Answered: Consider a solution consisting of 1.75…

Consider a solution consisting of 1.75 mol water and 0.97 mol ethanol. Express your answers in three significant figures. a. What is the Gibbs energy of mixing? b. What is the entropy of mixing?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.35QE

See similar textbooks

Similar questions

Temperature influences solubility. Does temperature have the same effect on all substances? Justify your answer. (Hint: Consider Le Chateliers principle.)
The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
The lattice enthalpy of sodium chloride, H for NaCl(s)Na+(g)+Cl(g) is 787 kJ/mol; the heat of solution in making up 1 M NaCl(aq) is +4.0 kJ/mol. From these data, obtain the sum of the heats of hydration of Na+ and Cl. That is obtain the sum of H values for Na+(g)Na+(aq)Cl(g)Cl(aq) If the heat of hydration of Cl is 338 kJ/mol, what is the heat of hydration of Na+?
7.9. For a solution of and in which , what are the mole fractions of and in the vapor phase? Use conditions and data from exercise 7.8.
Vapor-pressure lowering is a colligative property, as are freezing-point depression and boiling-point elevation. What is a colligative property? Why is the freezing point depressed for a solution as compared to the pure solvent? Why is the boiling point elevated for a solution as compared to the pure solvent? Explain how to calculate T for a freezing-point depression problem or a boiling-point elevation problem. Of the solvents listed in Table 10-5, which would have the largest freezing-point depression for a 0.50 molal solution? Which would have the smallest boiling-point elevation for a 0.50 molal solution? A common application of freezing-point depression and boiling-point elevation experiments is to provide a means to calculate the molar mass of a nonvolatile solute. What data are needed to calculate the molar mass of a nonvolatile solute? Explain how you would manipulate these data to calculate the molar mass of the nonvolatile solute.
A forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar mass = 303.35 g/mol). She dissolves 1.22 0.01 g of the solid in 15.60 0.01 g benzene. The freezing point is lowered by 1.32 0.04C. a. What is the molar mass of the substance? Assuming that the percent uncertainty in the calculated molar mass is the same as the percent uncertainty in the temperature change, calculate the uncertainty in the molar mass. b. Could the chemist unequivocally state that the substance is cocaine? For example, is the uncertainty small enough to distinguish cocaine from codeine (C18H21NO3, molar mass = 299.36 g/mol)? c. Assuming that the absolute uncertainties in the measurements of temperature and mass remain unchanged, how could the chemist improve the precision of her results?
Consider a solution consisting of 1.75 mol water and 0.97 mol ethanol. What is the Gibbs energy of mixing? 5.12 kJ -4.02 kJ 3.21 kJ -6.25 kJ
The dissolution of ammonium nitrate (NH4NO3) in water is a classic example of a solute that has an endothermic enthalphy of solution (ΔHsolution). What is (are) the "driving force" (driving forces) for the dissolution of NH4NO3? Formation of dispersion interactions only. Formation of dispersion interactions and increasing entropy. Formation of ion-dipole interactions only. Increasing entropy only. Formation of ion-dipole interactions and decreasing entropy
Part C A solution is formed when the solute uniformly disperses throughout (or dissolves in) the solvent. The process can be described though three steps: A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. 1. separation of solvent-solvent particles, 2. breaking of solute-solute particles, and Action Enthalpy separation of solute 18.5 kJ/mol 3. formation of solute-solvent interactions. separation of solvent 19.8 kJ/mol formation of solute-solvent interactions -84.7 kJ/mol solute The overall energy change for the solution process, AHsoln , is the sum of the enthalpies of the three steps. Whether AHsoln is endothermic or exothermic depends on the relative magnitudes of AH1, AH2, and AH3, where the subscript indicates the step in the process corresponding to the enthalpy value. Calculate the enthalpy of solution in kilojoules per mole of solute. Enter your answer numerically in…
12.) Fure nquid A and B are mixed and the solutions result to a mixture with 0.300 mol A and 0.500 mol B at 353 K. What would be the mole fraction of B at the vapor phase if at the given temperature the vapor pressure of pure A is 291 Torr and pure B is 102 Torr? A. 0.375 B. 0.625 C. 0.369 D. 0.631 E. 0.826
Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies. Which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute-solvent interactions are the same for both solids. The solid with the smaller lattice energy. The solid with the smaller lattice energy, if entropy increases as a result of mixing and the solid with the larger lattice energy, if entropy decreases as a result of mixing. The solid with the larger lattice energy. They will have the same or very similar solubilities. The solid with the larger lattice energy, if entropy increases as a result of mixing and the solid with the smaller lattice energy, if entropy decreases as a result of mixing.
From your data in Part 1 of the experiment, you calculate the natural log of the partial pressure of water and 1/T value in K for 5 points between 50°C and 80°C. You make a graph of In(P) vs. 1/T and determine that the slope of the linear line is -4800 K. Use this information to calculate AHvap of water. Make sure to use R = 8.314 J mol-1-K-1. Oa. 46.6 kJ/mol Ob. 0.578 kJ/mol Oc. 31.5 kJ/mol O d. 39.9 kJ/mol