The partial molar volumes of water and ethanol in a solution with XH20 = 0.45 at 25°C are 17.0 and 57.5 cm3/mol, respectively. Calculate the total volume upon mixing %3D sufficient ethanol with 3.75 mol of water to give this concentration. O 226 cm3 O 315 cm3 327 cm3 335 cm3
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- You are handed a 15.85% by mass aqueous KCl (m.m. = 74.5513 g mol–1) solution (at 25 °C). Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Vapor pressure of the solution in atmThe distribution coefficient of hydrogen sulfide between benzene and water at 25 degrees Celsius is 5.9880. What is the minimum volume of benzene at 25 degrees Celsius necessary to extract in a single step 80% of the hydrogen sulfide from 1 liter of 0.15 molar aqueous solution of hydrogen sulfide?a.) 0.1336b.) 23.9520c.) 0.6680d.) 1.5030E.) none of the aboveAssume you dissolve 30.0 g of cobalt sulfate heptahydrate (CoSO4.7H2O) in 500 ml of a 1.0 MH2SO4 solution. Calculate the following for CoSO4.7H2O in this solution:(The Specific Gravity of 1.0 M H2SO4 @ 20°C is 1.0814 g/ml.) Molality, Mole fraction and Weight percentage
- Suppose that a solution made from an unknown solute dissolved in solvent X. Its molality is 0.0125 and it boils 0.047oC higher than solvent X's boiling point. With the use of valid approximations, calculate the osmotic pressure of the said solution at 60oC? The following are useful thermodynamic data for solvent X to solve the problem: ΔSvap=87.92 J*K-1mol-1 Tb=61.15oC density at 60oC=1.394 g/cm3Given the property on the left as the criterion, which of the following order of comparison is TRUE? Select one: a. Increasing electrical conductivity at 25 °C: Si < SiO2 < SiCl4 b. Increasing standard boiling point: 0.10 molal solution of sucrose in CH3CH2OH < pure CH3CH2OH < 0.10 molal aqueous solution of sucrose c. Increasing standard melting point: I2 < Br2 < Cl2 d. Increasing melting point: Na < NaCl < Na2OA solution is prepared by dissolving 22.4 g of MgCl2 in 0.200 L of water. Taking the density of pure water to be 1.00 g cm-3 and the density of the resulting solution to be 1.089 g cm-3, calculate the mole fraction, molarity, and molality of MgCl2 in this solution.
- 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.Mass of empty dish: 38.386 grams Volume of 0.0400 M stock solution: 5.00 mL Mass of Dish and 0.0400 M stock solution: 44.751 grams Mass of Dish and CuSO4 (after evaporation): 38.468 grams 1. Calculate the density of the solution a)Calculate the percent by mass, CuSO4, in stock solution (100 x g CuSO4/g solution) b)Calculate the molality of the stock solution (mole CuSO4 / kg solvent) c) Calculate the molarity of the stock solution (moles CuSO4 / L solution)279.28 mL of 1.22 M organic salt was mixed with 168.14 mL of Ethanol (d= 0.789 g/mL, MW 46.07g/mole). Pure ethanol has a vapor pressure of 0.059 atm what will be the vapor pressure of the solution?
- Hexane and perfluorohexane show partial miscibility below 22.70 °C. The critical concentration at the upper critical temperature is x = 0.355, where x is the mole fraction of C6F14. At 22.0 °C the two solutions in equilibrium have x = 0.24 and x = 0.48, respectively, and at 21.5 °C the mole fractions are 0.22 and 0.51. Sketch the phase diagram. Describe the phase changes that occur when perfluorohexane is added to a fixed amount of hexane at (i) 23 °C, (ii) 22 °C.The partial molar volumes of water and ethanol in a solution with xH2O=0.45 at 25 ∘C are 17.0 and 57.0 cm3⋅mol−1, respectively. Calculate the volume change upon mixing sufficient ethanol with 4.30 mol of water to give this concentration. The densities of water and ethanol are 0.997 and 0.7893 g⋅cm−3, respectively, at this temperature. Express your answer to two significant figures and include the appropriate units.Uranium tetrafluoride and zirconium tetrafluoride melt at 1035 °C and 912 °C respectively. They form a continuous series of solid solutions with a minimum melting temperature of 765 °C and composition x(ZrF4) = 0.77. At 900 °C, the liquid solution of composition x(ZrF4) = 0.28 is in equilibrium with a solid solution of composition x(ZrF4) = 0.14. At 850 °C the two compositions are 0.87 and 0.90, respectively. Sketch the phase diagram for this system and state what is observed when a liquid of composition x(ZrF4) = 0.40 is cooled slowly from 900 °C to 500 °C.