Concept explainers
Knudsen effusion cells are used to determine vapor pressures of high-temperature materials. For example, a Knudsen cell is filled with tungsten and heated to
Want to see the full answer?
Check out a sample textbook solutionChapter 19 Solutions
Bundle: Physical Chemistry, 2nd + Student Solutions Manual
- Which has the greatest vapour pressure at 25°C? SiO2 CO2 H2Oarrow_forwardAt what temperature and pressure is the triple point of CO2?arrow_forward2. A closed vessel of volume 10.0 L initially contains 1.303 g of water and no water vapor. Please calculate the mass of liquid water remaining once the system reaches equilibrium at 30 degrees Celsius. The vapor pressure of water at that temperature is equal to 0.0418 atm.arrow_forward
- The vapor pressure of water at 30 °C is 4.24 kPa. Calculate the vapor pressure if 95.0 g of glycerol, C₃H₈O₃(l), is added to 100.0 mL of water. The density of water at 30 °C is 0.996 g・mL⁻¹.arrow_forwardThe phase diagram for helium is shown. Liquid helium can exist in two possible forms; Helium II and Helium I. Explain. (i) What is the maximum temperature at which Helium – II can exist? (ii)What is the minimum pressure at which solid helium can exist? (iii) What is the normal boiling point for Helium – 1? (iv) Can solid helium sublime?arrow_forwardThe standard enthalpy of vaporization (H°vap) of ethylenediamine ((NH2CH2)2) is 44.0 kJ/mol.The normal boiling point of ethylenediamine is 116.5°C.Calculate the vapour pressure of ethylenediamine at 102.0°C.arrow_forward
- The vapor pressure of liquid carbon tetrachloride, CC14, is 15, 539 Pa at 290 K and 69,518 Pa at 340 K. The vapor pressure of solid carbon tetrachloride is 275 Pa at 232 K and 2,092 Pa at 250 K. Estimate the temperature of the triple point of carbon tetra- chloride.arrow_forwardCalculate the change in the chemical potential of liquid water and water vapor when the pressure is increased from 1.0 atm to 10 atm at 100°C. Discuss the effect of the pressure increase on the equilibrium between the liquid water and the water vapor. Assume that water vapor behaves perfectly and the density of water is 1 g/cm3.arrow_forwardPrior to the discovery that freon-12 (CF2Cl2) is harmful to the Earth’s ozone layer it was frequently used as the dispersing agent in spray cans for hair spray etc. Estimate the pressure that a can of hair spray using freon-12 has to withstand at 40 °C, the temperature of a can that has been standing in sunlight. The enthalpy of vaporization of freon-12 at its normal boiling point of −29.2 °C is 20.25 kJ mol−1; assume that this value remains constant over the temperature range of interest.arrow_forward
- At which temperature is the vapor pressure of ethanol equal to 80. kPa?arrow_forward(b) Using the Crystallographer's formula to determine the density (in g/cm³) of Po: ρ = Σ Ζ * Μ Vell* N You must know that a primitive cubic cell has Z = 1 Since Po is a metal, the value of "i" = 1, since it's the only entity! MM of Po= 208.998 g/mol Vcell (in cm³) = a³ Vcell (3.36 x 10-8 cm)³ = 3.793 x 10-23 cm³ N = 6.022 x 1023 atoms/mol Thus: p = (1 atom/cell) (208.998 g/mol) = 9.16 g/cm³ (3.793 x 10-23 cm³) (6.022 x 1023)arrow_forwardThe vapor pressure of ammonia at –50°C is 0.4034 atm; at 0°C, it is 4.2380 atm. (a) Calculate the molar enthalpy of vaporization (AHvap) of ammonia. (b) Calculate the normal boiling temperature of NH3(€).arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY