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- It is found that the boiling point of a binary solution of A andB with xA = 0.6589 is 88 °C. At this temperature the vapour pressuresof pure A and B are 127.6 kPa and 50.60 kPa, respectively. (i) Is thissolution ideal? (ii) What is the initial composition of the vapour abovethe solution?5B.11(a) The vapour pressure of pure liquid A at 300 K is 76.7kPa and that of pure liquid B is 52.0kPa. These two compounds form ideal liquid and gaseous mixtures. Consider the equilibrium composition of a mixture in which the mole fraction of A in the vapour is 0.350. Calculate the total pressure of the vapour and the composition of the liquid mixture.b) Suppose you had a solution of 6.84 g of sugar (sucrose, C12HO1) in 90.0 g of water. (i) Calculate the number of moles of sugar and water present. (H=1; C=12; 0=16) (ii) Calculate the mole fraction of the water in the solution. (iii) At 100°C, the saturated vapour pressure of water at its boiling point is 101325 Pa. Calculate the vapour pressure of the solution at that temperature. (Remember to give your answer to a suitable number of significant figures.) (iv) Would the solution of sugar in water boil at this temperature, assuming the external pressure remains at 101325 Pa? Explain your answer.
- (b) CMC of a surfactant in water at 25 °C is 0.5 g L-¹ and at 45 °C is 0.3 g L-1. The molar mass of the surfactant is 110 g mol-¹. (i) Calculate: The Gibbs energy of micellisation, AGO, of the surfactant at 25 °C and 45 °C, The fractions (%) of the surfactant molecules in free and in micellar states in 0.5 g L-¹ aqueous solution of the surfactant and temperature 45 °C. ● ● (ii) Calculate CMC for the surfactant in water at 55 °C.3. Assume that toluene and hexane form an ideal solution. At 365 K pure toluene has a vapour pressure of 0.582 bar and pure hexane has a vapour pressure of 1.99 bar. Consider a solution with mole fraction of hexane = 0.250. (a) Calculate the partial pressures of toluene and hexane, and the total pressure above the solution. (b) Some of the vapour is removed and allowed to condense in a second container. Calculate the partial pressures of hexane and toluene and the total pressure above this solution.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.
- 70.3(b) Calculate the Gibbs energy, entropy, and enthalpy of mixing when 25 g of hexane is mixed with 25 g of heptane at 298 K; treat the solution as ideal.Referring to Fig. 5.8, deduce the molar solubility of (i) NH4Cl, (ii) (NH4)2SO4 in water at 25 °C.3. (a) At 10 °C, the vapour pressures of pure chloroform (CHCI;) and pure dichloromethane (CH2CI2) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by mixing CHCI3 and CH;Cl2 is ideal. ii. Given the following data for this solution: p (CH2C12) = 1.33 gcm³; p (CHC13) = 1.48 gcm3; partial molar volume of CH2C12 = 56.5 cm³mol·'; partial molar volume of CHC13 = 77.3 cm³mol'. Calculate AmixV
- (a) Derive an expression for the ratio of solubilities of AgCI at two different temperatures; assume that the standard enthalpy of solution of AgCI is independent of temperature in the range of interest. (b) Do you expect the solubility of AgCI to increase or decrease as the temperature is raised?P5B.1 Potassium fluoride is very soluble in glacial acetic acid (ethanoic acid) and the solutions have a number of unusual properties. In an attempt to understand them, freezing-point depression data were obtained by taking a solution of known molality and then diluting it several times (J. Emsley, J. Chem. Soc. A, 2702 (1971)). The following data were obtained: b/(mol kg") 0.015 0.037 0.077 0.295 0.602 ΔΤΙΚ 0.115 0.295 0.470 1.381 2.67 Calculate the apparent molar mass of the solute and suggest an interpretation. Use AfH= 11.4kJ mol™ and T;* = 290 K for glacial acetic acid. lusThe rise in atmospheric carbon dioxide results in higher concentrations of dissolved carbon dioxide in natural waters. Use Henry's law and the data as given to calculate the solubility of CO2 in water at 25 °c when its partial pressure is (a) 3.8 kPa. (b) 50.0 kPa.