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 I have been determined: melting point enthalpy of fusion 75. °C 10.00 kJ/mol boiling point 110. °C enthalpy of vaporization 36.00 kJ/mol 1.70 g/cm³ (solid) density 47. J.K mol (solid) 1.20 g/mL (liquid) heat capacity 64. J.K 52. J.K mol mol 1 (liquid) (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 8.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. temperature (°C) 150- 140- 130- 120- 110- 100- 90- 80- 70- 60- 50. 0 heat added (kJ/mol) 田 X G

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 I have been determined: melting point enthalpy of fusion 75. °C 10.00 kJ/mol boiling point 110. °C enthalpy of vaporization 36.00 kJ/mol 1.70 g/cm³ (solid) density 47. J.K mol (solid) 1.20 g/mL (liquid) heat capacity 64. J.K 52. J.K mol mol 1 (liquid) (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 8.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. temperature (°C) 150- 140- 130- 120- 110- 100- 90- 80- 70- 60- 50. 0 heat added (kJ/mol) 田 X G

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.87PAE: 8.87 Use the vapor pressure curves illustrated here to answer the questions that follow. (a) What is...

See similar textbooks

Similar questions

8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
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?
Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?
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?
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.
A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 C. (a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the ideal gas law, PV = nRT.) (b) The vapor pressure of methanol at 30 C is 158 torr. What mass of methanol actually evaporates? Is liquid in equilibrium with vapor in the vessel?
Describe the behavior of a liquid and its vapor in a closed vessel as the temperature increases.
Referring to Figure 9.7, state what phase(s) is (are) present at (a) 1 atm, 10C. (b) 3 mm Hg, 20C. (c) 1000 mm Hg, 75C.
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?
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.
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 types of intermolecular forces in a substance are identical whether it is a solid, a liquid, or a gas. Why then does a substance change phase from a gas to a liquid or to a solid?