Please correct answer and don't use hand rating (b)(c)Substance is having a molecular weight of 132.8 g mol¹. Under normalmelting temperature of 430.65 K, the densities of solid Q and liquid Q are1080 and 1023 kg m³, respectively. Assuming there is a difference of 115 barin pressure, the melting point becomes 432.45 K. Calculate AS fusion andAH fusion at 1 bar for substance Q.Bromine in carbon tetrachloride forms a nearly ideal solution. The boilingpoint of pure bromine is 58.8 °C at 760 Torr.(i)(ii)Calculate the chemical potential of bromine relative to that of purebromine when Xbromine = 0.30 at its boiling point.If the activity coefficient of bromine in this solution was 0.93, whatwould be its vapor pressure?

Part (b) - Calculation for Substance QGiven Data:Molecular weight of Q = 132.8 g/mol Melting…

Answered: (b) (c) Substance is having a molecular…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 79QAP

See similar textbooks

Similar questions

6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .
Dichloromethane, CH2Cl2,is widely used as a degreaser and paint stripper. Its vapor pressure is 381.0 mm Hg at 21.9C and 465.8 mm Hg at 26.90C. Estimate (a) its heat of vaporization (Hvap). (b) its normal boiling point.
The molecular mass of butanol, C4H9OH, is 74.14; that of ethylene glycol, CH2(OH)CH2OH, is 62.08, yet their boiling points are 117.2 C and 174 C, respectively. Explain the reason for the difference.
The vapor pressure of liquid chloroform, CHCL3, is 100 mm Hg at 283K. A 0.302g sample of liquid CHCL3 is placed in a closed, evacuated 360 ml container at a temperature of 283K. Assuming that the temperature remains constant, will all of the liquid evaporate? What will the pressure un the container be when equilibrium is reach?
2. Which one of the following statements is incorrect? (a) According to the Gibbs phase rule, four phases of a pure substance cannot exist (b) All triple points correspond to a gas-liquid-solid equilibrium (c) The triple point in a P-T diagram becomes a triple line in a P-V diagram (d) The chemical potential determines which of several phases is the most stable
The standard boiling point of pure toluene is 384 K. At 384 K, the equilibrium vapor pressure of another pure liquid E is 0.250 bar. Their latent heats of vaporization delta Hm,vap are 32.30 kJ/mol for toluene and 16.15 kJ/mol for E. At what temperature would you estimate that the two substances, toluene and E, have the same equilibrium vapor pressure?
Suppose the vapor pressure of a substance is measured at twodifferent temperatures. (a) By using the Clausius–Clapeyronequation (Equation 11.1) derive the following relationshipbetween the vapor pressures, P1 and P2, and the absolute temperaturesat which they were measured, T1 and T2: (b) Gasoline is a mixture of hydrocarbons, a componentof which is octane (CH3CH2CH2CH2CH2CH2CH2CH3). Octane has a vapor pressure of 13.95 torr at 25 °C and a vaporpressure of 144.78 torr at 75 °C. Use these data and the equationin part (a) to calculate the heat of vaporization of octane.(c) By using the equation in part (a) and the data given in part(b), calculate the normal boiling point of octane. Compareyour answer to the one you obtained from Exercise 11.81.(d) Calculate the vapor pressure of octane at -30 °C.
The latent heat of fusion of water at 0Cis 6.025 kJ/mol and the molar heat capacities (Cp,m) of water and ice are 75.3 and 37.7 J K-1 mol-1, respectively. The Cp values can be taken to be independent of temperature. Calculate H for the freezing of 1 mol of supercooled water at -10.0C.
The fragment of H2O phase diagram is shown. What transition (e.g. liquid->solid, solid->gas... or none) would be observed when a sample of H2O initially at 0.003 atm and -5 C is heated at constant pressure to 0 C?
7. The vapor pressure of sulfur dioxide in the solid and liquid states are given by the equations: In Psolid = 29.28 – 4308/T In Pliquid = 24.02 – 3284/T where P is the vapor pressure expressed in Pa, and T is the absolute temperature. Calculate the temperature and the pressure of the triple point of sulfur dioxide.
(2) Sublimation. Figures below represent the phase diagrams for water and carbon dioxide. (a) Describe the difference in sublimation behavior under the pressure and temperature conditions prevailing on Earth. (b) How would you explain the sublimation of the polar ice caps on Mars during the Martian Summer? 217.7 METING FREZING Normal melting point Solid -Normal boiling point Liquid VAPOURISON COKDENSATION Gas 0.006 SUBLIMATION DEPOSITION 100 374.4 Temperature ("C) Pressure (atm)
Liquid mercury has a density of 13.69 g cm^-3, and solid mercury has a density of 14.690 g cm^-3 both being measured at the melting point, -38.87C, at 1 bar pressure. The heat of fusion is 9.75 J g^-1. Calculate the melting point of mercury at a pressure of 10 bar.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS