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 enthalpy of fusion 75. °C 10.00 kJ/mol boiling point enthalpy of vaporization 110. °C 36.00 kJ/mol 1.70 g/cm³ (solid) density 1 1 47. J.K ·mol (solid) 1.20 g/mL (liquid) heat capacity 1 1 52. J.K mol (liquid) 64. J-K mol (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 he observed during this experiment. temperature (°C) 150- 140- 130- 120- 110- 100- 90- 80- 70- 60- 0 heat added (kJ/mol) 5

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 enthalpy of fusion 75. °C 10.00 kJ/mol boiling point enthalpy of vaporization 110. °C 36.00 kJ/mol 1.70 g/cm³ (solid) density 1 1 47. J.K ·mol (solid) 1.20 g/mL (liquid) heat capacity 1 1 52. J.K mol (liquid) 64. J-K mol (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 he observed during this experiment. temperature (°C) 150- 140- 130- 120- 110- 100- 90- 80- 70- 60- 0 heat added (kJ/mol) 5

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...

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Similar questions

Describe the behavior of a liquid and its vapor in a closed vessel as the temperature increases.
8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.
Carbon tetrachloride, CCl4, has a vapor pressure of 213 torr at 40.C and 836 torr at 80.C. What is the normal boiling point of CCl4?
he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?
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?
Consider the following data for the vapor pressure of diethyl ether, a widely used anesthetic in the early days of surgery. Follow the instructions in Question 13 to estimate the heat of vaporization of diethyl ether.
If you've ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopic basis how a vapor pressure builds up in a closed container above a liquid. What processes in the container give rise to this phenomenon?
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?
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 a substance X with a Hvap = 20.3 kJ/mol and Hfus = 9.0 kJ/mol. The melting point, freezing point, and heat capacities of both the solid and liquid X are identical to those of water. a If you place one beaker containing 50 g of X at 10C and another beaker with 50 g of H2O at 10C on a hot plate and start heating them, which material will reach the boiling point first? b Which of the materials from part a, X or H2O, would completely boil away first? c On a piece of graph paper, draw the heating curve for H2O and X. How do the heating curves reflect your answers from parts a and b?
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?

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