Step 1: Calculation of total pressure
Total pressure = partial pressure of chloroform + partial pressure of acetone
Total pressure = 20 + 220 mm Hg = 240 mm Hg.
Step 2: calculation of partial pressure using mole fraction
Partial pressure of chloroform = mole fraction of chloroform X total pressure
Partial pressure of chloroform = 0.12 / 0.92 X 240
= 31.30 mm Hg.
The given partial pressure of chloroform is 20 mm Hg, but calculated partial pressure of chloroform is 31.30 mm Hg.
Since, there is a difference in mole fraction , the combination of solution is a real solution and not ideal solution.
Ideal Solutions maintain, same pressure, both theoritithe and calculated.
A solution consists of chloroform and acetone. At 300 K, the partial vapor pressure for chloroform/is...
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At 300 K, the vapor pressure of pure liquid A and B is 200 mmHg and 450 mmHg, respectively. If the total pressure of the mixture A and B is 350 mmHg and the assumption that the solution is ideal, calculate: (a) Mole fraction of A and B in liquid phase and vapor phase, (b) The activity and activity coefficient of A and B in the solution, and (c) The mixing free energy, Agm, and the mixing entropy, Asm, of...
4. At 300 K, the vapor pressure of pure liquid A and B is 200 mmHg and 450 mmHg, respectively. If the total pressure of the mixture A and B is 350 mmHg and the assumption that the solution is ideal, calculate: (a) Mole fraction of A and B in liquid phase and vapor phase, (b) The activity and activity coefficient of A and B in the solution, and (c) The mixing free energy, Agm, and the mixing entropy, Asm,...
1. As the mole fraction of chloroform approaches 1, the vapor pressure of acetone could be calculated using A. Raoult's Law. B. Henry's Law. 2.If a chloroform-acetone mixture with an chloroform mole fraction of 0.62 is subjected to fractional distillation, what is the composition of the distillate? A. pure chloroform B. pure azeotrope C. pure acetone 3. Do chloroform and acetone form an ideal solution? A. no B. cannot be determined from the information given C. yes 4. If a...
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3. Do chloroform and acetone form an ideal solution? A. no B. cannot be determined from the information given C. yes 4. If a chloroform-acetone mixture with an acetone mole fraction of 0.6 is subjected to fractional distillation, what is the composition of the distillate? A. pure azeotrope B. pure acetone C. none of the choices shown D. pure chloroform 5. The acetone-chloroform intermolecular attractions are _________________ the acetone-acetone or chloroform-chloroform attractions. A. less than B. equal to C. greater...
Your lab partner combined chloroform (CHCl3) and acetone (C3H60) to create a solution where the mole fraction of chloroform, Xchloroform, is 0.219. The densities of chloroform and acetone are 1.48 g/mL and 0.791 g/mL, respectively. Calculate the molarity of the solution. Number Calculate the molality of the solution. Number Imi ITI