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d. Using the assumption that 1gram of water is 1mL of volume, what is the volume in Liters of O2 that was obtained?

d. Using the assumption that 1gram of water is 1mL of volume, what is the volume in Liters of O2 that was obtained?

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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1. 2. d. e. C. Prelab-Determination of Gas Law Constant R Set up your Chem 105 lab kit tub and fill it up. Be sure to let it sit overnight so the temperature stabilizes to room temperature. Tap water can go in 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: partially full full b. a. Calculate the atmospheric pressure of your environment in mmHg from a weather barometric reading. linch=25.4mm 29.34 in Hgx- 248.25g 306.03g 25.4mm=745.236 mm Hg lin Atmospheric pressure = 745mmHg Calculate the pressure exerted by the collected O2 at the water temperature. Ptotal Po,+PHo and the vapor pressure of H₂O at 24 °C = 22.4 mm Hg) Po₂ = Protal-PH₂D Poz=745.236 mm Hg -22.4mm Hg Poz=722.836 mmHg Pressure of O₂ = 723 mm Hg Convert this pressure to atmospheres OR kPa. 1 atm = 760 mm Hg 723 mmHg x atm = 0.95latm 760 mmHg Pressure in atmospheres=0.951 atm 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. K=C+273.15 24°c +273.15-297.15 k
Transcribed Image Text:1. 2. d. e. C. Prelab-Determination of Gas Law Constant R Set up your Chem 105 lab kit tub and fill it up. Be sure to let it sit overnight so the temperature stabilizes to room temperature. Tap water can go in 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: partially full full b. a. Calculate the atmospheric pressure of your environment in mmHg from a weather barometric reading. linch=25.4mm 29.34 in Hgx- 248.25g 306.03g 25.4mm=745.236 mm Hg lin Atmospheric pressure = 745mmHg Calculate the pressure exerted by the collected O2 at the water temperature. Ptotal Po,+PHo and the vapor pressure of H₂O at 24 °C = 22.4 mm Hg) Po₂ = Protal-PH₂D Poz=745.236 mm Hg -22.4mm Hg Poz=722.836 mmHg Pressure of O₂ = 723 mm Hg Convert this pressure to atmospheres OR kPa. 1 atm = 760 mm Hg 723 mmHg x atm = 0.95latm 760 mmHg Pressure in atmospheres=0.951 atm 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. K=C+273.15 24°c +273.15-297.15 k
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