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- A mixture of ethane,propane and n-butane exists at -10°C at a total pressure of 3000 mmHg. Determine the mole fraction of ethane in a vapor phase if the propane and n-butane compositions are equal in the liquid phase. Vapor pressures at -10°C are (in mmHg) : ethane=14000,propane=2700 and n-butane=500A. 0.4435B. 0.3992C. 0.739D. 0.5269In calculating ΔHmix for regular solutions, please derive 1) the mole fraction for the minimum of ΔHmix 2) the equation for the minimum of ΔHmixThe freezing point of a substance is the temperature at which the solid and liquid forms can coexist indefinitely, at equilibrium. Under these conditions molecules pass between the 2 phases at equal rates because their escaping tendencies from the two phases are identical. Like the boiling point elevation, the freezing point of a solution is directly proportional to the molal concentration of the solution, that is, AT= Kr m Where, ATr refers to the freezing point lowering, Kf, the freezing point depression constant, and m, the molality of the solution. Some of the Kf values are shown in Table 1. For water, Kf is 1.86 °C/m, therefore, any 1 m aqueous solution of nonvolatile solute or a 0.5 m aqueous solution of NaCl will freeze at 1.86 °C lower than pure water. EXERCISE: Problem Solving: Show your solution! 1. A solution containing a nonelectrolyte dissolved in water has a boiling point of 0.305 °C. Calculate the freezing point of the same solution.
- At 25°C, some water is added to a sample of gaseousmethane (CH4) at 1.00 atm pressure in a closed vessel, andthe vessel is shaken until as much methane as possible dissolves. Then 1.00 kg of the solution is removed and boiledto expel the methane, yielding a volume of 3.01 L ofCH4(g) at 0°C and 1.00 atm. Determine the Henry’s lawconstant for methane in water.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.4. Why is the free energy of an ideal liquid mixture less than the free energy of the pure liquid? How does this lead to freezing point depression, with the assumption that the coexisting solid is pure?
- Calculate the solubility of nitrogen in water at an atmospheric pressure of 0.500 atm (a typical value at high altitude). Atmospheric Gas Mole Fraction kH mol/(L*atm) N2 7.81 x 10-1 6.70 x 10-4 O2 2.10 x 10-1 1.30 x 10-3 Ar 9.34 x 10-3 1.40 x 10-3 CO2 3.33 x 10-4 3.50 x 10-2 CH4 2.00 x 10-6 1.40 x 10-3 H2 5.00 x 10-7 7.80 x 10-4 MA chemistry student is given 550. mL of a clear aqueous solution at 37.° C. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 19.° C. At that point, the student sees that a precipitate has formed. He transfers the liquid to a clean new beaker and throws away the precipitate. The student then evaporates the water from the liquid in the new beaker under vacuum. It weighs 0.055 kg. Using only the information above, can you calculate the solubility of Xin water at 19.° C ? If you said yes, calculate it. Be sure your answer has a unit symbol and 2 significant digits. O yes Ono 0 ロ･ロ X H ola 0 S 10 olCarbon 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
- Convert the units of Henrys law constant for CO2, in table 7.2, to units of, mmHg, atm, and bar. In which cases does the numerical value of the constant change?Explain how the unit molarity automatically includes the concept of partial molar volumes.7.5. For this chemical equilibrium in an enclosed system, how many degrees of freedom are there?
