Here you have 0.30 mole of benzene and 0.70 mole of methylbenzene at 25 °C. a. The following shows chemical potential curves of three states of methylbenzene. Explain how the chemical potential curve of liquid would change as benzene is dissolved in methylbenzene. b. Explain how boiling-point elevation and freezing-point depression occur in a solution using the graph. Mark where the boiling point and freezing point of the solution would be. Solid Liquid Vapour Solid stable Liquid T. Vapour stable stable Temperature, T Chemical potential, u

Here you have 0.30 mole of benzene and 0.70 mole of methylbenzene at 25 °C. a. The following shows chemical potential curves of three states of methylbenzene. Explain how the chemical potential curve of liquid would change as benzene is dissolved in methylbenzene. b. Explain how boiling-point elevation and freezing-point depression occur in a solution using the graph. Mark where the boiling point and freezing point of the solution would be. Solid Liquid Vapour Solid stable Liquid T. Vapour stable stable Temperature, T Chemical potential, u

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section13.7: Colligative Properties Of Solutions

Problem 13.11PSP

See similar textbooks

Similar questions

This question is related to chemical potential in a solution and how it relates to physical properties. What is the relationship between the freezing point of a dilute solution vs. that of the pure liquid? Provide an explanation for this relationship based on thermodynamics. If the temperature is increased in a saturated solution of A in equilibrium with solid A, what will you observe? Give a thermodynamic explanation for this (based on chemical potential and mole fraction)
The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL
At 90°C, the vapor pressure of pure 1,2-dimethylbenzene (orthoxylene) is 20 kPa and that of pure 1,3-dimethylbenzene (methaxylene) is 18 kPa. What is the composition of the liquid phase that boils at 90°C whose total vapor pressure is 19 kPa? What is the composition of the vapor phase in equilibrium with the solution?
The density of an aqueous solution increases as solutes such as salts are added. What bearing might this have on predicting whether the aqueous solution will be on the top or on the bottom for an extraction?
During the formation of the n-butyl bromide, a washing is carried out with the NaHCO3 solution and 2 phases are formed again. What is the organic phase? Justify
List 7 real-life applications in Chemical Equilibrium in a Liquid Phase and list 7 real-life applications in Distribution of a Solute between Immiscible Solvents.
Tube 1 and Tube 2: at 20C and 4 mL(0,1M NaOH) and 10 mL Benzoic acid,solution concentration . Calculate solubility at 20C as molality. (take density of the solution as 1 g/mL). And then find ln(molality)
Benzene and Toluene form nearly ideal solutions. The boiling point of purer benzene is 80.1°C. Calculate the chemical potential of benzene relative to that of pure benzene when Xbenzene=0.30 (mole fraction) at its boiling point. If the activity coefficient of benzene in this solution were actually 0.93 rather than 1.00, what would be its vapor pressure?
Sodium chloride (NaCl) was isolated from SiO2 and CaCO3 by dissolving it in distilled water. Unmentioned is that CaCO3 is slightly soluble in water (0.001 g/100 mL). Describe the effect this fact will have on each component of the mixture: will the “isolated“ mass of each be greater than, equal to, or less than that in the sample?
Calculate the solubility of 1,4-dibromobenzene in benzene at 25.000C and at 45.000 assuming that these two compounds form ideal mixtures. The enthalpy of fusion of 1,4-dibromo benzene is 20.39 kJ mol-1 and its melting point is 87.400C. Report the solubility of 1,4-dibromo benzene in benzene as (a) its mole fraction, and (b) grams of 1,4-dibromo benzene in 1000 grams of benzene.
A solution of 5.00 g acetic acid in 100 g benzene freezes at 3.380C. A solution of 5.00 g acetic acid in 100 g water freezes at -1.490C. Find the molecular weight of acetic acid from each of these data. What can you conclude about the state of the acetic acid molecules dissolved in each of these solvents?
During the experiment, to obtain the Beer's law plot for FeSCN2+ ion at various concentrations, the following solutions are mixed to form a solution of FeSCN2+ through reaction as follows: Fe3+ + SCN- <=> FeSCN2+ 2.9 mL 0.2 M Fe(NO3)3 in 0.50M HNO3 , 1.5 mL 0.50M HNO3, and 1.4 mL 2.00 x 10–2 M KSCN in 0.50M HNO3. Assuming all SCN- ion is converted to product FeSCN2+ , determine the concentration of FeSCN2+ in the reaction mixture.