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. 5.1 Draw a diagram to illustrate that, 5.1.1 The chemical potential of the liquid solvent in a solution is lower than that of the pure 5.1.2 5.1.3 liquid. The temperature at which the chemical potential of the solvent is equal to that of the solid solvent (freezing point) is lowered as a result. The temperature at which the chemical potential of the solvent is equal to that of the vapour (boiling point) is raised.

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

174 Solubility and 18.3 Gibbs Free E... 5.3 Enthalpies of... 18.5 Gibbs Free E... Reading Schedule 19.8 E OKINETICS AND EQUILIBRIUM Calculating the solubility of an ionic compound when a commo... sp Calculate the solubility at 25 °C of BaCrO, in pure water and in a 0.0100M BaCl, solution. You'll find K, data in the ALEKS Data tab. Round both of your answers to 2 significant digits. esc solubility in pure water: solubility in 0.0100 M BaCl₂ solution: Explanation 30 Methods for Measuring the pH of an Aqueous Slide 28 of 104 A Recheck Z 2 W CLICK TO YOU holes Notes Comments 9:1 + S 3 D 4 C > R F 00 0° 0.9 0x0 96 5 X 63% 53 T G 6 B 3 Y ola I'm H 7 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessits Department of Psychology Queens College - CUNY U N 8 J Is M 9 K O 1 H 0 w P [O contion D

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?

2. A benzene (B)-toluene (T) solution is in equilibrium with its vapor at 80°C. If уB -0.670, calculate XB and the total vapor pressure of the solution. The vapor pressures at 80°C of benzene and toluene are 100.4 kPa and 38.7 kPa, respectively. (answer: XB-0.439, P= 65.8 kPa)** Calculate the equilibrium concentration (represented as a mole fraction) of carbon dioxide in fat given that

2 CHEMICAL POTENTIAL [6] Calculate the difference in slope of the chemical potential against temperature on either side of (a) The freezing point of water (b) The boiling point of water Data: Afus H=6.01 x 103 J mol-1 AvapH =40.6 x 103 J mol-1 Which state function does the slope represent? Why is the slope steeper for evaporation?

#5. Thank you.