Please help with question 2. G, H, and I Chem 105 Online1.2.Prelab-Determination of Gas Law Constant Rso the temperature stabilizes to room temperature. Tap water can go inSet up your Chem 105 lab kit tub and fill it up. Be sure to let it sit overnightthis tub.A 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:248.25gpartially fullfull306.03ga.b.C.d.e.Calculate the atmospheric pressure of your environment inmmHg from a weather barometric reading.Calculate the pressure exerted by the collected O2 at thewater temperature. Pota-Po,+PH,o 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.105 Onlinef.g.h.i.j.k.Using the density of H2O2, calculate the mass of 5.00 mL of the H₂O2 solution.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 O2.Determine how many grams this is equivalent to.Determine the gas constant, R.Calculate the % error in R for this determination.Briefly explain why it is essential that none of the yeast comes into contactstopper is firmly in place.

Answered: Image /qna-images/answer/c1731ad1-e530-4016-97bf-cd98b92e315b.jpg

g. h. 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. 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

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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Question

Please help with question 2. G, H, and I

Chem 105 Online
1.
2.
Prelab-Determination of Gas Law Constant R
so the temperature stabilizes to room temperature. Tap water can go in
Set up your Chem 105 lab kit tub and fill it up. Be sure to let it sit overnight
this tub.
A student performed the experiment as described, using 5.00 mL of an
aqueous 3.00% H₂O2 solution, with a density of 1.101 g/mL. The water
temperature was 24.0 °C, and the barometric pressure was 29.34 inches
of Hg. The weights of the gas-collection bottle and water were:
248.25g
partially full
full
306.03g
a.
b.
C.
d.
e.
Calculate the atmospheric pressure of your environment in
mmHg from a weather barometric reading.
Calculate the pressure exerted by the collected O2 at the
water temperature. Pota-Po,+PH,o and the vapor pressure of
H₂O 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 the
volume in Liters of O2 that was obtained?
Convert the water temperature, in Celsius, to Kelvin.
105

Online
f.
g.
h.
i.
j.
k.
Using the density of H2O2, calculate the mass of 5.00 mL of the H₂O2 solution.
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.
Determine the gas constant, R.
Calculate the % error in R for this determination.
Briefly explain why it is essential that none of the yeast comes into contact
stopper is firmly in place.

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