actual - theoretical)/ actual x 100

= (3 - 5.35)/3x100

=78%

Question 10 of 12

10.0/ 10.0 Points

Please upload (in PDF format) a picture of your flask/balloon apparatus (Step 5). See Figure 5: Gas collection apparatus sample in the eScience procedure. To receive credit, your pot, water, flask, and inflated balloon must be clearly visible in the picture, as well as clear label with your name, the lab title (with Experiment number), and the date in clear view. This must be a single picture in a PDF file in order to receive credit.

NOTE: If your document is not clear, organized, and properly labeled, or any part of it is unclear to your instructor, you will not receive credit.

Question 11 of 12

Please upload (in PDF format) a picture of your completed Table 3: Charles’ Law Part 1 Data (Step 6). To receive credit, this must be saved as a single PDF file.

NOTE: If your tables are not clear, organized, and properly labeled (with units), or any part of it is unclear to your instructor, you will not receive credit.

Question 12 of 12

8.0/ 8.0 Points

How does the molecular motion of the air particles explain your results in Experiment 2: Charles' Law, Part 1? Note that the pressure on the surface of the balloon remained constant, at atmospheric pressure. Be as detailed as possible with your answer to receive full credit.

The speed of the molecules of air is directly proportional to temperature. As the temperature increases, the air particles have more energy, and consequently they move more vigorously. Because of the increase in the random motion and energy, particles strike the wall of the balloon with stronger force resulting in greater inflation of the balloon.