4. The vapor in equilibrium with a solution of ethanol (eth) and 0.9900 has a pressure of chloroform (chl) at 45°C with Xh 438.59 torr and has Xchl.(g) assumed to be essentially ideally dilute. a. Find the vapor-phase partial pressures. b. Calculate the vapor pressure of pure chloroform at 45°C. = chl (1) 0.9794. The solution can be

4. The vapor in equilibrium with a solution of ethanol (eth) and 0.9900 has a pressure of chloroform (chl) at 45°C with Xh 438.59 torr and has Xchl.(g) assumed to be essentially ideally dilute. a. Find the vapor-phase partial pressures. b. Calculate the vapor pressure of pure chloroform at 45°C. = chl (1) 0.9794. The solution can be

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...

See similar textbooks

Similar questions

A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal places
Show work
5. At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene if Xenzene = 0.620.
Shown below is a plot of the solubility of benzoic acid in water as a function of temperature. Estimate the Solubility (Constant) Sof benzoic acid at 60°C (include units!) Solubility of Benzoic Acid in Moles/Liter in Water as a Function of Temperature 0.12 Moles per Liter 0.1 0.08 0.06 0.04 0.02 20 0.092 moles/liter If you have trouble viewing this image Click to open: 0.04 moles/liter 0.06 moles/liter 30 1.34 moles/liter 50 40 Degrees Centigrade 60 70
Lithium chloride has a solubility of 45.80 g in 100. g of water at 25°C. Express this solubility in terms ofmass percent molality mole fraction
Potassium Dichromate molar mass-294.185g/mol c at saturation-0.510mol/L solubility-576.833 Ksp-?
b) Determine the freezing point of 500 g antifreeze, C2H6O2 in 2.5 kg of water. Given Kf for water is 1.86 °C.m-1.
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
The following data table indicates the solubility of a substance. By examining the data presented, predict the solubility of the substance at 50 oC. Temperature (oC) Solubility (mM) 5 5.00 15 4.35 25 3.70 35 3.05 45 2.40
Shown below is a plot of the solubility of benzoic acid in water as a function of temperature. Estimate the Solubility (Constant) S of benzoic acid at 60°C (include units!) Solubility of Benzoic Acid in Moles/Liter in Water as a Function of Temperature 0.12 Moles per Liter 0.1 0.08 0.06 0.04 0.02 20 0.092 moles/liter If you have trouble viewing this image Click to open: 0.04 moles/liter 0.06 moles/liter 30 1.34 moles/liter 50 40 Degrees Centigrade 60 70
Using the Kf and Kb equations with electrolytes A certain liquid X has a normal boiling point of 110.90 °C and a boiling point elevation constant K=1.66 °C-kg mol -1 .A solution is prepared by dissolving some ammonium sulfate ((NH SO,) in 150.g of X. This solution boils at 112.2 °C. Calculate the mass of (NH), SO, that was dissolved. Round your answer to 2 significant digits. ? Explanation Check ©2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | étv A
2. A benzene (B)-toluene (T) solution is in equilibrium with its vapor at 80°C. If уB -0.670, calculate XB and the total vapor pressure of the solution. The vapor pressures at 80°C of benzene and toluene are 100.4 kPa and 38.7 kPa, respectively. (answer: XB-0.439, P= 65.8 kPa)** Calculate the equilibrium concentration (represented as a mole fraction) of carbon dioxide in fat given that