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…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 13ALQ

See similar textbooks

Similar questions

The pure vapour pressure of benzene (C6H6) is 745 torr; the pure vapour pressure to toluene(C7H8) is 290 torr. What is the mole fraction of benzene in a benzene/toluene mixture whose total vapour pressure is 500 torr? Give answer to 3dp.
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.
A polynomial fit to measurements of the total volume of a binary mixture of A and B isv = 778.55 − 22.5749x + 0.568 92x2 + 0.010 23x3 + 0.002 34x4where v = V/cm3, x = nB/mol, and nB is the amount of B present. Derive an expression for the partial molar volume of B.
The partial molar volumes of propanone and trichloromethane in a mixture in which the mole fraction of CHCI3 is 0.4693 are 74.166 cm3 mol-1, and 80.235 cm3 mol-1, respectively. What is the volume of a solution of total mass 1.000 kg?
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.
The partial molar volumes of propanone (acetone) and trichloromethane (chloroform) in a mixture in which the mole fraction of CHCl3 is 0.4693 are 74.166 cm3 mol−1 and 80.235 cm3 mol−1, respectively. What is the volume of a solution of mass 1.000 kg?
An open vessel containing (a) water, (b) benzene, (c) mercury stands in a laboratory measuring 5.0 m x 4.3 m x 2.2 m at 25 °c. The vapour pressures of each substance are (a) 2.3 kPa, (b) 10 kPa, (c) 0.30 Pa, respectively. What massof each substance will be found in the air if there is no ventilation?
In the following balanced reaction: 2Al(s) + 6HCl(aq) → 2AlCl3(s) + 3H2(g) 2.32 g of Al react with excess HCl to produce hydrogen gas which is passed through water and collected at 25oC and a barometric pressure of 7.40 x 102 Torr. The vapour pressure of water at 25oC is 23.770 Torr. Calculate the partial pressure of hydrogen gas.
5C. 2(b) Sketch the phase diagram of the system of NH/NH, given that the two substances do not form a compound; NH, freezes at -78 °C; N₂H, freezes at 2 °C; a eutectic is formed when the mole fraction of N H is 0.07; and the eutectic melts at -80 °C.
In a closed, insulated system, the vapour pressure of water at 15.37 °C is 2687 Pa. What percentage of the standard atmospheric pressure (1 atm) is this?
Phenol and water form non-ideal liquid mixtures. When 7.32 g of phenol and 7.95 g of water are mixed together at 60 °C they form two immiscible liquid phases with mole fractions of phenol of 0. 0 42 and 0 .161 . (a) Calculate the overall mole fraction of phenol in the mixture. (b) Use the lever rule to determine the relative amounts of the two phases .
A container is divided into two equal compartments. One contains 3.0 mol H2(g) at 25°C; the other contains 1.0 mol N2(g) at 25°C. Calculate the Gibbs energy of mixing when the partition is removed. Assume perfect behavior.

SEE MORE QUESTIONS

Recommended textbooks for you

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS