4) For such a phase diagram, a) Do you expect the newly formed bonds (A-B) are stronger than the initial bonds or not? Briefly explain the reason. Is this solution formation reaction endothermic or exothermic? b) Then, is the activity coefficient greater than 1 or not? How would you expect change in volume and change in Enthalpy due to formation of the solution? c) Describe the function (interatomic bond parameter). Explain/compare the bond strength (newly formed A-B vs initial A- A and B-B) depending on sign of the 2-function. T L+α L A Хв B

4) For such a phase diagram, a) Do you expect the newly formed bonds (A-B) are stronger than the initial bonds or not? Briefly explain the reason. Is this solution formation reaction endothermic or exothermic? b) Then, is the activity coefficient greater than 1 or not? How would you expect change in volume and change in Enthalpy due to formation of the solution? c) Describe the function (interatomic bond parameter). Explain/compare the bond strength (newly formed A-B vs initial A- A and B-B) depending on sign of the 2-function. T L+α L A Хв B

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...

See similar textbooks

Similar questions

The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal liquid-liquid solution. lf a solution is ideal, what is true about Hsoln, T for the solution formation, and the interactive forces within the pure solute and pure solvent as compared to the interactive forces within the solution? Give an example of an ideal solution. Answer the previous two questions for solutions that exhibit either negative or positive deviations from Raoults law.
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
A student determines the molar mass of acetone, , She found that the equilibrium temperature of a mixture of ice and water was 1.0C on her thermometer. When she added 11.1g of her sample to the mixture, the temperature, after through stirring, fell to -3.0C. She then poured off the solution through a screen into a beaker. The mass of the solution was 90.4g. a. what was the freezing point depression? b. what was the molarity of the acetone? c. how much aceton was in the decanted solution? d. how much water was in the decanted solution? e. how much acetone would there bein a solution containing 1kg of water and acetone at the same concentration as she has in herexperiment? f. what did she find to be the molar mass of aceton, assumingshe made the calculation properly?
For freezing point depression what is delta T mean? Is it the temperature of the solvent minus the temperature of the solution at freezing point?
The following is a T-x-y phase diagram for a binary system at constant pressure. a) Calculate the degrees of freedom (F) for the points represented by ‘c’ and ‘P’. Explain the significance of F in each case. b) An organic compound X is commonly used in commercial antifreeze agents, such as radiator fluids. Calculate the freezing point of a solution of 400 g of X in 500 g water. (Kf for water is -1.86 0C.m-1 and freezing point of pure water = 0oC). c) When a solution of 1.00 g of A in 100 cm3 of water was shaken with 10 cm3 of organic solvent (S), 0.80 g of A was transferred to the ether layer. How much of A would be extracted using 5 cm3 of S instead of 10 cm3?
This question is related to chemical potential in a solution and how it relates to physical properties. What is the relationship between the freezing point of a dilute solution vs. that of the pure liquid? Provide an explanation for this relationship based on thermodynamics. If the temperature is increased in a saturated solution of A in equilibrium with solid A, what will you observe? Give a thermodynamic explanation for this (based on chemical potential and mole fraction)
State ‘Raoult’s Law’ for a solution of volatile liquids.
State Raoult’s law in its general form with respect to solutions.
If 0.219 g of a solute is dissolved into 7.832 g of t-butanol (normal freezing point is 25C), and the solution freezes at 26.4C, what is the molar mass of the solute in g/mole? Given kf for t-butanol = 8.3C/m. Make sure to use correct units and sig figs.
Figure 5.2 shows the experimentally determined phase diagrams for the nearly ideal solution of hexane and heptane. (a) Indicate which phases are present in each region of the diagram. (b) For a solution containing 1 mol each of hexane and heptane molecules, estimate the vapour pressure at 70 °C when vaporization on reduction of the external pressure just begins. (c) What is the vapour pressure of the solution at 70 °C when just one drop of liquid remains? (d) Estimate from the figures the mole fraction of hexane in the liquid and vapour phases for the conditions of part b. (e) What are the mole fractions for the conditions of part c? (f) At 85 °C and 760 Torr, what are the amounts of substance in the liquid and vapour phases when zheptane = 0.40?