Concept explainers
Interpretation:
The state/s of Cl2 in the cylinder needs to be determined.
Concept introduction:
Critical point is the point at which both the liquid and the gas phase of a substance have the same density. At critical point, the liquid and vapor phases are indistinguishable. Just below the critical point, the surface separating the liquid from its vapor is observed. When a liquid is approaching its critical point, density of the liquid decreases and density of the vapor increases, surface tension of the liquid becomes zero. Critical temperature and pressure indicates the maximum temperature and pressure at which a liquid can exist. A gas can be liquefied only below its critical temperature.
Want to see the full answer?
Check out a sample textbook solutionChapter 12 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
- You and a friend each synthesize a compound with the formula XeCI2F2. Your compound is a liquid and your friend's compound is a gas (at the same conditions of temperature and pressure). Explain how the two compounds with the same formulas can exist in different phases at the same conditions of pressure and temperature.arrow_forwardAnswer the following questions: (a) If XX behaved as an ideal gas, what would its graph of Z vs. P look like? (b) For most of this chapter, we performed calculations treating gases as ideal. Was this justified? (c) What is the effect of the volume of gas molecules on Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (d) What is the effect of intermolecular attractions on the value of Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (e) In general, under what temperature conditions would you expect Z to have the largest deviations from the Z for an ideal gas?arrow_forward5-106 The normal boiling point of hexane, C6H14, is 69°C, and that of pentane, C5H12, is 36°C. Predict which of these compounds has a higher vapor pressure at 20°C.arrow_forward
- In each of the following groups of substances, pick the one that has the given property. Justify your answer. a. highest boiling point: HBr, Kr, or Cl2 b. highest freezing point: H2O, NaCl, or HF c. lowest vapor pressure at 25C: Cl2, Br2, or I2 d. lowest freezing point: N2, CO, or CO2 e. lowest boiling point: CH4, CH3CH3, or CH3CH2CH3 f. highest boiling point: HF, HCl, or HBr g.arrow_forwardIn terms of the kinetic molecular theory, in what ways are liquids similar to gases? In what ways are liquids different from gases?arrow_forwardCarbon 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?arrow_forward
- What types of solids are these substances? (a) The hydrocarbon decane, C10H22, has a melting point of 31 C and is a poor electrical conductor. (b) Solid MgCl2 has a melting point of 714 C and conducts electricity only when melted.arrow_forwardHow many grams of water at 0C will be melted by the condensation of 1 g of steam at 100C?arrow_forwardIn terms of the kinetic molecular theory, in what ways are liquids similar to solids? In what ways are liquids different from solids?arrow_forward
- Based on the data below, what mass of propane must be burned to supply the heat required to vaporize 7.25 kg of water at 25 ºC? The ΔHvapof water at 25 ºC is 44.0 kJ/mol. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O (l) ΔH = − 2.22 x 103kJ A. 352 g B. 176 g C. 567 g D. 88.6 g E. 245 garrow_forwardIdeal Gas Law A sample of liquid acetone is placed in a .035 L flask and vaporized by heating to 75°C at 102 atm. The vapor weighs 5.87 g Calculate the number of moles of the acetone. where V = volume in liters P = pressure in atmosphere n = moles T=temperature in Kelvin R= universal gas constant, =0.0821 L atm/mol. K =8.314 L kPa/mol, Karrow_forwardUse vapor pressure. A student leaving campus for spring break wants to make sure the air in her dorm room has a high water vapor pressure so that her plants are comfortable. The dorm room measures 3.76 m × 4.17 m × 3.31 m and the student places a pan containing 1.62 L of water in the room. Assume that the room is airtight, that there is no water vapor in the air when she closes the door, and that the temperature remains a constant 25 °C. The vapor pressure of water at 25 °C is 23.8 mm Hg. (a) Calculate the pressure that the water vapor would exert if all of the liquid water evaporated. mm Hg (b) Will all of the water in the pan evaporate?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning