13.37 The Henry's law constant for helium gas in water at 30°Cis 3.7 x 10 M/atm and the constant for N2 at 30 °C is6.0 x 10 M/atm. If the two gases are each present at 1.5S0latm pressure, calculate the solubility of each gas.

Henry’s law constant (k) of He is 3.7×10-4 M/atm. Solubility of He can be determined using Henry’s…

Answered: 13.37 The Henry's law constant for…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.51QE

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To make homemade ice cream, you cool the milk and cream by immersing the container in ice and a concentrated solution of rock salt (NaCl) in water. If you want to have a water-salt solution that freezes at 10. C, what mass of NaCl must you add to 3.0 kg of water? (Assume the vant Hoff factor, i, for NaCl is 1.85.)
The Henry's law constant for the solubility of helium gas in water is 3.8104M/atm at 25C. (a) Express the constant for the solubility of helium gas in M/mm Hg. (b) If the partial pressure of He at 25C is 293 mm Hg, what is the concentration of dissolved He in mol/L at 25C? (c) What volume of helium gas can be dissolved in 10.00 L of water at 293 mm Hg and 25C? (Ignore the partial pressure of water.)
Silver ion has an average concentration of 28 ppb (parts per billion) in U.S. water supplies. (a) What is the molality of the silver ion? (b) If you wanted 1.0 102 g of silver and could recover it chemically from water supplies, what volume of water in liters would you have to treat? (Assume the density of water is 1.0g/cm3.)
Reserpine is a natural product isolated from the roots of the shrub Rauwolfia serpenlina. It was first synthesized in 1956 by Nobel Prize winner R. B. Woodward. It is used as a tranquilizer and sedative. When 1.00 g reserpine is dissolved in 25.0 g camphor, the freezing-point depression is 2.63C (Kr for camphor is 40.C kg/mol). Calculate the molality of the solution and the molar mass of reserpine.
What is the usual solubility behavior of an ionic compound in water when the temperature is raised? Give an example of an exception to this behavior.
Juice (d=1.0g/mL) from freshly harvested grapes has about 24% sucrose by mass. What is the molality of sucrose, C12H22O11, in the grape juice after 25% (by mass) of the water content has been removed? Assume a volume of 15.0 L.
A 0.029 M solution of potassium sulfate has an osmotic pressure of 1.79 atm at 25 C. (a) Calculate the vant Hoff factor, i, for this solution. (b) Would the vant Hoff factor be larger, smaller, or the same for a 0.050 M solution of this compound?
An aqueous solution of sodium bromide freezes at 1.61 C. What is the total molality of solute particles? How many grams of sodium bromide are present in 1 kg of water? (Assume an ideal value for the vant Hoff factor.)
An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25 C. (a) What is the average molar mass of starch? (The result is an average because not all starch molecules are identical.) (b) What is the freezing point of the solution? Would it be easy to determine the molecular weight of starch by measuring the freezing point depression? (Assume that the molarity and molality are the same for this solution.)
The freezing point of a 0.031-m solution of copper(II) sulfate in water is 0.075 C. (a) Calculate the vant Hoff factor, i, for this solution. (b) Would the vant Hoff factor be larger, smaller, or the same for a 0.050-m solution of this compound?
A compound contains 42.9% C, 2.4% H, 16.6% N, and 38.1% O. The addition of 3.16 g of this compound to 75.0 mL of cyclohexane (d=0.779g/mL) gives a solution with a freezing point at 0.0C. Using Table 10.2, determine the molecular formula of the compound.
A carbonated beverage is made by saturating water with carbon dioxide at 0C and a pressure of 3.0 atm. The bottle is then opened at room temperature (25C), and comes to equilibrium with air in the room containing CO2(PCO2=1.0103M/atm). The Henry's law constant for the solubility of CO2 in water is 0.0769 M/atm at 0C and 0.0313 M/atm at 25C. (a) What is the concentration of carbon dioxide in the bottle before it is opened? (b) What is the concentration of carbon dioxide in the bottle after it has been opened and come to equilibrium with the air?

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13.37 The Henry's law constant for helium gas in water at 30°C is 3.7 x 10 M/atm and the constant for N2 at 30 °C is 6.0 x 10 M/atm. If the two gases are each present at 1.5 S0latm pressure, calculate the solubility of each gas.