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WorksheetsHonors Chemistry Final Review Part 2
Total questions: 45
Worksheet time: 23mins
Name
Class
Date
1.
According to kinetic-molecular theory, particles of an ideal gas
a)
attract each other but do not collide
b)
repel each other and collide
c)
neither attract nor repel each other but collide
d)
neither attract nor repel each other and do not collide
2.
Molecules at the surface of a liquid can enter the vapor phase only if
a)
equilibrium has not been reached
b)
the concentration of the vapor is zero
c)
the energy ig high enough to overcome attractive forces of liquid
d)
condensation is not occurring
3.
If the rate of evaporation from the surface of a liquid exceeds the rate of condensation
a)
the system is in equilibrium
b)
the liquid is boiling
c)
energy as heat is no longer available
d)
the concentration of the vapor is increasing
4.
The kinetic molecular theory explains the behavior of
a)
gases only
b)
solids and liquids only
c)
liquids and gases only
d)
solids, liquids and gases
5.
At the triple point, water can
a)
have only three pressure values
b)
exist in equilibrium in three different phases
c)
only be present as a vapor
d)
exist only as a solid
6.
Whenever a liquid changes to a vapor, it
a)
absorbs energy from its surroundings
b)
is in equilibrium with its vapor
c)
is boiling
d)
is condensing
7.
During phases changes, the temperature of the substance
a)
remains constant
b)
increases
c)
decreases
d)
approaches water's boiling point
8.
Why does the Cartesian diver (medicine dropper) sink when you squeeze the bottle?
a)
pressure inside the bottle decreases
b)
temperature inside the bottle increases
c)
volume of gas inside the medicine dropper decreases
d)
numer of moles of gas inside the medicine dropper increases
9.
If the temperature of a fixed quantity of gas decreases and the pressure remains unchanged...
a)
its volume increases
b)
its volume is unchanged
c)
its volume decreases
d)
its density decreases
10.
Which principle says that under similar pressures & temperatures, equal volumes of gases contain the same number of molecules?
a)
Boyle
b)
Graham
c)
Avogadro
d)
Dalton
11.
Graham's Law: the rate of diffusion of 2 gases at the same temperature and pressure are inversely proportional to
a)
their volumes
b)
the square roots of their molar masses
c)
their compressibilities
d)
their rates of vaporization
12.
Which of the following best describes energy in the form of heat?
a)
energy transferred between samples of matter because of a difference in temperatures
b)
measure of average kinetic energy of particles in a sample of matter
c)
energy stored in a sample of matter
d)
bond energy
13.
Why would a camper near the top of Mt. Everest find that water boils at less than 100 degrees C?
a)
there is greater atmospheric pressure than at sea level
b)
the flames are hotter at that elevation
c)
the atmosphere has less moisture
d)
there is less atmospheric pressure than at sea level
14.
A reaction is spontaneous if ΔG is
a)
zero
b)
negative
c)
positive
d)
greater than ΔH
15.
Enthalpy change is the
a)
pressure change of a system at constant temperature
b)
temperature change of a system at constant pressure
c)
entropy change of a system at constant pressure
d)
amount of energy absorbed/lost by system at constant pressure
16.
The enthalpy of formation of an element is
a)
negative
b)
positive
c)
zero
d)
negative or positive, depending on which element
17.
What is the order of strength of intermolecular forces from weak to strong?
a)
dipole-dipole, dispersion, hydrogen
b)
hydrogen, dispersion, dipole-dipole
c)
dispersion, dipole-dipole, hydrogen
d)
hydrogen, dipole-dipole, dispersion
18.
Litmus is _____ in an acid & _____ in a base
a)
clear, pink
b)
pink, clear
c)
red, blue
d)
blue, red
19.
The heat of vaporization is the energy required to transform a ____ to a _____.
a)
gas, liquid
b)
solid, gas
c)
solid, liquid
d)
liquid, gas
20.
As ice melts, the water molecules
a)
go from well-ordered phase to less-ordered phase
b)
go from less-ordered phase to more-ordered phase
c)
stay ordered the same as in ice
d)
none of the above
21.
2 factors that determine whether a reaction will occur spontaneously are the ΔH of a reaction system and...
a)
the pressure in the system
b)
the concentration of the reactants in the system
c)
the randomness of the particles at the end of the reaction
d)
the quickness of the reaction
22.
In an endothermic reaction, the total energy at the beginning of the reaction is
a)
greater than the total energy at the end of the reaction
b)
less than the total energy at the end of the reaction
c)
equal to the total energy at the end of the reaction
d)
none of the above
23.
Spontaneous reactions are driven by
a)
decreasing enthalpy & decreasing entropy
b)
increasing enthalpy & decreasing entropy
c)
decreasing enthalpy & increasing entropy
d)
increasing enthalpy & increasing entropy
24.
The change in energy represented by a thermochemical equation is
a)
equal to the # of moles of substances undergoing a change
b)
indirectly proportional to the # of moles undergoing change
c)
directly proportional tho the # of moles undergoing change
d)
less than the number of moles undergoing change
25.
To be effective, a collision requires
a)
sufficient energy
b)
a favorable orientation
c)
sufficient energy & a favorable orientation
d)
a reaction mechanism
26.
The minimum energy required for an effective collision is called
a)
energy of enthalpy
b)
activation energy
c)
free energy
d)
kinetic energy
27.
The energy of the activated complex is higher than the energy of only the reactants.
a)
True
b)
False
28.
The higher the concentration of reactants
a)
the higher the reaction rate
b)
the slower the reaction rate
29.
Catalysts generally affect chemical reactions by changing endothermic reactions into exothermic reactions.
a)
True
b)
False
30.
A reaction order is found by comparing the concentration ratio with the
a)
rate ratio
b)
time ratio
c)
temperature ratio
d)
pressure ratio
31.
A very high value of Keq indicates that
a)
equilibrium is reached slowly
b)
products are favored
c)
reactants are favored
d)
equilibrium has been reached
32.
The equilibrium constant, Keq, and the rate constant, k, depend on changes in
a)
concentration
b)
pressure
c)
temperature
d)
concentration, pressure, & temperature
33.
Single step reactions & the rate determining step of multi-step reactions cannot use coefficients as exponents.
a)
True
b)
False
34.
A substance whose water solution is a poor conduction of electricity is a(n)
a)
polar substance
b)
nonelectrolyte
c)
electrolyte
d)
ionic substance
35.
In a chemical equilibrium problem, the coefficients are used as the exponents.
a)
True
b)
False
36.
When pressure increases, to return to equilibrium the reaction shifts
a)
towards the side with more moles of gas
b)
towards the side with less moles of gas
c)
towards the side with a higher temperature
d)
towards the side with a lower temperature
37.
Colloids...
a)
can be separated by filtering
b)
settle out when allowed to stand
c)
scatter light
d)
contain particles larger than 1000 mm
38.
Which of the following expresses concentration
a)
molality
b)
molarity
c)
moles of solute per liter of solution
d)
all three express concentration
39.
If less solute is dissolved than the maximum amount the solution can hold, the solution is
a)
saturated
b)
unsaturated
c)
supersaturated
d)
concentrated
40.
A species that can react as either an acid or base is a(n)
a)
Lewis acid
b)
oxyacid
c)
salt
d)
amphoteric substance
41.
Phenolphthalein is clear in a base.
a)
True
b)
False
42.
Whose acid base definitions is the most encompassing?
a)
Arrhenius
b)
Lewis
c)
Bronsted-Lowry
d)
Arrhenius & Lewis
43.
Larger particles diffuse faster than smaller particles
a)
True
b)
False
44.
The difference in pH between a pH of 12 and apt of 14 is
a)
10x
b)
100x
c)
1000x
d)
10,000x
45.
The relationship between temperature & pressure is direct, therefore the graph would be a straight line.
a)
True
b)
False
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