Calculate the solubility of hydrogen in water at an atmospheric pressure of 0.550 atm (a typical value at high altitude).Atmospheric GaskH mol/(L*atm)Mole Fraction7.81 x 1012.10 x 1019.34 x 1033.33 х 1042.00 x 10-65.00 x 107N26.70 x 1041.30 x 1031.40 x 103O2ArCO23.50 x 1021.40 x 1037.80 x 10-4CH4Нм

Total pressure = 0.550 atm Mole fraction of H2 = 5.00×10-7 Henry’s constant (kH) =…

Answered: Calculate the solubility of hydrogen in…

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 12.56QE

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Similar questions

Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density = 0.879 g/cm3). The elevated boiling point of the solution was 355.4 K. What mass of solute was dissolved in the solvent? For the solvent, the enthalpy of vaporization is 33.90 kJ/mol, the entropy of vaporization is 95.95 J/K mol, and the boiling-point elevation constant is 2.5 K kg/mol.
Explain how the unit molarity automatically includes the concept of partial molar volumes.
In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of CO2 was dissolved in the lake at the time. (a) What volume of gas is this at standard temperature and pressure? (b) Assuming that this dissolved gas was in equilibrium with the normal partial pressure of CO2 in the atmosphere (0.038%, or 0.29 torr), use the Henrys law constant for CO2 in water to estimate the volume of Lake Nyos.
The density of a 3.75 M aqueous sulfuric acid solution in a car battery is 1.225 g/mL. Express the concentration of the solution in molality, mole fraction H2SO2, and mass percentage of H2SO4.
Hydrochloric acid is sold as a concentrated aqueous solution. If the concentration of commercial HCl is 12.0 M and its density is 1.18 g/cm3, calculate the following: (a) the molality of the solution (b) the weight percent of HCl in the solution
Determine the mole fraction of acetone in a 1.00 m solution of acetone (CH3COCH3) dissolved in ethanol (CH3CH3OH). The density of acetone is 0.788 g cm–3 and the density of ethanol is 0.789 g cm–3. Enter in decimal form (0.0111, 0.00220, 0.300 etc.)
For the calculation of the solubility c of a gas in a solvent, it is often convenient to use the expression c = Kp, where K is the Henry’s law constant. Breathing air at high pressures, such as in scuba diving, results in an increased concentration of dissolved nitrogen. The Henry’s law constant for the solubility of nitrogen is 0.18 μg/(g H2O atm). What mass of nitrogen is dissolved in 100 g of water saturated with air at 4.0 atm and 20 °C? Compare your answer to that for 100 g of water saturated with air at 1.0 atm. (Air is 78.08 mol per cent N2.) If nitrogen is four times as soluble in fatty tissues as in water, what is the increase in nitrogen concentration in fatty tissue in going from 1 atm to 4 atm?

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