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2. 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 a. b. C. 248.25g 306.03g 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. Ptotal Po,+PH₂O and the vapor pressure of H₂O at 24 °C = 22.4 mm Hg) Convert this pressure to atmospheres OR kPa.

2. 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 a. b. C. 248.25g 306.03g 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. Ptotal Po,+PH₂O and the vapor pressure of H₂O at 24 °C = 22.4 mm Hg) Convert this pressure to atmospheres OR kPa.

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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Please help with question 2 a, b, and c
1. 2. 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 a. b. e. C. d. 248.25g 306.03g 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. Ptotal=Po₂+PH₂o 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.
Transcribed Image Text:1. 2. 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 a. b. e. C. d. 248.25g 306.03g 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. Ptotal=Po₂+PH₂o 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.
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