### Henry's Law and Vapor Pressure Measurements**Problem:**The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35 °C with the following results:| \( x_C \) | 0 | 0.20 | 0.40 | 0.60 | 0.80 | 1 ||------------|------|-------|-------|-------|-------|------|| \( P_C \) (torr) | 0 | 35.3 | 82.5 | 142 | 200 | 273 || \( P_A \) (torr) | 347 | 250 | 175 | 92.3 | 36.8 | 0 |The question asks for the Henry's law constant for chloroform in this system.**Options:**A) 365 torr B) 347 torr C) 177 torr D) 273 torr E) 485 torr **Solution:**Henry's law states that the vapor pressure of a solute (in this case, chloroform) is directly proportional to its mole fraction in the solution. Mathematically, it can be expressed as:\[ P_C = k_H \cdot x_C \]Where:- \( P_C \) is the vapor pressure of chloroform.- \( x_C \) is the mole fraction of chloroform.- \( k_H \) is the Henry's law constant.To find \( k_H \):We use any given pair of \( x_C \) and \( P_C \) values. For simplicity, let's use when \( x_C = 1 \):\[ P_C = k_H \cdot x_C \]\[ 273 \text{ torr} = k_H \cdot 1 \]\[ k_H = 273 \text{ torr} \]Therefore, the Henry's law constant for chloroform in this system is 273 torr.**Answer:**D) 273 torr

Given Data: xC00.20.40.60.81PC (torr)035.382.5142200273PA (torr)34725017592.336.80To…

The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35 °C with the following results: 0 0 347 A) 365 torr 0.20 35.3 250 0.40 82.5 175 XC Pc (torr) PA (torr) What is the Henry's law constant for chloroform in this system? 0.60 142 92.3 0.80 200 36.8 1 273 0

The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35 °C with the following results: 0 0 347 A) 365 torr 0.20 35.3 250 0.40 82.5 175 XC Pc (torr) PA (torr) What is the Henry's law constant for chloroform in this system? 0.60 142 92.3 0.80 200 36.8 1 273 0

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

Camphor (C10H16O) melts at 179.8 °C, and it has aparticularly large freezing-point-depression constant,Kf = 40.0 °C/m. When 0.186 g of an organic substance of unknownmolar mass is dissolved in 22.01 g of liquid camphor,the freezing point of the mixture is found to be 176.7 °C.What is the molar mass of the solute?
You are handed a 15.85% by mass aqueous KCl (m.m. = 74.5513 g mol–1) 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. Determine the following: Freezing Point of Solution in Degrees Celcius
Given that the solubility of any organic material in a given solvent is due to the intermolecular forces present between the solvent and solute, solvents like hexanes (the alkanes isomers of C6H14) are rarely used for extraction purposes. In the space provided here, suggest a reasonable explanation for this experimental observation.
A and B form an ideal binary solution at 30 °C. The vapor pressure of pure A at 30 °C is 42.2 mmHg, and the vapor pressure of pure B at 30 °C is 17.0 mmHg. a) If a solution is prepared with a liquid mole fraction of Xa = 0.6, calculate the partial pressure of each component in the solution. b) Determine the total vapor pressure above the solution.
A solution contains 6.23 g of urea, CO(NH2)2 (a non-volatile solute) in 0.400 kg of water. a) What is the mole fraction of water in this solution? b) If the vapour pressure of pure water at 25oC is 23.7 Torr, what is the vapour pressure of the solution, Psoln, assuming ideal behaviour?
Two volatile liquids A and B form an ideal solution. The vapor pressures for the pure liquids (at T = 50.0 °C) are pA° = 418. torr and pB° = 226. torr. For a solution at T = 50.0 °C, it is found that pA = pB. Based on this information, find XA, the mole fraction of A in the liquid phase for the solution.
There is a system in which solid colloids (density = 2.5 g/cm^3) with a particle diameter of 300 nm are dispersed in water. In this system, what is the main role of colloidal particles, sedimentation or diffusion?
The solvent for an organic reaction is prepared by mixing 70.0 mL of acetone (C3H6OC3H6O) with 56.0 mL of ethyl acetate (C4H8O2C4H8O2). This mixture is stored at 25.0 ∘C∘C. The vapor pressure and the densities for the two pure components at 25.0 ∘C∘C are given in the following table. What is the vapor pressure of the stored mixture? Compound Vapor pressure(mmHg) Density(g/mLg/mL) acetone 230.0 0.791 ethyl acetate 95.38 0.900
What masses of nitrogen and oxygen are dissolved in 192 g of water at 20.0 °C when the water is saturated with air, in which PN2 equals 593 torr and Poz equals 159 torr? At 1.00 atm pressure, the solubility of pure oxygen in water is 0.00430 g O2/100.0 g H20, and the solubility of pure nitrogen in water is 0.00190 g N2/100.0 g H20. i mg of nitrogen mg of oxygen eTextbook and Media Hint Assistance Used How is concentration related to partial pressure?
There are two solutions of eugenol (b.p. = 248 °C, v.p. = 4 torr at 100° C) and water (b.p = 100 °C and v.p. = 760 torr at 100 °C). The molar fraction of eugenol and water in solution A are 0.80 and 0.20 respectively. The molar fraction of eugenol and water in solution B are 0.20 and 0.80 respectively. Which statement is true regarding the boiling point of the two solutions? (Hint: eugenol and water are immiscible) A. Solution A will have a higher boiling point. B. Solution B will have a higher boiling point. C. Both solutions will boil at the same temperature. D. The relative boiling points cannot be determined with the given information. A. Solution A will have a higher boiling point. OB. Solution B will have a higher boiling point. C. Both solutions will boil at the same temperature. OD. The relative boiling points cannot be determined with the given information.
A CHM 126 student performed the "Determination of Molar Mass by Freezing Point Depression" experiment. He started the experiment by measuring the mass and freezing point of the pure solvent with minimal error. Instead of quickly finishing the experiment, he took a lunch break. After returning from lunch, he noted that the solvent had absorbed some impurities from the atmosphere. He went ahead and performed the rest of the experiment anyway. Assuming a negligible (very minor) change in the mass of the solvent after absorbing impurities, which of the following choices contains only correct statements: because of the experimental error, the measured ATwill increase, the measured molality will increase, and the measured molar mass will contain no additional error because of the experimental error, the measured ATwill decrease, the measured molality will decrease, and the measured molar mass will decrease because of the experimental error, the measured ATwill decrease, the measured molality…
9.294 g of a non-volatile solute is dissolved in 305.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 60°C the vapour pressure of the solution is 148.07 torr. The vapour pressure of pure water at 60°C is 149.40 torr. Calculate the molar mass of the solute (g/mol). 61.1 g/mol You are correct. Your receipt no. is 162-1722 ? Previous Tries Now suppose, instead, that 9.294 g of a volatile solute is dissolved in 305.0 g of water. This solute also does not react with water nor dissociate in solution. The pure solute displays, at 60°C, a vapour pressure of 14.94 torr. Again, assume an ideal solution. If, at 60°C the vapour pressure of this solution is also 148.07 torr. Calculate the molar mass of this volatile solute. Note that the calculation is greatly simplified if you recognize that: \solute = 1- Xwater.