10:47Henry's Law Explained - Gas Solubility & Partial Pressure - Chemistry ProblemsThe Organic Chemistry Tutor875views
Multiple ChoiceHenry's Law Constant for nitrogen in water is 1.67 × 10-4 M • atm–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?1652views2rankHas a video solution.
Multiple ChoiceAt 0°C and 1.00 atm, as much as 0.84 g of O2 can dissolve in 1.0 L of water. At 0°C and 4.00 atm, how many grams of O2 dissolve in 1.0 L of water?1352views1rankHas a video solution.
Multiple ChoiceThe atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry's Law Constant for oxygen in water at this temperature is 5.3 × 10–5 M/atm.1143views6rankHas a video solution.
Multiple ChoiceWhat would be the vapor pressure at 25.0 °C of a solution of 5.00 g of glucose (C6H12O6) in 100.0 g of ethanol (C2H5OH)? Pure ethanol has a vapor pressure of 54.68 mmHg at 25 °C.157views
Multiple ChoiceAt 25 °C, the solubility of O2 is 4.55 × 10−3 M at 3.5 atm pressure. What is the solubility of O2 at the same temperature and at 2.0 atm pressure?138views
Textbook QuestionA scuba diver is breathing compressed air that is 21% (by volume) oxygen at a depth of 66 ft. beneath the surface. The total pressure at this depth is 3.0 atm. The Henry's law constant (k) for O2 in water at a normal body temperature (37 °C ) is 1.93 * 10-3 mol>(L atm). What is the solubility of O2 in the blood of the diver at 66 ft. beneath the surface? (LO 13.9) (a) 1.22 * 10-3 M (b) 2.76 * 10-2 M (c) 1.22 * 10-1 M (d) 2.76 * 10-1 M538viewsHas a video solution.
Textbook QuestionFish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure of oxygen above the water in atmospheres at 0 °C is needed to obtain this concentration? The solubility of O2 in water at 0 °C and 1 atm partial pressure is 2.21 * 10-3 mol>L.610viewsHas a video solution.
Textbook QuestionAt an altitude of 10,000 ft, the partial pressure of oxygen in the lungs is about 68 mm Hg. What is the concentration in mg/L of dissolved O2 in blood (or water) at this partial pres- sure and a normal body temperature of 37 °C? The solubil- ity of O2 in water at 37 °C and 1 atm partial pressure is 1.93 * 10-3 mol>L.593viewsHas a video solution.
Textbook QuestionThe Henry's law constant for CO2 in water at 25 °C is 3.1x10^-2 M atm-1. (a) What is the soubility of CO2 in water at this temperature if the soltuion is in contact with air at normal atmospheric pressure?11170viewsHas a video solution.
Textbook QuestionMost fish need at least 4 ppm dissolved O2 in water for survival. (b) What partial pressure of O2 above water is needed to obtain 4 ppm O2 in water at 10 °C? (The Henry's law constant for O2 at this temperature is 1.71 * 10-3 mol>L@atm.)436viewsHas a video solution.
Textbook QuestionThe presence of the radioactive gas radon (Rn) in well water presents a possible health hazard in parts of the United States. (a) Assuming that the solubility of radon in water with 1 atm pressure of the gas over the water at 30 °C is 7.27 * 10-3 M, what is the Henry's law constant for radon in water at this temperature?422views1rankHas a video solution.
Textbook QuestionA saturated solution forms when 0.0537 L of argon, at a pressure of 1.0 atm and temperature of 25 °C, is dissolved in 1.0 L of water. Calculate the Henry's law constant for argon.1243views1commentsHas a video solution.
Textbook QuestionA gas has a Henry's law constant of 0.112 M>atm. What total volume of solution is needed to completely dissolve 1.65 L of the gas at a pressure of 725 torr and a temperature of 25 °C?1894views2rankHas a video solution.
Textbook QuestionAt ordinary body temperature 137 °C2, the solubility of N2 in water at ordinary atmospheric pressure (1.0 atm) is 0.015 g>L. Air is approximately 78 mol % N2. (b) At a depth of 100 ft in water, the external pressure is 4.0 atm. What is the solubility of N2 from air in blood at this pressure?1051views1commentsHas a video solution.
Open QuestionAt 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen.172viewsHas a video solution.
Open QuestionAt 298 k, the Henry's law constant for oxygen is 0.00130 m/atm. Air is 21.0% oxygen. at 298 k, what is the solubility of oxygen in water exposed to air at 1.00 atm?56viewsHas a video solution.
Open QuestionAt 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm?188viewsHas a video solution.