15. The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35°C with the following results (see graph below, where the blue points represent the values for chloroform and the red points represent the data for acetone). What is the Henry's law constant for acetone in chloroform under these conditions? Vapor Pressure vs. Composition Data for Acetone-Chloroform Pressure (mmHg) 400 350 300 250 200 150 100 50 -50 -100 A) 184 torr B) 254 torr C) 380. torr D) 347 torr E) 177 torr 0.1 ● 0.2 0.3 0.4 0.5 0.6 Mole Fraction of Chloroform 0.7 0.8 0.9

The solubility of Ne in water at 25 °C is 2.1 × 10⁻⁴ M when the partial pressure of Ne is 0.20 atm. What is the value of the Henry's law constant for Ne?

17. The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35 °C with the following results: 0 0 347 0.20 35.3 250 0.40 82.5 175 0.60 142 92.3 XC Pc (torr) PA (torr) What is the Henry's law constant for chloroform in this system? A) 365 torr B) 347 torr C) 177 torr D) 273 torr E) 485 torr 0.80 200 36.8 1 273 0

cvg.cengagenow.com OWLV2 | Online teaching and learning resource from Cengage Learning [Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of chloroform, CHCl3, is 61.70 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in chloroform is estrogen (estradiol). A student dissolves 11.36 grams of estrogen, C₁8H24 O2 (272.4 g/mol), in 170.7 grams of chloroform. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3 CH₂OH CHC13 C6H6 Diethyl ether CH3 CH2 OCH2 CH3 The molality of the solution is The boiling point of the solution is Kb (°C/m) Kf (°C/m) 0.512 1.86 1.22 1.99 3.67 2.53 2.02 m. °C. 5.12 +88

At a certain temperature the vapor pressure of pure benzene and pure toluene are 380 torr and 130 torr, respectively. If the mole fraction of benzene is 0.48, what is the total vapor pressure.

An experiment conducted at 20 oC requires an atmosphere in which the partial pressure of water is a constant 10.0 torr. The experiment will be conducted inside a sealed container in which there is a beaker containing a solution of ethylene glycol (FW 62.07) and water (FW 18.02). At 20 oC, the vapor pressure of pure ethylene glycol is 0.056 torr and that of pure water is 17.3 torr. What mass of ethylene glycol must be mixed with 200. g water to produce a solution with a 10.0 torr vapor pressure of water? (Report the answer to three significant figures.)

Henry's law constant for carbon dioxide dissolving in water is 3.5*10^-2 mol/L*atm at 20 degrees celsius. What is the maximum molar concentration of carbon dioxide in a pond at this temperature ? The mole fraction of CO2 in air is 3.14*10^-4