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g. Since the concentration of the H₂O2 solution is 3% by mass, calculate the mass of H₂O2 in the mass determined from the previous part of the 5.00 mL of the solution.

g. Since the concentration of the H₂O2 solution is 3% by mass, calculate the mass of H₂O2 in the mass determined from the previous part of the 5.00 mL of the solution.

Chemistry
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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5 Online f. g. h. i. Using the density of H₂O2, calculate the mass of 5.00 mL of the H₂O2 solution. mass of ₂02Vxd j. me of d Since the concentration of the H₂O2 solution is 3% by mass, calculate the mass of H₂O2 in the mass determined from the previous part of the 5.00 mL of the solution. k. =SML x 1.101 g/m2 = 5.505g Using the molar mass of H₂O2, calculate the number of moles of H₂O2 reacting. #of moles noves CLIC SPICY mass of H₂02 molar mass =0.1659 34.0g/mol = 0.00485mol Using stoichiometry and the balanced chemical equation for the decomposition of H2O2, calculate the number of moles of collected O2. Determine how many grams this is equivalent to. 2 H₂022 H₂0 +0₂ H₂02:0₂ 2:1 0.00485 mole of H₂02 = 7 mole of 02 0.00485 mol 102 x 1 mol 02 -0.002425 moloz 2 mol H₂02 molar mass 0₂ 32.0 g/mol Determine the gas constant, R. Calculate the % error in R for this determination. mass of 02:0.002425 mol x32.0 g/mol = 0.07769 mass of th02-0.1659=2.14 ~ 2 0.07769 equivalent to 2 mass of 02 Briefly explain why it is essential that none of the yeast comes into contact with the H₂O2 solution before the stopper is firmly in place.
Transcribed Image Text:5 Online f. g. h. i. Using the density of H₂O2, calculate the mass of 5.00 mL of the H₂O2 solution. mass of ₂02Vxd j. me of d Since the concentration of the H₂O2 solution is 3% by mass, calculate the mass of H₂O2 in the mass determined from the previous part of the 5.00 mL of the solution. k. =SML x 1.101 g/m2 = 5.505g Using the molar mass of H₂O2, calculate the number of moles of H₂O2 reacting. #of moles noves CLIC SPICY mass of H₂02 molar mass =0.1659 34.0g/mol = 0.00485mol Using stoichiometry and the balanced chemical equation for the decomposition of H2O2, calculate the number of moles of collected O2. Determine how many grams this is equivalent to. 2 H₂022 H₂0 +0₂ H₂02:0₂ 2:1 0.00485 mole of H₂02 = 7 mole of 02 0.00485 mol 102 x 1 mol 02 -0.002425 moloz 2 mol H₂02 molar mass 0₂ 32.0 g/mol Determine the gas constant, R. Calculate the % error in R for this determination. mass of 02:0.002425 mol x32.0 g/mol = 0.07769 mass of th02-0.1659=2.14 ~ 2 0.07769 equivalent to 2 mass of 02 Briefly explain why it is essential that none of the yeast comes into contact with the H₂O2 solution before the stopper is firmly in place.
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