Steam pressures for pure CCl4 and SiCl4 are given as 0.4226 bar and 0.7999 bar respectively, while the temperature is 50°C. For a mixture prepared with these two liquids and boiling at 50°C under a pressure of 0.5333 bar, find the composition of the phases as a mole fraction and a mass fraction. [M(CCl4):153,82 g/mol, M(SiCl4):169,9 g/mol]

Steam pressures for pure CCl4 and SiCl4 are given as 0.4226 bar and 0.7999 bar respectively, while the temperature is 50°C. For a mixture prepared with these two liquids and boiling at 50°C under a pressure of 0.5333 bar, find the composition of the phases as a mole fraction and a mass fraction. [M(CCl4):153,82 g/mol, M(SiCl4):169,9 g/mol]

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.3E

See similar textbooks

Similar questions

A mixture of phenol and water, under certain conditions of temperature and composition, forms two separate liquid phases, one rich in phenol and the other rich in water. At 30⁰ the compositions of the upper and lower layers are 70% and 9% by mass phenol, respectively. If 40kg of phenol and 60kg of water are mixed and the layers are allowed to separate at 30⁰C, what will be the weight of the two layers?
A liquid-vapour mixture whose composition is 60 mole % of benzene is contained within a vessel at 60C. What fraction of moles are both methanol and in the liquid phase?
A mixture consisting of 1-mol-% ethane, 5-mol-% propane, 44-mol-% n-butane, and 50-mol-% isobutane is brought to a condition of 294.15 K (21°C) at pressure P. If the molar fraction of the system that is vapor is 0.2, what is pressure P (in bar), and what are the compositions of the vapor and liquid phases?
Name two characteristic physical properties that distinguish condensed from gas phases, and one which distinguishes solid from liquid phases. Discuss the differences for each property. Name one colligative property and by an equation (label all variables) and 1-2 sentences the physical meaning. Consider a balloon. What thermodynamic system does it represent? How does this system interact with the environment? Calculate the heat capacity at constant pressure of methane for all its contribution and the total value according to the equipartition theorem. What is a more realistic value at room temperature? Why?
Calculate the following: (a) The bubble-point temperature of an equimolar mixture of liquid n-hexane and n-heptane at 1.0 atm and the composition (mole fractions) of the vapor in equilibrium with this mixture. (b) The dew-point temperature of a gas mixture with a molar composition of 30% n-hexane, 30% n-heptane, and 40% air at 1 atm and the composition (mole fractions) of the liquid in equilibrium with this mixture.
Q1a-> A sample of hydrogen (H₂) gas was collected over water at 60°C. If the total volume of gas collected was 53.9 mL and the atmospheric pressure was 1.14 bar, what mass (in g) of hydrogen gas was collected above the water? The vapour pressure of water at 60°C is 150 torr. Q1b=> What is the molar mass (in g mol-¹) of a gas which has a density of 1.91 g/L at a pressure of 0.91 bar and temperature 15.3°C? Your answer may not correspond to an actual gas. Do not try to identify the gas.
L-Serine is an amino acid important for its roles in synthesizing other amino acids and for its use in intravenous feeding solutions. It is often synthesized commercially by fermentation, and recovered by subjecting the fermentation broth to several processing steps and then crystallizing the serine from an aqueous solution. The solubilities of L-serine (L-Ser) in water have been measured at several temperatures, producing the following data:5T(K) 283.4 285.9 289.3 299.1 316.0 317.8 322.9 327.1x(mole fraction L-Ser) 0.0400 0.0426 0.0523 0.0702 0.1091 0.1144 0.1181 0.1248One of the ways such data can be represented is with the van’t Hoff equation: ln x =( a=T b).Graph the data so that the resulting plot is linear. Estimate a and b and give their units.
Iron(II) chloride (melting point 677 °C) and potassium chloride (melting point 776 °C) form the compounds KFeCl3 and K2FeCl4 at elevated temperatures. KFeCl3 melts congruently at 399 °C and K2FeCl4 melts incongruently at 380 °C. Eutectics are formed with compositions x = 0.38 (melting point 351 °C) and x = 0.54 (melting point 393 °C), where x is the mole fraction of FeCl2. The KCl solubility curve intersects the A curve at x = 0.34. Sketch the phase diagram. State the phases that are in equilibrium when a mixture of composition x = 0.36 is cooled from 400 °C to 300 °C.
Butane liquid and vapor coexist at 370.0 K and 14.35 bar. The densities of the liquid and vapor phases are 8.128 mol/ L and 0.6313 mol/L , respectively. Use the van Der Waals equation, the Redlich-Kwong equation and the Peng-Robinson equation to calculate these densities. Use α = 16.44 bar L2 mol-2 and β = 0.07245 L mol-1 for the Peng-Robinson equation. Please show each step and calculations explicitly, particularly how to arrive to the numerical result for the densities
Crude oil containing 5.0 mole per cent of gasoline is stripped by running the crude down a columnup which live steam is passed so that 15 kmol of steam are used/100 kmol of oil stripped. Determinethe number of theoretical plates required to reduce the gasoline content to 0.05 mole per cent, assumingthat the crude oil is non-volatile. The vapor–liquid relation of the gasoline in the oil is given by ye = 44x,where ye is the mole fraction in the vapor and x the mole fraction in the liquid. The temperature ismaintained constant by internal heating so that steam does not condense in the tower.
Aniline, C6H5NH2, and hexane, C6H14 , form partially miscible liquid - liquid mixtures at temperatures below 69. 1 °C. When 42.8 g of aniline and 75 .2 g of hexane are mixed together at a temperature of 67.5 °C, two separate liquid phases are formed, with mole fractions of aniline of 0.308 and 0.618.(a) Determine the overall mole fraction of aniline in the mixture. (b) Use the lever rule to determine the relative amounts of the two phases.
What is w when 1.83 kg of H20(1), initially at 25.0 °C, is converted into water vapour at 185 °C against a constant external pressure of 1.00 atm? Assume that the vapour behaves ideally and that the density of liquid water is 1.00 g/ml (Remember to include a+or-sign as appropriate.) Enter your answer in acceptable SI units, accurate to 3. significant figures. Use an acceptable Sl symbol for units.