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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A compound contains 42.9%C,2.4%H,16.6%N, and 38.1%O by mass. The addition of 3.16 g of this compound to 75 mL of cyclohexane (density is 0.779 g/mL) gives a solution with a freezing point of 0°C. The normal freezing point of cyclohexane is 6.5°C and its freezing point depression constant is 20.2°C/m. What is the empirical mass? A. 84 g/mol B. 88 g/mol C. 36 g/mol D. 55 g/mol E. 98 g/mol F. 44 g/mol
Pure napthalene freezes at 80.6oC and has a freezing point depression constant of 6.9oC/m. The freezing point of a solution containing 7.27 g of an unknown non-ionizing compound in 62.18 g of napthalene is 69.5oC. What is the molar mass of the unknown compound?
A solution consisting of 0.240 mol of methylbenzene, C6H5CH3, in 252 g of nitrobenzene, C6H5NO2, freezes at –0.7°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?
At a particular temperature, the solubility of CO₂ in water is 0.13 M when the partial pressure is 1.5 atm. What partial pressure (in atm) of CO₂ would give a solubility of 0.078 M?
The Henry's law constant for O2 is 1.3 x 10° mol · L. atm at 25°C. (a) What is the concentration of O2 in water at 25°C if the partial pressure of O2 in the atmosphere is 0.21 atm? Express concentration: (i) in mol/L, and (ii) in ppm (by mass). (b) How many grams of O2 is dissolved in water in a 1.0 x 10ʻ- L capacity aquarium? (Assume density of solution is 1.0 g/mL).
A compound contains 42.9%C,2.4%H,16.6%N, and 38.1%O by mass. The addition of 3.16 g of this compound to 75 mL of cyclohexane (density is 0.779 g/mL) gives a solution with a freezing point of 0°C. The normal freezing point of cyclohexane is 6.5°C and its freezing point depression constant is 20.2°C/m. What is the molecular mass? A. 98 g/mol B. 125 g/mol C. 168 g/mol D. 178 g/mol E. 207 g/mol F. 150 g/mol
Use Raoult's Law to determine the vapor pressure of a solution at 55°C that contains 34.2 grams of sodium chloride in 375 grams of water. The par pressure of pure water at 55°C is 118.1 torr. Assume 100% dissociation of the solute. 871 to 115 torr
1.) The vapor pressure of pure acetone, (CH3)2CO, at 250C is 229 torr. A.) Calculate the vapor pressure of acetone in a 42.0 mol % solution in water. B.) the vapor pressure of acetone in this solution is 164 torr at 250C. Is the deviation from Raoult's law positive or negative?
How many grams of NaOH must be added to 300ml of water at 48°C to have a solution whose vapor pressure is 78 torr. (Vapor pressure of H2O at 48°c is 83.7 torr)
At 45 °C, a solution is prepared by mixing 48.0 g Na2SO4 with 240.0 g water. The vapor pressure of water at 45 °C is 71.9 torr. Assuming total dissociation of the salt, determine: (a) mole fraction of Na2SO4; (b) mole fraction of water; (c) vapor pressure of the solution. (molar mass, g/mol: Na2SO4= 142.04; water = 18.02) (a) XNa2s04 = (b) Xwater = (d) Psoln =
In a solution of acetone and water, the mole fraction of water is 0.573. If the vapor pressure of pure water and pure acetone at 25 ºC are 23.8 mmHg and 51.2 mmHg, respectively, what is the mole fraction of water in the vapor phase. Give your answer to three sig figs.
Calculate the solubility of O, in water at a partial pressure of O2 of 120 torr at 25°C. The Henry's law constant for 0, is 1.3 x 10-8 mol/L· atm for Henry's law in the form C= kP, where Cis the gas concentration (mol/L).

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