2. A polynomial fit to measurements of the molar volume of a binary mixture of A and B is:y = -6.6864x² + 60.067x + 22.764where y = V (cm³ mol·1), x = xXA, and xẠ is the mole fraction of A. What are the partial molarvolumes of A and B at xA = 0.5?3. The partial molar volumes of propanone (acetone) and trichloromethane (chloroform) in amixture in which the mole fraction of CHCI3 is 0.4693 are 74.166 cm³ mol-i and 80.235 cm³mol-1, respectively. What is the volume of a solution of mass 1.000 kg?

Answered: Image /qna-images/answer/dd247d00-ff20-4223-b139-edd888340878.jpg

Answered: A polynomial it to measurements of the…

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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What is the partial pressure of methane needed to dissolve 21mg of the gas in 100g of benzene at 25 degrees Celsius, knowing that Henry's law constant for methane is worth 5.69x104kPa? (M metano - 16,04g mol-1 , M benzeno - 78,11g mol-1).
At 20 oC, the mass density of a 20 percent by mass ethanol-water solution is 968.7 kg m-3. Give that the partial molar volume of ethanol in the solution is 52.2 cm3 mole-1, calculate the partial molar volume of the water.
Pure liquid A has vapor pressure 200. bar and pure liquid B has vapor pressure 100. bar. In an AB mixture with mole fraction X = 0.500, compute the mole fraction of A in the vapor.
Show that (demonstrate) for an ideal binary solution, where 1 is the solvent and 2 is the solute, the increase in the boiling point of the solvent (ΔT) due to the presence of the solute is given by the relation: ∆T=Kebb2=(T'eb-Teb) where Keb=[R(Teb)2M1]/1000∆vapH1] Keb=ebulloscopic constant Please show all of the steps and calculations used to demonstrate the question. As well as a brief explanation of the principle used.
Suppose the vapor pressures of two components of a binary solution are given by:P1 = x1P1∗e^((x^2_2)/2) and P2 = x2P2∗e^((x^1_2)/2)a) Given that P1* = 75.0 torr and P2* = 160 torr, calculate the total vapor pressure and thecomposition of the vapor phase at x1 = 0.40.b) Plot y1 versus x1 for this system. Why does the curve lie below the straight line connecting theorigin with the point x1 = 1, y1 = 1? Describe a system for which the curve would lie above thediagonal. Please only solve part b
Partial molar volumes of acetone and chloroform in their equimolar (0.5/0.5 molar fractions) mixture are 74.2 cm3mol-1 and 80.2 cm3mol-1. What is density of this solution?
The vapor pressures of CCl4 (A) and C₂HCl3 (B) between T = 350 and 360 K, can be determined empirically by the formulas 2790.78 (T - 46.75) 2345.4 (T- 80.45) where T is given in K, and the vapor pressures will be in units of bars. In this problem, assume that these two substances form an ideal solution in this temperature range, in all proportions. In PA* 1 bar In PB* 1 bar 9.2199 = 8.3922 2 (a) Find the mole fraction of CCl4 (component A) in both the liquid and vapor phases at T = 354 K, and an ambient pressure of 0.96 bar. (b) Suppose this mixture is heated slightly to a temperature of T = 358 K but its solution has the same composition (i.e. the same mole fractions of CCl4 and C₂HCl3). What is the total vapor pressure of the solution now (in bars), and what is the mole fraction of CCl4 in the vapor?
3. The second Virial coefficient of an equimolar binary vapor mixture of methane and n-hexane is -517 cm'/mol at 50°C. What is B at the same temperature for a mixture containing 25 mol% methane and 75 mol% n-hexane. At 50°C B =-33 cm'/mol for methane, B =-1512cm'/mol for n-hexane.
A solvent (molar mass = 98.2 g mol-¹) has a vapour pressure of 4930 Pa at 20 °C; at 50 °C this increases to 1.94 x 104 Pa. A mass of 12.8 g of an unknown solute is dissolved in 100.0 g of the solvent. Assume the solute has negligible vapour pressure. Estimate the normal boiling point of the solution.
The graph given below plots the (approximate) partial molar volumes of ethanol (black line) and water (red line) in units of ml/mole at 25°C in a mixture as a function of the mole fraction of ethanol. Use the information in this graph (note the different y axes for water and ethanol) and the densities at 25°C to calculate the resulting total volume of the g following two mixtures.(pethanol = 0.789 ml & PH20 = 0.998 ) ml a. 150 ml ethanol + 100 ml H2O b. 200 ml ethanol + 40 ml H2O H20 VELOH Vet o*HA -V ELOH V H2O T 0.8 1.0 0.2 0.4 0.6 0.0 XELOH 53 54 55 57 15 18
Looking at the following image of a curve of partial pressures vs mole fractions of the two components A and B of an ideal mixture of liquids that obeys Raoult's Law where pa and pe are the partial pressures of the two liquids A and B respectively and xa and xg are the mole fractions of A and B respectively, which of the following statements is true? PA Pa R S A. The intercepts R and S are representative of the equilibrium vapour pressures of the components A and B respectively B. The intercepts R and S are representative of the equilibrium vapour pressures of the components B and A respectively C. The slopes of the two curves, red and blue, are representative of the equilibrium vapour pressures of the components A and B respectively D. Both (B) and (C) E. The slopes of the two curves, red and blue, are representative of the mole fractions of the components A and B respectively

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