We discussed the temperature-composition phase diagram for a binary system given below. Mole fraction for B at key points are indicated.°CP = 1Vapourb,80P = 2P= 2LiquidP = 1LiquidP= 210-Qa,0.70XB0.20Mole fraction of B,0.85 0.9Starting from point a, of the binary mixture, what is the mole fraction of component B in the vapor when the mixture begins boiling?0.200.90Uncertain, since more information is needed.0.850.70ОООООTemperature, T

The number of phases that exists in equlibrium in a system depends on the variables temperature,…

We discussed the temperature-composition phase diagram for a binary system given below. Mole fraction for B at key points are indicated. °C P= 1 Vapour 80 P = 2 P= 2 Liquid P= 1 Liquid P = 2 10+ Qa, 0.20 Mole fraction of B, x 0.70 0.85 0.9 1 Starting from point a, of the binary mixture, what is the mole fraction of component B in the vapor when the mixture begins boiling? 0.20 0.90 Uncertain, since more information is needed. 0.85 0.70 Temperature, T

We discussed the temperature-composition phase diagram for a binary system given below. Mole fraction for B at key points are indicated. °C P= 1 Vapour 80 P = 2 P= 2 Liquid P= 1 Liquid P = 2 10+ Qa, 0.20 Mole fraction of B, x 0.70 0.85 0.9 1 Starting from point a, of the binary mixture, what is the mole fraction of component B in the vapor when the mixture begins boiling? 0.20 0.90 Uncertain, since more information is needed. 0.85 0.70 Temperature, T

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 114CP: Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution...

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Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25C. The vapor above the solution is collected and condensed. Using the following data, determine the composition in mole fraction of the condensed vapor. Substance Gfo C6H6(l) 124.50 kJ/mol C6H6(g) 129.66 kJ/mol CCI4(l) 65.21 kJ/mol CCI4,(g) 60.59 kJ/mol
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.
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. (i) Determine the overall mole fraction of aniline in the mixture. (ii) Use the lever rule to determine the relative amounts of the two phases.
The binary water-phenol diagram is given below, in molar fraction, under the total pressure Pt = 1 atm. 1) How many phases are there in the domain marked "I"? 2) From which temperature the mixture become miscible in all proportions? How do you call that temperature? 3) At a temperature T = 50 °C, in a controlled temperature container containing water. Phenol is then poured at the same temperature until the molar fraction of phenol in the mixture XC2H50H is equal to 0.05. Then, we continue to add the phenol gradually, at a constant temperature, to XC2H5OH of phenol in the mixture is XC2H5OH = 0.8. = 0.4. Then finally we stop adding phenol when the molar fraction a. How many phases are present at each one of the three mixture compositions in the container during the addition of the phenol? b. What is the composition of the phases when the fraction of phenol is XC2H5OH = 0.4? c. What is the proportions of the phases with respect to each other when XC2H5OH = 0.4? (Show your calculations)…
2. A polynomial fit to measurements of the molar volume of a binary mixture of A and B is: y = -6.6864x² + 60.067x + 22.764 where y = V (cm³ mol·1), x = xXA, and xẠ is the mole fraction of A. What are the partial molar volumes of A and B at xA = 0.5? 3. The partial molar volumes of propanone (acetone) and trichloromethane (chloroform) in a mixture in which the mole fraction of CHCI3 is 0.4693 are 74.166 cm³ mol-i and 80.235 cm³ mol-1, respectively. What is the volume of a solution of mass 1.000 kg?
Consider the following two temperature vs composition phase diagrams of two ideal binary mixtures – one consisting of liquids A and Band the other consisting of liquids Cand D- with TAi TB, Tc, and Tp being the boiling point temperatures of A, B, C, and D respectively at constant pressure. The curves in red are the vaporization curves while the curves in blue are the condensation curves. PA, PB, Pc, and Pp* are the vapour pressures of A, B, C, and D respectively. Tg - TA is greater than Tp* - Te. The number of vaporization-condensation cycles required to achieve greater than 99 % purity in the first solution is NAB and the number of vaporization- condensation cycles required to achieve greater than 99 % purity in the second solution is NcD Which of the following statements is true? Mole fraction, x Mole fraction, x. O A. NAB NCD and pa* > PB* B. NAB NCDand Pa* PB* D. NAB NCD and PA> PB* E. NAB NCDand pD* > Pc O O Temperature, T Temperature, T
7. Assume that the data in the table below stems from a liquid mixture that obeys Raoult's law. mole fraction p(MBenzene)/Torr p(Benzene)/Torr Total x(Methylbenzene pressure/Torr 0 0.30 0.45 0.61 0.84 1 0 7.19 (ii) 14.90 (iv) 25.02 80.00 (i) 43.57 (iii) 11.90 a) Estimate the missing values. b) Estimate the total pressure for each composition. c) Determine which component is more volatile
Two liquids, A and B, show partial miscibility below 52.4 °C. The critical concentration at the upper critical temperature is x = 0.459, where x is the mole fraction of A. At 40.0 °C the two solutions in equilibrium havex = 0.22 and x = 0.60, respectively, and at 42.5 °C the mole fractions are 0.24 and 0.48. Sketch the phase diagram. Describe the phase changes that occur when B is added to a fixed amount of A at (i) 48 °C, (ii) 52.4 °C.
Hexane and perfluorohexane show partial miscibility below 22.70 °C. The critical concentration at the upper critical temperature is x = 0.355, where x is the mole fraction of C6F14. At 22.0 °C the two solutions in equilibrium have x = 0.24 and x = 0.48, respectively, and at 21.5 °C the mole fractions are 0.22 and 0.51. Sketch the phase diagram. Describe the phase changes that occur when perfluorohexane is added to a fixed amount of hexane at (i) 23 °C, (ii) 22 °C.
(b) Surface sanitizers were prepared using ethyl alcohol/water and isopropyl alcohol/water solutions. An experiment was done to determine which composition would be most effective and as such two solutions were formulated: 70 % v/v ethyl alcohol and 70 % v/v isopropyl alcohol. Calculate the vapour pressure of these solutions and use your answer to reason which combination would stay on the surface longer. P° (Ethyl alcohol) = 12.4 kPa P° (Isopropyl alcohol) = 4.4 kPa P° (Water) = 2.4 kPa
kPa is the dissociation vapor pressure 608 of AB salt at 427°C and at 459°C it has increased to 1115 kPa. Find (a) Kp, (b) AG° at the two temperatures as well as AHO. Assume the ideal behaves of gases and the AH is independent on above temperature, also every latm. = 101.323 kPa. AB(s) == A(g) + B(g) %3%3D
When 2.0 g of aspirin was shaken up in a flask containing two immiscible liquids it was found that the mole fractions in the two liqu ids were 0.11 and 0.18. When a further 1.0 g of aspirin was added, it was found that the mole fraction in the first liquid increased to 0.15. What would you expect the mole fraction in the second liquid to become?