5. Consider the ideal solution formed by mixing 1.0 mol of n-Hexane with 1.0 mol of n-Heptane at 298 K and calculate the Gibbs energy of mixing.5.1Draw a diagram to illustrate that,5.1.1 The chemical potential of the liquid solvent in a solution is lower than that of the pure5.1.25.1.3liquid.The temperature at which the chemical potential of the solvent is equal to that of thesolid solvent (freezing point) is lowered as a result.The temperature at which the chemical potential of the solvent is equal to that of thevapour (boiling point) is raised.

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Answered: 5. Consider the ideal solution formed…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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12.35. Consider a binary mixture for which the excess Gibbs energy is given by GE/RT = 2.6x1x2. For each of the following overall compositions, determine whether one or two liquid phases will be present. If two liquid phases will be present, find their composi- tions and the amount of each phase present (phase fractions). (a) z1 = 0.2 (b) z1 = 0.3 (c) z1 = 0.5 (d) z1 = 0.7 (e) z1 = 0.8
6. Using phase diagram for the mixtures of benzene and ethylbenzene shown below, estimate: Benzene / Ethybenzene at 1.00 atm By NRTL A) Boiling point of pure ethylbenzene 140- 135- 130- B) Boiling point (Tpp) of solution with molar fraction of benzene 0.3. 125 120- 115 110- C) Composition of vapor phase (molar fractions of both liquids) above the solution with molar fraction of benzene 0.3 at Töp. 105- 100 90 85 80- 75- a1 02 03 04 05 06 0.7 0.8 09 Benzene Mole Fracfioni
Consider a binary solutian for which the vapor pressure (in torr) of one of the components (say component 1) is given empirically by the equation below. P, = 79. 1xje.67o.15x Calculate the activity and the activity coefficient of component 1 when x1- 0.26 based on a solvent standard state. (2 sig fig) Calculate the activity and the activity coefficient of component 1 based on a solute standard state. (2 sig fig) Y1 Periodic Table Constants & Factors
Please answer b and c
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3.3 Consider the variation of molar Gibbs energy with pressure. 3.3.1 Write the mathematical expression for the slope of graph of molar Gibbs energy against 3.3.2 pressure at constant temperature. Draw in same diagram graphs showing variation with pressure of molar Gibbs energies of a substance in gaseous, liquid and solid forms at constant temperature. 3.3.3 Indicate in your graphs melting and boiling points. 3.3.4 Indicate for the respective phases the regions of relative stability.
The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 (b) A reversible isomerization reaction converts reactant A to product X. Calculate the Gibbs energy change at non-standard conditions (310 K) if the concentration of A is 2 x 10-4M and that of X is 3 x 10-6 M. Comment on whether the reaction is spontaneous at these conditions. The equilibrium constant Keq = 0.05. Assume standard temperature is 298K.
4 GIBBS ENERGY The following reaction happens in red blood cells CO2(g) + H2O (1) HCO3(aq) Using the following thermodynamic data (at 298.0 K) AH (kJ mol) 393.51 -285.83 CO2(g) H₂O (1) - CO (04) -699.65 Sm (IK 'mol) 213.7 69.9 187.4 (a) Calculate the standard entropy and the standard Gibbs energy of reaction at 298.0 K. Is the reaction exergonic or endergonic? (b) Using the Gibbs-Helmholtz equation, determine the standard Gibbs energy of the reaction at 310.0 K (37.0°C, body temperature). Notes Assume that the enthalpy of reaction does not change from 25.0°C to 37.0°C.
Part C A solution is formed when the solute unilormly disperses throughout (or dissolves in) the solvent The process can be described though three stops A hypothetical solution forms between a solid and a liquid The vakues of the thermodynamic Involved in the process are shown in the following table 1 separation of solvent-solvant particles, 2. breaking of solute-solute particles and 3. formation of solute-solvent interactions Action Enthalpy 145 kJ/mol 21.8 kJ/mol séparation of solute separation of solvent formation of solute-solvent interactions -85.7 kJ/mol solute The overall energy change for the solution process, AHa is the sum of the enthalpies of the threoe stepo. Whether AHs endothermic or exothermic depends on the relative magnitudes of AH, AH, and AH, where the subscript Indicates the step in the process corresponding to the enthalpy value Calculate the enthalpy of solution in kilojoules per mole of solute Enter your answer numerically in kilojoules per mole of solute. > View…
which of the following is the correct answer in the image provided and explain your reason for the choice.
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?

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