AP CHEM WKST
SOLIDS, LIQUIDS & SOLUTIONS REVIEW QUESTIONS
NAME: _________________________________________
1) What causes air pressure?
2) What is the quantity at STP for the following units of pressure and temperature?
a) ____________ mmHg
d) ____________ psi
g) ____________ °C
b) ____________ torr
e) ____________ atm
h) ____________ inHg
c) ____________ K
f)
____________ kPa
3) Suppose that, at exactly the same instant, two careless students drop glass containers of gas at a distance of 5 m on
either side of you. Before the containers break, they have equal volumes and the H 2S in one container and the SO2 in
the other are both at room temperature and pressure. Assuming that your nose is equally sensitive to both gases,
will you smell the rotten-egg odor of H2S first or the choking odor of SO2? Explain.
4) Rate the following gases in increasing order of diffusion rate.
C2H2, Cl2, H2S, N2, NO2, CH4
5) What two properties of real gas molecules cause deviations from ideal gas behavior?
6) When does a real gas approach ideal gas behavior?
7) Consider a sample of gas molecules for the following questions.
a) How is the average kinetic energy of the gas molecules related to temperature?
b) How is the average velocity of the gas molecules related to temperature?
c) How is the average velocity of the gas molecules related to the molar mass of the gas at constant temperature?
8) Consider 1.0 L of Ne gas at STP. Will the average KE, average velocity, and frequency of collisions of gas molecules
against the walls of the container increase, decrease, or remain the same under each of the following conditions.
a) T increases to 100°C
b) T decreases to –50°C
c) V is decreased to 0.5 L
d) the number of moles of Ne is doubled
9) Consider three identical flask filled with different gases.
flask A → N2 at 400 torr and 0°C
flask B → CO2 at 500 torr and 27°C
flask C → O2 at 300 torr and 30°C
a) In which flask is the average KE the greatest for the molecules of the gases?
b) In which flask is the average velocity the least for the molecules of the gases?
10) What two corrections did van der Waals make to the KMT model to make it work for real gases?
11) Tell whether the following pairs of variables are directly proportional or inversely proportional if all other variables
remain constant.
a) V and P
b) V and T (Kelvin)
c) P and T
d) P and mol
e) V and mol
12) Why are intermolecular forces so strong in liquids and solids, but so weak in gases?
13) What type(s) of interparticle forces are found in the following?
a) HCl
c) CH4
e) K2O
b) Ar
d) NH3
f) CO2
g) H2S
h) SO2
-214) In each of the following groups, pick the one that has the given property. Justify your answer.
a) highest boiling point: HCl, HBr, HI
e) highest surface tension: CH4, CH3CN, CH3OH
b) highest freezing point: H2O, H2S, H2Se
f) lowest vapor pressure at 20C: NH3, PH3, SbH3
c) lowest boiling point: N2, CO, CO2
g) greatest viscosity: CH3CH2CH3, CH3CH3, CH3CH2OH
d) lowest freezing point: CH4, CH3CH3, CH3CH2CH3
h) greatest heat of vaporization: Cl2, Br2, I2
15) Propane, C3H8, is a gas at room temperature; hexane, C6H14, is liquid; dedecane, C12H26, is a solid. Explain.
16) The shape of the meniscus of water is different than that of mercury in a glass tube. Why?
17) Would water rise higher by capillary action in a capillary tube made of glass or polyethylene, both with the same
diameter? Why? How high will it go?
18) Why does water bead up more on a car that is waxed than isn’t?
19) Indicate whether the following is soluble or insoluble in water: NH 3, PCl5, CH3OCH3, CH3OH, CH3(CH2)4CH3, I2, SF4,
SO3.
20) In the following heating curve, explain what is happening in terms of energy at the indicated positions.
B
Temperature
C
A
Time
21) What causes the supercooling of a liquid when freezing occurs?
Pressure
22) In the following phase diagram, label the following parts: solid, liquid, gas, critical temperature, critical pressure,
critical point, triple point.
Temperature
23) What is the temperature and pressure for water at the following:
a) triple point
b) critical point
24) Tell what type of solid the following would form.
a) graphite
e) SF6
b) O2
f) Kr
c) Ba(NO3)2
g) SiO2
d) Cu
h) K2O
i)
j)
k)
l)
(NH4)2SO4
PCl3
Pt
H2Se
-325) Tell what type of solid is indicated.
a) has nondirectional covalent bonds
b) has an extremely high melting point
c) good conductors of electricity and heat
d) made up of molecules
e) soft with a low melting point
f) consist of cations in an electron sea
g) hardest type of solids
26) Indicate which solid in each of the following is described by the given property.
a) highest melting point: Fe, NaCl, NO2
b) lowest melting point: KCl, S8, C
c) best conductor of electricity as a solid: P4, BaCl2, Pt
27) Why must bodily injections be isotonic with body cells?
28) During osmosis, what will pass through the semipermeable membrane and in which direction?
29) How does an increase in temperature affect the solubility of a:
a) solid solute
b) gaseous solute
c) liquid solute
30) What effect does pressure have on the solubility of a:
a) solid solute
b) liquid solute
c) gaseous solute
31) Which of the following would dissolve in water?
SF6, CH3OH, CH4, Ba(NO3)2, ClF3, CH3CH2CH2CH3
32) Explain how disorder affects the formation of a solution.
33) Explain what happens in terms of energy when a solution is formed.
34) Explain why adding a solute will change the vapor pressure of a pure solvent.
35) Describe what is meant by a positive and a negative deviation from Raoult’s Law.
36) What causes a solution to be ideal, or to have a positive or negative deviation in regards to Raoult’s Law and give
the signs for ΔH for each?
37) Explain what happens to the vapor pressure of a pure solvent when you add the following types of solute to it.
a) a nonvolatile, nondissociating solute
b) a nonvolatile, dissociating solute
c) a volatile solute with a vapor pressure lower than the pure solvent
d) a volatile solute with a vapor pressure higher than the pure solvent
38) Why does adding a solute to water cause a different freezing point and boiling point to occur?
39) Explain why a 1.0 m NaCl solution will have a higher boiling point than a 1.0 m sugar solution.
40) Explain why a 1.0 M NaCl solution will not change the temperature as much as your would expect when freezing or
boiling the solution.
41) List in order of decreasing freezing point the following solutions.
1.0 M C6H12O6
1.0 M NaCl
1.0 M MgCl2
1.0 M (NH4)3PO4
42) Explain how “reverse osmosis” works. Give an example of this being used.
43) Explain how “dialysis” works.
TERMS TO KNOW:
adhesive force
barometer
capillary action
cohesive force
colligative property
crenation
dialysis
diffusion
effusion
elastic collisions
hdrophillic
hdrophobic
heat of hydration
heat of solution
hemolysis
hypertonic
hypotonic
ideal gas
ideal solution
ion pairing
isotonic
joule
manometer
molar volume
negative deviation from Raoult’s Law
normal boiling point
osmosis
osmotic pressure
partial pressure
pascal
positive deviation from Raoult’s Law
real gas
semipermeable membrane
STP
surface tension
van’t Hoff factor
vapor pressure
viscosity
volatile