Please help with question 2G-I nerown. Youhe water Inside thequal to the leveldmixture's pressunpressure. You wize the pressureHe!2A student performed the experiment as described, using 5.00 mL of anaqueous 3.00% H₂O2 solution, with a density of 1.101 g/mL. The watertemperature was 24.0 °C, and the barometric pressure was 29.34 inchesof Hg. The weights of the gas-collection bottle and water were:partially fullfulla.b.C.e.d.248.25g306.03gCalculate the atmospheric pressure of your environment inmmHg from a weather barometric reading.Calculate the pressure exerted by the collected O2 at thewater temperature. Proto-Po,+PHO and the vapor pressure ofH₂O at 24 °C = 22.4 mm Hg)Convert this pressure to atmospheres OR kPa.Using the assumption that 1gram of water is 1mL of volume, what is thevolume in Liters of O2 that was obtained?Convert the water temperature, in Celsius, to Kelvin. g.h.i.j.k.Since 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.Using the molar mass of H₂O2, calculate the number of moles of H₂O₂reacting.Using stoichiometry and the balanced chemical equation for thedecomposition of H₂O2, calculate the number of moles of collected 02.Determine how many grams this is equivalent to.Determine the gas constant, R.Calculate the % error in R for this dots

g.) Using mas percent and madd of solution we can calculate mass of H2O2 . h ) Using mass and molar…

g. h. i. 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. Using the molar mass of H₂O2, calculate the number of moles of H₂O2 reacting. 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.

g. h. i. 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. Using the molar mass of H₂O2, calculate the number of moles of H₂O2 reacting. 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.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 141QRT

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