Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 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.arrow_forwardThe 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.arrow_forwardA 6.85 g solution of a certain biomolecule in 100.0 g H2O has a density = 1.024 g/mL. Its osmotic pressure = 4.61 atm at 293.15 K. What is the molar mass of the biomolecule?arrow_forward
- Which of the following statements is false? (No need for explanation) The osmotic pressure of a solution is given by the equation π =CRT ( where C is the molarity of the solution). B. Decreasing order of osmotic pressure for 0.01M aqueous solution of barium chloride, potassium chloride, acetic acid and sucrose. (BaCl2 >KCl>CH3COOH>C12H22O11 ) C. Two different solutions of sucrose of the same molality prepared in different solvents will have the same depression in freezing point. D. According to Raoult’s Law, vapor pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution.arrow_forwardThe partial pressure of CO2, gas above the liquid in a bottle of champagne at 20 °C is 5.2 atm. What is the solubility of CO2, in champagne? Assume the Henry's law constant for CO2, is the same in champagne as it is in water: at 20 °C, kH =3.7 × 10^-2 mol Be sure to use the correct number of significant figures.arrow_forwardA solution contains 1.75 g of a non–volatile, non–electrolyte solute dissolved in 23.47g stearic acid. The freezing point of the solution is 67.2⁰C. The freezing point of pure stearic acid is 69.3⁰C and its freezing point constant, Kfp, is 4.5⁰C kg/mol. What is the molar mass of the solutearrow_forward
- 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?arrow_forwardThe partial pressure of CO2 gas above the liquid in a bottle of champagne at 20°C is 4.3 atm. What is the solubility of CO2 in champagne? Assume the Henry's law constant is the same for champagne as it is for water: at 20°C, kH = 3.7 × 10−2 mol/(L·atm).arrow_forwardThe 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 10.18 grams of aspirin, C9H8O4 (180.1 g/mol), are dissolved in 239.0 grams of diethyl ether.diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.VP(solution) = mm Hgarrow_forward
- The freezing point of ethanol (C2H5OH) is -114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C) of a solution prepared by dissolving 59.1 g of glycerin (C3H8O3, a nonelectrolyte) in 400.0 g of ethanol? The molar mass of ethanol is 46.068 g/mol. Enter your answer with 1 decimal place and no unit. Answer:arrow_forward1. Calculate the molecular weight of a small protein if a 0.55 g sample dissolved in 180 mL of water has an osmotic pressure of 9.2 mmHg at 25°C. (R= 0.0821 L · atm/(K · mol)) 2. What is the molality of a solution that contains 19.16 g of glucose, C6H1206, in 228.5 g of water? (Molar mass of Glucose = 180.00 g/mol)arrow_forwardThe concentration of dissolved argon in water exposed to gaseous argon at a partial pressure of 101.3 kPa at 20 \deg C is 1.5 x 10-3 mol/L. Use Henry's law to determine the solubility of argon when its partial pressure is 50.3 kPa.arrow_forward
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