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Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :
  • a)
    xA = 0.37; xB = 0.63
  • b)
    xA = 0.28; xB = 0.72
  • c)
    xA = 0.76; xB = 0.24
  • d)
    xA = 0.4; xB = 0.6
Correct answer is option 'B'. Can you explain this answer?
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Liquids A and B form an ideal solution in the entire composition range...



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Liquids A and B form an ideal solution in the entire composition range...
And 4 atm, respectively. What is the vapor pressure of a mixture of A and B that contains equal amounts of each liquid?
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Ideal Solution at Fixed TemperatureConsider two liquids B and C that form an ideal solution. We hold the temperature fixed at some value T thatis above the freezing points of B and C. We shall plot the systems pressure P against XB, the overall molefraction of B in the system :Where are the number of moles of B in the liquid and vapor phases, respectively. For a closed system XB is fixed, although may vary.Let the system be enclosed in a cylinder fitted with a piston and immersed in a constant-temperature bath. To see what the P-versus–XB phase diagram looks like, let us initially set the external pressure on the piston high enough for the system to be entirely liquid (point A in figur e) As the pressure is lowered below that at A, the system eventually reaches a pressure where the liquid just begins to vaporizes (point D). At point D, the liquid has composition at D is equal to the overall mole fraction XB since only an infinitesimal amount of liquid has vapourized. What is the composition of the first vapour that comes off ? Raoults law, relates the vapour-phase mole fractions to the liquid composition as follows :............(1)Where PB0 and PC0 are the vapour pressures of pure B and pure C at T, where the systems pressure P equals the sum PB + PC of the partial pressures, where, and the vapour is assumed ideal. ............(2)Let B be the more volatile component, meaning that . Above equation then shows that The vapour above an ideal solution is richer than the liquid in the more volatile component. Equations (1) and (2) apply at any pressure where liquid –vapour equilibrium exists, not just at point D.Now let us isothermally lower the pressure below point D, causing more liquid to vaporize. Eventually, wereach point F in figure , where the last drop of liquid vaporizes. Below F, we have only vapour. For any pointon the line between D and F liquid and vapour phases coexist in equilibrium.Q. Two liquids A and B have the same molecular weight and form an ideal solution. The solution has a vapour pressure of 700 Torrs at 80ºC. It is distilled till 2/3rd of the solution (2/3rd moles out of total moles) is collected as condensate. The composition of the condensate is xA = 0.75 and that of the residue is xA= 0.30. If the vapour pressure of the residue at 80ºC is 600 Torrs, find the original composition of the liquid ?

Ideal Solution at Fixed TemperatureConsider two liquids B and C that form an ideal solution. We hold the temperature fixed at some value T thatis above the freezing points of B and C. We shall plot the systems pressure P against XB, the overall molefraction of B in the system :Where are the number of moles of B in the liquid and vapor phases, respectively. For a closed system XB is fixed, although may vary.Let the system be enclosed in a cylinder fitted with a piston and immersed in a constant-temperature bath. To see what the P-versus–XB phase diagram looks like, let us initially set the external pressure on the piston high enough for the system to be entirely liquid (point A in figur e) As the pressure is lowered below that at A, the system eventually reaches a pressure where the liquid just begins to vaporizes (point D). At point D, the liquid has composition at D is equal to the overall mole fraction XB since only an infinitesimal amount of liquid has vapourized. What is the composition of the first vapour that comes off ? Raoults law, relates the vapour-phase mole fractions to the liquid composition as follows :............(1)Where PB0 and PC0 are the vapour pressures of pure B and pure C at T, where the systems pressure P equals the sum PB + PC of the partial pressures, where, and the vapour is assumed ideal. ............(2)Let B be the more volatile component, meaning that . Above equation then shows that The vapour above an ideal solution is richer than the liquid in the more volatile component. Equations (1) and (2) apply at any pressure where liquid –vapour equilibrium exists, not just at point D.Now let us isothermally lower the pressure below point D, causing more liquid to vaporize. Eventually, wereach point F in figure , where the last drop of liquid vaporizes. Below F, we have only vapour. For any pointon the line between D and F liquid and vapour phases coexist in equilibrium.Q.If the above process is repeated for all other compositions of mixture of C and B. If all the points where vapours start converting into liquid are connected and all the points where vapours get completely converted into liquid are connected then obtained graph will look like

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Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer?
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Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer?.
Solutions for Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE. Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.
Here you can find the meaning of Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer?, a detailed solution for Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice Liquids A and B form an ideal solution in the entire composition range. At 350 K, the vapor pressures of pure A and pure B are 7 × 103 Pa and 12 × 103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is :a)xA = 0.37; xB = 0.63b)xA = 0.28; xB = 0.72c)xA = 0.76; xB = 0.24d)xA = 0.4; xB = 0.6Correct answer is option 'B'. Can you explain this answer? tests, examples and also practice JEE tests.
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