Please help with question g 5 Onlinef.g.h.i.Using the density of H₂O2, calculate the mass of 5.00 mL of the H₂O2 solution.mass of ₂02Vxdj.me of dSince the concentration of the H₂O2 solution is 3% by mass, calculate the massof H₂O2 in the mass determined from the previous part of the 5.00 mL of thesolution.k.=SML x 1.101 g/m2= 5.505gUsing the molar mass of H₂O2, calculate the number of moles of H₂O2reacting.#of molesnovesCLICSPICYmassof H₂02 molar mass=0.165934.0g/mol= 0.00485molUsing stoichiometry and the balanced chemical equation for thedecomposition of H2O2, calculate the number of moles of collected O2.Determine how many grams this is equivalent to.2 H₂022 H₂0 +0₂H₂02:0₂ 2:10.00485 mole of H₂02 = 7 mole of 020.00485 mol 102 x 1 mol 02 -0.002425 moloz2 mol H₂02molar mass 0₂ 32.0 g/molDetermine the gas constant, R.Calculate the % error in R for this determination.mass of 02:0.002425 mol x32.0 g/mol= 0.07769mass of th02-0.1659=2.14 ~ 20.07769equivalent to 2mass of 02Briefly explain why it is essential that none of the yeast comes into contactwith the H₂O2 solution before the stopper is firmly in place.

Mass percentage is defined as the quantity of solute present in 100 g of solution.

Answered: g. Since the concentration of the H₂O2…

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

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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