From the equivalent conductivities at infinite dilution following at 18°C, find the value of Λ° for NH4OH: Ba(OH)2 Λ° = 228.8 BaCl2 Λ° = 120.3 NH4Cl Λ° = 129.8
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From the equivalent conductivities at infinite dilution following at 18°C, find the value of Λ° for NH4OH:
Ba(OH)2 Λ° = 228.8
BaCl2 Λ° = 120.3
NH4Cl Λ° = 129.8
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- There is a 15.85% by mass aqueous KCl (molecular weight 74.5513 g mol–1) solution at 25 °C. 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. Could you please find osmotic pressure?The excess Gibbs energy of solutions of methylcyclohexane (MCH) and tetrahydrofuran (THF) at 303.15 K were found to fit the expressionGE = RTx(1 − x){0.4857 − 0.1077(2x − 1) + 0.0191(2x − 1)2}where x is the mole fraction of MCH. Calculate the Gibbs energy of mixing when a mixture of 1.00 mol MCH and 3.00 mol THF is prepared.Calculate the value of the equilibrium constant, Ke , for the reaction Q(g)+X(g) = 2 M(g)+N(g) given that M(g) Z(g) 6 R(g) = 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) 9R(g) Kei 3.59 Kc2 0.567 Kc3 = 13.8 K. =
- Calculate the value of the equilibrium constant, Ke , for the reaction Q(g) + X(g) = 2 M(g) + N(g) given that M(g) = Z(g) 6 R(g) = 2 N(g) + 4Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kel = 3.52 K2 = 0.585 Kc3 12.3 K. IIAt 25°C the equivalent conductivities of dilute NaI solutions are as following:Find Λ° of NaI at 25°C1. (a) In the experiment carried out to determine the degree of association of benzoic acid in benzene (C6H6), the cooling curves of pure benzene and benzoic acid solution prepared by dissolving 0.358 g benzoic acid in 20 mL of benzene were obtained by using Beckmann thermometer, calibrated before the experiment. The cooling curves are given in the figure below. Calculate the degree of association of benzoic acid in benzene for the given solution. Ky= 5.055 K kg.mol-¹, dbenzene- 0.876 g.cm³, MBenzoic acid=122.12 g.mol-¹ T(°C) 2.88 2.38 Benzene Solution t(min)
- 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: Freezing Point of Solution in Degrees CelciusYou 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: Osmotic Pressure in atmYou 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: Boiling point of solution (in °C to one decimal place) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)
- 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 atmYou 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: Boiling Point in degrees CelciusThe 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.