Substance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined: melting point 70. °C boiling point 115. °C enthalpy of fusion enthalpy of vaporization 10.00 kJ/mol 24.00 kJ/mol 2.30 g/cm³ (solid) 2.00 g/mL (liquid) density 31. J-Kmol (solid) do heat capacity 47. J-K¯-mol¯' (liquid) 55. J-Kmol (vapor) You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at 50 °C is put into an evacuated flask and heated at a constant rate until 10.0 kl/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. 150 140 130 120 100 90 70 30 heat added (k/mol) (3.) aruedu

Substance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined: melting point 70. °C boiling point 115. °C enthalpy of fusion enthalpy of vaporization 10.00 kJ/mol 24.00 kJ/mol 2.30 g/cm³ (solid) 2.00 g/mL (liquid) density 31. J-Kmol (solid) do heat capacity 47. J-K¯-mol¯' (liquid) 55. J-Kmol (vapor) You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at 50 °C is put into an evacuated flask and heated at a constant rate until 10.0 kl/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. 150 140 130 120 100 90 70 30 heat added (k/mol) (3.) aruedu

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 23QAP: A pure substance X has the following properties: Mp=90C, increasing slightly as pressure increases;...

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8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
A pure substance X has the following properties: Mp=90C, increasing slightly as pressure increases; normal bp=120C; liquid vp=65mm Hg at 100C, 20 mm Hg at the triple point. (a) Draw a phase diagram for X. (b) Label solid, liquid, and vapor regions of the diagram. (c) What changes occur if, at a constant pressure of 100 mm Hg, the temperature is raised from 100C to 150C?
The molar heat of fusion of sodium metal is 2.60 kJ/mol, whereas its heat of vaporization is 97.0 kJ/mol. a. Why is the heat of vaporization so much larger than the heat of fusion? b. What quantity of heat would be needed to melt 1.00 g sodium at its normal melting point? c. What quantity of heat would be needed to vaporize 1.00 g sodium at its normal boiling point? d. What quantity of heat would be evolved if 1.00 g sodium vapor condensed at its normal boiling point?
Consider the following data for xenon: Triple point: 121C, 280 torr Normal melting point: 112C Normal boiling point: 107C Which is more dense, Xe(s) or Xe(l)? How do the melting point and boiling point of xenon depend on pressure?
Water at 0C was placed in a dish inside a vessel maintained at low pressure by a vacuum pump. After a quantity of water had evaporated, the remainder froze. If 9.31 g of ice at 0C was obtained, how much liquid water must have evaporated? The heat of fusion of water is 6.01 kJ/mol and its heat of vaporization is 44.9 kJ/mol at 0C.
The heats of vaporization of liquid O2, liquid Ne, and liquid methanol, CH3OH, are 6.8 kJ/moL 1.8 kJ/mol, and 34.5 kJ/mol, respectively. Are the relative values as you would expect? Explain.
The following data are the equilibrium vapor pressure of limonene, C10H16, at various temperatures. (Limonene is used as a scent in commercial products.) (a) Plot these data as ln P versus 1/T so that you have a graph resembling the one in Figure 11.13. (b) At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is it 650 mm Hg? (c) What is the normal boiling point of limonene? (d) Calculate the molar enthalpy of vaporization for limonene using the Clausius-Clapeyron equation.
8.87 Use the vapor pressure curves illustrated here to answer the questions that follow. (a) What is the vapor pressure of ethanol (C2H5OH) at 60°C? (b) Considering only carbon disulfide (CS2) and ethanol, which has the stranger intermolecular forces in the liquid state? (c) At what temperature does heptane (C7H16) have a vapor pressure of 500 mm Hg? (d) What are the approximate normal boiling pains of each of the three substances? (e) At a pressure of 400 mm Hg and a temperature of 70°C, is each substance a liquid, a gas, or a mixture of liquid and gas?