PRINCIPLES OF MODERN CHEMISTRY-OWLV2
8th Edition
ISBN: 9781305271609
Author: OXTOBY
Publisher: CENGAGE L
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At 25°C, some water is added to a sample of gaseousmethane (CH4) at 1.00 atm pressure in a closed vessel, andthe vessel is shaken until as much methane as possible dissolves. Then 1.00 kg of the solution is removed and boiledto expel the methane, yielding a volume of 3.01 L ofCH4(g) at 0°C and 1.00 atm. Determine the Henry’s lawconstant for methane in water.
Henry s law is important in environmental chemistry, where it predicts the
distribution of pollutants between water and the atmosphere. The hydrocarbon
methylacetylene (C3H4) emitted in wastewater streams, for example, can pass into
the air, where it is degraded by processes induced by light from the sun.
The Henry s law constant for methylacetylene in water at 25 °C is 601 atm, when
the following form of the law is used:
= k
methylacetylene
Calculate the partial pressure of methylacetylene vapor in equilibrium with a
solution of 1.47 g of methylacetylene per 1060 L of water. How many
methylacetylene molecules are present in each cubic centimeter of vapor?
P
methylacetylene methylacetylene
methylacetylene
X
=
atm
molecules per cubic centimeter
The partial pressure of CO2 gas above the liquid in a bottle of champagne at 20°C is 5.5 atm. What is the solubility of CO2 in champagne? Assume Henry’s law constant is the same for champagne as for water: at 20°C, kH = 3.7 x 10-2 mol/L⋅atm.
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- Heat is released when some solutions form; heat is absorbed when other solutions form. Provide a molecular explanation for the difference between these two types of spontaneous processes.arrow_forwardIn 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.arrow_forward14. Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies. Which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute- solvent interactions are the same for both solids. (A) The solid with the larger lattice energy, if entropy increases as a result of mixing, and the solid with the smaller lattice energy, if entropy decreases as a result of mixing. (B) The solid with the smaller lattice energy, if entropy increases as a result of mixing, and the solid with the larger lattice energy, if entropy decreases as a result of mixing. (C) The solid with the smaller lattice energy. (D) The solid with the larger lattice energy. (E) They will have the same or very similar solubilities.arrow_forward
- Mm.9.arrow_forwardOsmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mLarrow_forwardThe commercially available soda (water and CO2) siphon uses one 8-gram cartridge of carbon dioxide CO2 to make about 1 liter of soda. In the so-prepared soda bottle, pressure is about 6 atm. However, carbonated drinks are produced in larger bottles. For example, Coca-Cola is sometimes bottled in 5-gallon jugs: Assume that Coca-Cola drink contains the same concentration of dissolved CO2 as soda. Using the Henry law, estimate the molar concentration of CO2 in the Coca-Cola drink in the jug at 25 ºC.arrow_forward
- f dissolving 1.5 g of a solute into 100 mL of water caused the temperature of the solution toincrease by 4.7 ⁰C, what would the change of temperature be if 3.0 g of the solute were dissolvedin the same volume of water? Explain.arrow_forwardwhat is the molar mass of toluene if 0.85g of toluent depresses freezing pt 1.00 x102 g of benzene by 0.47 degrees C; Kf=5.12degrees C/m.arrow_forwardIn a study designed to prepare new gasoline-resistant coat-ings, a polymer chemist dissolves 6.053 g of poly(vinyl alcohol)in enough water to make 100.0 mL of solution. At 25°C, the os-motic pressure of this solution is 0.272 atm. What is the molar mass of the polymer sample?arrow_forward
- Suppose the change in temperature of solution is −9.84°C (∆Tfreezing = 9.84°C). The unknown solute consists of 0.404g. The mass of the solvent is 14.65g of t-Butanol. What is the molar mass of the solute. Assume the solute is organic kf,t-butanol = 9.1°C•kg/molarrow_forwardA chemistry student is given 5.00 L of a clear aqueous solution at 25.° C. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 15.° C. At that point, the student sees that a precipitate has formed. He transfers the liquid to a clean new beaker and throws away the precipitate. The student then evaporates the water from the liquid in the new beaker under vacuum. It weighs 1.00 kg. Using only the information above, can you calculate the solubility of Xin water at 15.° C ? If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits. 0 yes no ☐ x10 X Olo S U 2arrow_forwardLattice enthalpy for NaCl is +788 kJ mol¹ and AH = -784 kJ mol¹. Enthalpy of Hyd solution of NaCl isarrow_forward
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