liquidssolidsandsolutionpropertiesreviewtest by 8CuFyj


									Name ______________________________________ Date _______

                                                 Solid, Liquids & solutions review

1) Which one of the following decreases as the strength of           c) CO2
the attractive intermolecular forces increases?                      d) H2O
a) heat of vaporization                                              e) Cu
b) normal boiling temperature
c) extent of deviations from the ideal gas law                       9) At 1atm of pressure and a temperature of 0oC, which
d) sublimation temperature of a solid                                phase(s) of water can exist?
e) vapor pressure of a liquid                                        a) ice and water
                                                                     b) ice & water vapor
2) Hydrogen bonding accounts for which of the following              c) water only
observation?                                                         d) water vapor only
a) Hydrogen naturally exists as a diatomic molecule                  e) ice only
b) H2 is easily combustible with O2
c) water molecules are bent or “V-shaped”                            11) Which of the following has the highest melting
d) air is more dense than hydrogen gas                               temperature?
e) for its molar mass, water has a high boiling point                a) H2O
                                                                     b) CO2
3) Which of the following would you expect to have the               c) S8
highest boiling point?                                               d) MgF2
a) F2                                                                e) P4
b) Cl2
c) Br2                                                               12) You are given the following boiling point data:
d) I2                                                                a) water                   100oC
e) all of the above have the same boiling point                      b) methanol                64.9oC
                                                                     c) ethanol                 78.5oC
4) The molecules in a sample of solid SO2 (draw it!!) are            d) diethyl ether           34.5oC
attracted to each other by a combination of                          e) ethylene glycol         198oC
a) London forces and H-bonding                                       Which one of the above liquids would you expect to have
b) H bonding and ionic bonding                                       the highest vapor pressure at room temperature?
c) covalent bonding and dipole-dipole interactions
d) London forces and dipole-dipole interactions                      13) In which of the following processes will energy be
e) none of these                                                     evolved (released) as heating?
                                                                     a) sublimation
5) Which statement regarding water is true?                          b) crystallization (process when something freezes)
a) Energy must be given off in order to break the crystal            c) vaporization
lattice of ice & convert it to a liquid                              d) melting
b) H bonding is stronger than covalent bonds                         e) none of these
c) liquid water is less dense than solid water
d) only covalent bonds are broken when ice melts                     14) How much energy is needed to convert 64.0 grams of ice
e) all of the statements are false                                   at 0.00oC to water at 75.0oC?
                                                                     a) 10.1 kJ
6) Which substance involves no attractive forces except              b) 20.7 kJ
London dispersion forces?                                            c) 31.4 kJ
a) NaCl (l)                                                          d) 41.4 kJ
b) HF (l)                                                            e) 65.8 kJ
c) Ne (g)
d) H2O (l)                                                           15) A certain substance, X, has a triple-point temperature of
                                                                     20oC at a pressure of 2.0 atm.
                                                                     Which one of the statements a- d cannot possibly be true?
7) True or false – Water sits in an open beaker. Assuming            a) X can exist as a liquid above 20oC.
constant temperature and pressure, the rate of evaporation           b) X can exist as a solid above 20oC.
decreases as the water evaporates.                                   c) Liquid X can exist as a stable phase at 20oC, 1 atm
                                                                     d) Both liquid and solid X have the same vapor pressure at
8) A certain solid substance that is very hard, has a very high      20oC.
melting point, and is non-conducting unless melted is most           e) All could be true
likely to be
a) I2
b) NaCl
Questions 16 – 17 refer to the following compounds                  b) 6.8 M
         a) KBr (s)                                                 c) 0.16 M
         b) C2H5OH (l)                                              d) 12.4 mL
         c) CO2 (g)                                                 e) 15.8 mL
         d) C6H12 (l)
Select the letter that best satisfies each of the following         23) Rank the following compounds according to increasing
descriptions.                                                       solubility in water.
16) likely to be miscible in all proportions with water (this       I. CH3-CH2- CH2 -CH3
means that no matter how much you add it will completely            II. CH3- CH2-O- CH2- CH3
mix with water.)                                                    III. CH3- CH2-OH
17) produces a conducting solution when dissolved in water          IV. CH3-OH
                                                                    a) I<III<IV<II
18) A solution of H2O2 is 30.0% H2O2 by mass and has a              b) I<II<IV<III
density of 1.11g/mL. Calculate the molarity of the solution.        c) III<IV<II<I
a) 7.94 M                                                           d) I<II<III<IV
b) 8.82 M
c) 9.79 M                                                           24) The vapor pressure of water at 25.0oC is 23.8 torr.
d) 0.980 M                                                          Determine the mass of glucose (molar mass=180 g/mol)
                                                                    needed to add 500.0g of water to change the vapor pressure
19) In a 0.1 M NaCl I water, which one of the following will        to 23.1 torr. Don’t do this one unless you like solving
be closest to 0.1?                                                  algebra problems. A problem this involved would not be on
a) the mole fraction of NaCl                                        the test.
b) the mass fraction of NaCl                                        a) 72 g
c) the mass percent of NaCl                                         b) 152 g
d) the m of NaCl                                                    c) 103 g
                                                                    d) 115 g
20) How many ml of 18.4M H2SO4 are needed to prepare                e) 36 g
600.0 mL of 0.10M H2SO4?
a) 1.8 mL                                                           25) A salt solution sits in an open beaker. Assuming constant
b) 2.7 mL                                                           temperature and pressure, the vapor pressure of the solution
c) 3.3 mL                                                           a) increases over time
d) 4.0 mL                                                           b) decreases over time
e) 4.6 mL                                                           c) stays the same over time
                                                                    d) need to know which salt is in the solution to answer this
21) Which of the following concentration measures will              e) need to know the T & P to answer this.
change in value as the temperature of a solution changes?
a) mass percent                                                     26) Determine the change in boiling point for 300.0g of
b) mole fraction                                                    carbon disulfide (Kb = 2.34oC kg/mol) if 35 g of a
c) molality                                                         nonvolatile, nonionizing compound is dissolved in it. The
d) molarity                                                         molar mass of the compound is 70.0 g/mol and the boiling
e) none of these                                                    point of the pure carbon disulfide is 46.2 oC.
                                                                    a) 13.4 oC
22) Concentrated nitric acid is a solution that is 70% HNO 3        a) 10.9 oC
by mass. The density of this acid is 1.42 g/mL. What is the         a) 7.7 oC
molarity of this acid?                                              a) 15.6 oC
a) 0.06 M                                                           a) 3.9 oC


1) The Hvap of acetone (molar mass = 58 g/ mol) is 30.3 kJ/mol at its boiling point. How many kJ of heat would be released by
the condensation of 5.00 g of acetone?
2) A substance has the following properties:
        Normal boiling point = 500 K
        Normal melting point = 200 K
        Triple point = 150 K at 0.75 atm

         i) Draw a rough sketch of the phase diagram for the substance
         ii) On the sketch, label the points given above, as well as the regions for the solid, liquid, & gas phase

4) A solution is prepared from 31.4 g of a nonvolatile, nondissociating solute and 85.0 g of water. The vapor pressure of the
solution at 60oC is 142 torr. The vapor pressure of water at 60 oC is 150.torr. What is the molar mass of the solute?

3)d more e so higher LDF
4)d draw it. Its bent & O is more electronegative than S
11)d it’s an ionic bond
12)d low bp means low IMF which means high vapor pressure
13) b crystals are formed from solution, the ionic bonds are reformed – bond formation means releases
21) d
26)last one marked a, oops. 3.9

1) 2.61 kJ

4) 119 g/mol

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