1/5At 24.55 °C the vapor pressure of pure water is PH20 = 54.07 mmHg. Calculate the amount (in grams) of a non-dissociating solute (molar mass = 137.18) that when added to286.852 g of water will reduce the vapor pressure by 5.45 mmHg when compared with pure water at the same temperature.(The answer should be given with three numbers after the decimal; example 25.143)Molar mass of water = 18.02 g/molR = 0.08206 atm-L/mol-K0 °C = 273.15 K1.0000 atm =760.00 mmHgType your answer..Next

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Answered: 1/5 1 At 24.55 °C the vapor pressure of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Methane has a Henry's Law constant (k) of 9.88 x 10-2 mol/(L·atm) when dissolved in benzene at 25°C. How many grams of CH4 will dissolve in 1.00 L of benzene if the partial pressure of CH4 is 1.48 atm? (Molar mass of CH4 = 16.042 g/mol) O 0.146 g O 0.0667 g O 2.35 g O 4.83 g none of these
Calculate the freezing point of an 0.260 m aqueous solution of lithium perchlorate (LiClO4). The freezing point of pure water is 0.00 oC and the Kf of water is 1.86 oC/m.
The vapor pressure of pure water at 70°C is normally 233.7 mmHg, but decreased to 227.4 mmHg upon addition of an unknown amount of sodium hypochlorite, NaOCl, to 242.9 g of water at this temperature. How many grams of sodium hypochlorite were added? Assume complete dissociation of solute.
At 20.0 °C, the vapor pressure of cyclohexane, a nonpolar hydrocarbon, is 66.9 torr and that of toluene, a hydrocarbon related to benzene, is 21.1 torr. What is the vapor pressure of a solution of the two at 20.0 °C when toluene is present at a mole fraction of 0.156?Ptotal =? torr
The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is aspirin.Calculate the vapor pressure of the solution at 25 °C when 10.17 grams of aspirin, C9H8O4 (180.1 g/mol), are dissolved in 151.7 grams of diethyl ether.diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol. The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25°C.How many grams of estrogen (estradiol), C18H24O2, a nonvolatile, nonelectrolyte (MW = 272.4 g/mol), must be added to 192.1 grams of diethyl ether to reduce the vapor pressure to 452.63 mm Hg ?diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.
When 16.3 g of an organic compound known to be 57.15% C, 4.8% H, and 38.06% O by mass is dissolved in 700.7 g of water, the freezing point is −0.343⁢ ∘C. The normal freezing point of water is 0⁢ ∘C. What is the molecular formula for the organic compound? Assume that the organic compound is a molecular solid and does not ionize in water. ?f values for various solvents are given in the colligative constants table.
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Exactly 9.96 g of an unknown substance is dissolved in 2.50 x 102 g water. The freezing point of this solution is found to be -1.93 ° Calculate the molar mass of the unknown substance in g/mol. The kf of water is 1.86 °C/m.
An ideal solution contains 0.1279 mol H2O and an unknown number of moles of urea (nonelectrolyte, (NH2)2CO, MM = 60.056 g mol–1). The vapor pressure of the solution at 30.0 °C is 25.7 torr. The vapor pressure of pure water at this temperature is 31.8 torr. Calculate the number of grams of urea in the solution. P1 = X1Po1
A) The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is DDT.Calculate the vapor pressure of the solution at 25 °C when 8.376 grams of DDT, C14H9Cl5 (354.5 g/mol), are dissolved in 227.7 grams of diethyl ether.diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.VP(solution) = mm Hg B) The vapor pressure of water is 23.76 mm Hg at 25°C. How many grams of glucose, , a nonvolatile, nonelectrolyte (MW = 180.2 g/mol), must be added to 256.7 grams of water to reduce the vapor pressure to 23.49 mm Hg? water = H2O = 18.02 g/mol. Mass = g
What is the mole fraction of acetone, C3H6O, in the vapor phase from a solution consisting of a mixture of acetone and ethyl acetate, CH3COOCH2CH3, at 30.00 °C, if the total pressure above the solution is 202.2 torr? The vapor pressures of pure acetone and NaN at 30.00 °C are 285.0 torr and 118.0 torr, respectively.
The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is aspirin.Calculate the vapor pressure of the solution at 25 °C when 10.17 grams of aspirin, C9H8O4 (180.1 g/mol), are dissolved in 151.7 grams of diethyl ether.diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol. The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25°C.How many grams of estrogen (estradiol), C18H24O2, a nonvolatile, nonelectrolyte (MW = 272.4 g/mol), must be added to 192.1 grams of diethyl ether to reduce the vapor pressure to 452.63 mm Hg ?diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.

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