The partial pressure of CO, in air is approximately 4.0 10 4 3.2 x 10 mol/(L-atm) to find the concentration of CO, in atm. If the Henry's-law constant is Part A A can of soda under a CO, pressure of 24 atm at 25 "C Express your answer to two significant figures and include the appropriate units. MA Value Units Enter your answer using unts of chemical concentration No credit lost. Tty again Submit Ereis Answers Request Answer The partial pressure of CO, in air is approximately 4.0 10 atm. If the Henry's-law constant is 3.2 x 10 mol/(L atm) to find the concentration of CO, in Enter your answer using unts of chemical concentration No credit lost Try again Submit Previous Answern Request Answr Part B A can of soda open to the atmosphere at 25 "C Express your answer to two significant figures and include the appropriate units Value Units Submit RestAnser

The partial pressure of CO, in air is approximately 4.0 10 4 3.2 x 10 mol/(L-atm) to find the concentration of CO, in atm. If the Henry's-law constant is Part A A can of soda under a CO, pressure of 24 atm at 25 "C Express your answer to two significant figures and include the appropriate units. MA Value Units Enter your answer using unts of chemical concentration No credit lost. Tty again Submit Ereis Answers Request Answer The partial pressure of CO, in air is approximately 4.0 10 atm. If the Henry's-law constant is 3.2 x 10 mol/(L atm) to find the concentration of CO, in Enter your answer using unts of chemical concentration No credit lost Try again Submit Previous Answern Request Answr Part B A can of soda open to the atmosphere at 25 "C Express your answer to two significant figures and include the appropriate units Value Units Submit RestAnser

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 66QAP: The Henry's law constant for the solubility of radon in water at is 9.57106 M/mm Hg. Radon is...

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The Henry's law constant for the solubility of radon in water at is 9.57106 M/mm Hg. Radon is present with other gases in a sample taken from an aquifer at 30C. Radon has a mole fraction of 2.7106 in the gaseous mixture. The gaseous mixture is shaken with water at a total pressure of 28 atm. Calculate the concentration of radon in the water. Express your answers using the following concentration units. (a) molarity (b) ppm (Assume that the water sample has a density of 1.00 g/mL.)
Determine the value of the Henry's law constant, k, (mol/L·atm) of an unnamed gas where the concentration is 0.0350 M under a partial pressure of 1.55 atm and 0.0384 M under a partial pressure of 1.70 atm at the same temperature. Report your answer to the thousandths place. Do not include units.
Hydrogen gas has a Henry's law constant of 7.8 x 10-4 mol/kg bar at 25 degrees C when dissolving in water. If the total pressure of gas (H2 gas plus water vapor) over water is 1.00 bar, what is the concentration of H2 in the water in grams per mililiter? _ g/mL
ITEMS USED FOR EXPERIMENT: •Ring stand •Hot plate •125 mL Erlenmeyer flask•400 mL beaker•10 mL graduated cylinder •Aluminum foil•Rubberband•Paper Clip•Thermometer•Vial containing unknown liquid You know have the following data: Mass of flask + foil + rubberband: 78.637 gMass of flask + foil and rubberband+ unknown condensed liquid: 78.847 gTemperature of water bath: 100C = 373 KPressure of gas in our system: 29.02 inHg = 0.9699 atmVolume of gas in our system: 141 mL = 0.141 L 1. During the experiment, you collect the following data: Mass of flask: 80.001 g Mass of flask + unknown condensed liquid: 80.452 g Temperature of water bath: 100 °C Pressure of gas in our system: 0.998 atm Volume of gas in our system: 265 mL Which of the following number(s) need a conversion before they can be used? (Check all that apply) [ ] Group of answer choices [ ] Volume of gas in our system [ ] Mass of flask [ ] Temperature of water bath [ ] Pressure of gas in our system [ ] Mass of flask +…
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The active ingredient of Benadryl© Chesty Forte Cough Liquid is Guaiphenesin anexpectorant drug used to assist the expectoration ('bringing up') of phlegm from theairways in acute respiratory tract infections. A 200.0 mL bottle of Benadryl© ChestyForte Cough contains 4.00 g of Guaiphenesin (C10H14O4). i. If the recommended dose for a child is 150 mg of Guaiphenesin. What volume of thecough liquid should be administered? ii. If the recommended dose for an adult is 350 mg of Guaiphenesin. How many molesof Guaiphenesin does this equal?
The active ingredient of Benadryl© Chesty Forte Cough Liquid is Guaiphenesin anexpectorant drug used to assist the expectoration ('bringing up') of phlegm from theairways in acute respiratory tract infections. A 200.0 mL bottle of Benadryl© ChestyForte Cough contains 4.00 g of Guaiphenesin (C10H14O4). i. If the recommended dose for a child is 150 mg of Guaiphenesin. What volume of thecough liquid should be administered? ii. If the recommended dose for an adult is 350 mg of Guaiphenesin. How many molesof Guaiphenesin does this equal? (answer to 2 significant figures)
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Air, contalning nitrogen gas, used to bubble water home aquariums. In a total pressure of 1 atm of air, the mole fraction of nitrogen 0.78. From this information, determine the mass of nitrogen gas (In grams) that will be soluble in a 80.0 L home aquarium filled with water at 25 degrees * C . Henry's constant for nitrogen gas water at 25°C is 6.1 * 10 ^ - 4 * M / a * t * m Note : Report your answer to two significant figures and include the abbreviated form of the unit in your answer Answer (Mass of nitrogen gas dissolved in aquarium )