Practice Problems 2

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4.) A nonvolatile liquid would a. have weak attractive forces between molecules b. evaporate rapidly at room temperature c. have a high vapor pressure at room temperature d. be a very "explosive" substance e. have strong attractive forces between molecules _____e_________ 5.) Which statement about the boiling point of water is incorrect a. The boiling point is greater than 100 o C in a pressure cooker. b. The boiling point is less than 100 o C for locations at low elevations. c. At sea level and at a pressure of 760 mm Hg, the boiling point is 100 o C. d. In a pressure cooker, shorter cooking times are required due to the change in boiling point. d. The boiling point is a consequence of a molecule's intermolecular forces. ____b__________ 6.) Which of the following statements is correct a. dipole-dipole interactions occur only between nonpolar molecules b. a hydrogen bond is an extremely weak dipole-dipole interaction c. London forces are "instantaneous" dipole-dipole interactions d. Hydrogen bonding occurs between any two hydrogen-containing molecules ____c__________ 7.) Which of the following substances would be expected to have the lowest boiling point a. a nonpolar liquid b. a polar liquid with hydrogen bonding c. a polar liquid with weak dipole-dipole interactions d. a nonvolatile liquid e. a polar liquid with strong dipole-dipole interactions ____a_________ 8.) Which of the following compounds is incorrectly matched with the predominant intermolecular force associated with that compound in the liquid state. compound intermolecular force a. CCl4 dipole-dipole interactions b. H2O hydrogen bonding c. BF3 London forces d. NH3 hydrogen bonding e. Br2 London forces ____a________
9.) The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Considering these two factors, predict the order of increasing boiling points for the following substances: H2, NaCl, H2O, and CO2. a. CO2 < H2 < NaCl < H2O b. H2 < CO2 < H2O < NaCl c. H2O < NaCl < CO2 < H2 d. H2 < NaCl < H2O < CO2 e. NaCl < H2O < CO2 < H2 ____b________ 10.) The vapor pressure of PBr 3 reaches 400 mm Hg at 150 o C. The vapor pressure of PCl 3 reaches 400 mm Hg at 57 o C. a. At 100 o C which substance should evaporate at the faster rate ____PCl 3 _____ b. Which substance should have the lower normal boiling point ____ PCl 3 ____ c. Which substance should have the weaker intermolecular forces ____ PCl 3 ___ d. At 50 o C which substance should have the higher vapor pressure ____ PCl 3 ____ 11.) Consider the phase diagram shown below. a. What phase(s) is/are present at point A ___liquid_____________________ b. What phase(s) is/are present at point B _solid, liquid, gas_______________ c. Name point C and explain its significance. _critical point- above the critical temp., substance cannot be liquefied, regardless of pressure._________________ d. Starting at D, if the pressure is lowered while the temperature remains constant, describe what will happen. D = solid phase. As P is lowered, solidgas dividing line is reached. Solid will sublime. ___________
Page 1: Practice Problems 17 Chapter 12 CHE
Page 5 and 6: 16.) Which of the following should
Page 7: 24.) For the solid forms of the fol

Practice Problems 2

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