. In an ideal solution of liquids A and B, the vapor pressure of amixture of 0.60 mol of A and 2.4 mol of B is 0.42 atm at 70°C.1.80 moles of A is added to the solution at 70°C and the vaporpressure of the solution rises to 0.55 atm. Calculate the vaporpressure if some of the vapor in equilibrium with the first solutionwere completely condensed.a. 0.51 atmb. 0.35 atmc. 0.20 atmd. 0.80 atm

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Answered: . In an ideal solution of liquids A and…

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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135 g of acetone ( C3H6O) and 265 of water are mixed at 20. Find the vapor pressure of this solution. Water vapor pressure = 25 torr at 20C.
A solution is made by mixing 100.0 g acetone (CH3COCH3) and 100.0 g methanol (CH3OH). a. What is the vapor pressure of this solution at 25C? b. What is the composition of the vapor expressed as a mole fraction? Assume ideal solution and gas behavior. (At 25 C the vapor pressures of pure acetone and pure methanol are 271 and 143 torr, respectively.) The actual vapor pressure of this solution is 161 torr. Explain any discrepancies.
How many of the following statements is/are true. A. The vapor pressure of a solvent over a solution decreases as the mole fraction of the solvent increases in the solution. В. The solubility of a gas increases as the temperature increases. С. The vapor pressure of a solvent over a solution is less than that of pure solvent. D. The greater the pressure of a gas over a solution the greater its solubility. E. lonic solutes dissociate in solution causing an enhancement of all colligative properties. O 5 3 1 О 2 O 4
A dilute solution of bromine in carbon tetrachloride behaves as an ideal-dilute solution. The vapor pressure of pure CCI4 is 33.85 torr at 298 K. The Henry's Law constant when the concentration of Br2 is expressed as a mol fraction is 122.36 torr. Calculate the mole fraction of Br2 in the vapor when it's in equilibrium with a solution that has a mole fraction of Br2 equal to 0.050, having the assumption that the vapor still behaves as an ideal gas.
The vapor pressures of pure benzene and pure toluene at 25°C are 95.1 and 28.4 mmHg, respectively. Which of the below ideal solutions made by mixing different ratios of benzene and toluene has the lowest total vapor pressure at 25°C?Select one: a.1/1 benzene to toluene b.1/8 benzene to toluene c.1/2 benzene to toluene d.8/1 benzene to toluene e.2/1 benzene to toluene
We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 23.76 Hg to 22.5 Hg at 25°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the boiling point of this solution? (Hint: find the molality first, and for water, kb = .510 m/°C; boiling point of water: 100.0°C.)
1. A 4.0mg sample of a certain protein is dissolved in 20.0mL solution. The solution exhibits an osmotic pressure of 1.18orr at 25°C. Calculate the molecular weight of that protein
Using butanol (C4H9OH) rather than ethanol (C₂H5OH) as a gasoline additive has an advantage in providing a higher fuel value when mixed with octane. V At 20°C, the vapor pressure of butanol is 5.00 torr and the vapor pressure of octane is 10.0 torr. What is the vapor pressure at 20°C of a solution prepared by mixing 16.2 g of butanol and 127 g of octane? torr
The vapor pressure of pure water at 25 °C is 23.76 mm Hg. Calculate the vapor pressure of a solution prepared by mixing 125 g of sucrose (C12H22011) in 500 g H20

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