3. In today's experiment you determine that you collected 1.33 x 10-3 mols of oxygen. Calculate (show your setup for the conversion!) how many mols of H,O, were in your hydrogen peroxide solution. Note: You will need a conversion factor from the equation you balanced in question 2. mols of H,O, 4. Based on your answer above, how many grams of H,0, were in the hydrogen peroxide solution? (H,O, has a molecular weight of 34.0 g/mol) grams of H,O, 5. Assume the grams of H,O, calculated in question 4 were found in a 6.00 hydrogen peroxide solution. Calculate the mass percent H,O, in the solution. gram sample of a % HO,
3. In today's experiment you determine that you collected 1.33 x 10-3 mols of oxygen. Calculate (show your setup for the conversion!) how many mols of H,O, were in your hydrogen peroxide solution. Note: You will need a conversion factor from the equation you balanced in question 2. mols of H,O, 4. Based on your answer above, how many grams of H,0, were in the hydrogen peroxide solution? (H,O, has a molecular weight of 34.0 g/mol) grams of H,O, 5. Assume the grams of H,O, calculated in question 4 were found in a 6.00 hydrogen peroxide solution. Calculate the mass percent H,O, in the solution. gram sample of a % HO,
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer the three following questions by using the chart for reference. Please type instead of showing the work handwritten, I’m bad at reading hand writing.
![3. In today's experiment you determine that you collected 1.33 X 10-3 mols of
Calculate (show your setup for the conversion!) how many mols of H,O, were in your
hydrogen peroxide solution. Note: You will need a conversion factor from the equation
you balanced in question 2.
охygen.
mols of H,O,
4. Based on your answer above, how many grams of H,0, were in the hydrogen peroxide
solution? (H,O, has a molecular weight of 34.0 g/mol)
grams of H,O,
5. Assume the grams of H,O, calculated in question 4 were found in a 6.00 gram sample of a
hydrogen peroxide solution. Calculate the mass percent H,O, in the solution.
% H,O,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdbbec8f6-4681-4cc6-afa4-b921cc4a8dba%2Fa6e2a0d2-3bc8-4e50-a210-d506b84e3380%2Fdaxkc3v_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3. In today's experiment you determine that you collected 1.33 X 10-3 mols of
Calculate (show your setup for the conversion!) how many mols of H,O, were in your
hydrogen peroxide solution. Note: You will need a conversion factor from the equation
you balanced in question 2.
охygen.
mols of H,O,
4. Based on your answer above, how many grams of H,0, were in the hydrogen peroxide
solution? (H,O, has a molecular weight of 34.0 g/mol)
grams of H,O,
5. Assume the grams of H,O, calculated in question 4 were found in a 6.00 gram sample of a
hydrogen peroxide solution. Calculate the mass percent H,O, in the solution.
% H,O,
![Trial 1
Trial 2
31.588 g
32.434 g
1. Mass of empty test tube
37.475 g
39.707 g
2. Mass of test tube with H,O, solution
5.887 g
7.273 g
3. Mass of H,O, solution
4.4186 lit/mol
5.4528 lit/mol
4. Volume of oxygen collected
17.9 C
17.1 C
5. Temperature (°C)
291.05 k
290.25 k
6. Kelvin temperature (K = °C + 273.15)
%3D
0.867 atm
0.867 atm
7. Atmospheric pressure
0.1839 mol
0.2272 mol
8. Moles of oxygen gas](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdbbec8f6-4681-4cc6-afa4-b921cc4a8dba%2Fa6e2a0d2-3bc8-4e50-a210-d506b84e3380%2Ftz3k3n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Trial 1
Trial 2
31.588 g
32.434 g
1. Mass of empty test tube
37.475 g
39.707 g
2. Mass of test tube with H,O, solution
5.887 g
7.273 g
3. Mass of H,O, solution
4.4186 lit/mol
5.4528 lit/mol
4. Volume of oxygen collected
17.9 C
17.1 C
5. Temperature (°C)
291.05 k
290.25 k
6. Kelvin temperature (K = °C + 273.15)
%3D
0.867 atm
0.867 atm
7. Atmospheric pressure
0.1839 mol
0.2272 mol
8. Moles of oxygen gas
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