What is the molar Gibbs energy of mixing for the formation of a solution consisting of 100.0 g of methanol (M = 32.04 g mol') and 100 g of ethanol M = 46.07 g mol·') at 300K? Assume ideal solution behavior. [-1688]
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![What is the molar Gibbs energy of mixing for the formation of a solution consisting of 100.0 g
of methanol (M = 32.04 g mol') and 100 g of ethanol M = 46.07 g mol·') at 300K? Assume
ideal solution behavior. [-1688]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2c4896e9-f856-45f8-9abb-e3fc59ba0fb1%2F0af8a3b2-0b15-446f-95bc-3fd1993c2ed6%2F7xralz9.jpeg&w=3840&q=75)
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- What mass of a non-electrolyte solute is required, when mixed with 225 g H2O, to change the equilibrium vapor pressure of H2O from 1.013 x 105 Pa to 8.104 x104 Pa, at approximately 110 °C? The molar mass of the non-electrolyte solute is 62.07 g mol−1. Assume ideal behaviour for the solution.A solution is prepared by dissolving iodine, I2, in tetrachloromethane,CCI4 at 25 °c. What are the mole fractions of the solute and solvent for a solute of molality 0.100 mol kg-1? Hence calculate the change in the chemical potential of the solvent caused by the solute.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.
- The osmotic pressu re of an aqueous solution of urea at 300 K is 150 kPa. Calculate the freezing point of the same solution.Determine the (i) Gibbs energy, (ii) entropy, and (iii) enthalpy of mixing when 2.5 mol toluene is mixed with 2.5 mol of benzene at 298 K (assume an ideal solution)Estimate the mean ionic activity coefficient of CaCl2 in a solution that is 0.010 mol kg−1 CaCl2(aq) and 0.030 mol kg−1 NaF(aq) at 25 °C.
- One mole of a component A and twomoles of a component B are mixed at270C to form an ideal binary solution. calculate the Vmix , Gmix Hmix and Smix. Assume that R=8.314 JK1mol-1 ?The osmotic pressure of an aqueous solution of a non-ionic solute is 120 kPa at 300 K. Assuming that the molarity and molality of the solution are essentially equal for dilute solutions, calculate the temps at which this solution freezes and boils. (Kf(H2O)= 1.86 °/m, and Kb(H2O)= 0.512 °/m)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of 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. Find the freezing point of the solution(in C to 2 decimal places)
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of 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. Find the osmotic pressure in atm to three decimal placesA solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of 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 boiling point of the solution(in C to 2 decimal places)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of 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 two decimal places) 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)