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WorksheetsAP Comprehensive Assessment
Total questions: 106
Worksheet time: 53mins
Name
Class
Date
1.
What is the formula for molarity?
a)
moles of solute
b)
liters of solution
c)
liters of solution per moles of solute
d)
moles of solute per liters of solution
2.
When heat is added more to a chemical system than released during a chemical change, we say what has occurred?
a)
endothermic change
b)
exothermic change
c)
heat is equally flowing into and out of a chemical system
d)
none of the above
3.
Methane is:
a)
CH4
b)
CH3
c)
C2H6
d)
CO2
4.
Another name for methane would ge:
a)
carbon dioxide
b)
carbon hydride
c)
mono-carbon tetra-hydride
d)
carbon tetra-hydride
5.
What is the formula for tri-carbon octa-hydride?
a)
C3H6
b)
C3H8
c)
C3H10
d)
C8H3
6.
What is the organic name for C4H10?
a)
methane
b)
ethane
c)
propane
d)
butane
7.
Combustion of a hydrocarbon fuel results in:
a)
heat given off
b)
carbon dioxide released
c)
water released
d)
all of the other answers are correct
8.
Water is:
a)
polar
b)
non-polar
c)
an ionic compound
9.
Water is the universal _________________.
a)
solute
b)
solvent
c)
solution
10.
Where generally on the Periodic Table are the metals?
a)
left side
b)
left side not including hydrogen
c)
right side
d)
right side not including the last vertical column
11.
If I wanted to make an aqueous mixture more dilute, I would:
a)
add water
b)
boil off water
c)
add solute
d)
heat the solution
12.
Burning two moles of C3H8 will make how many carbon dioxide moles?
a)
1
b)
6
c)
8
d)
10
13.
The amount of energy needed to go from the reactants to the "activated complex" or "transition state" is called:
a)
endothermic energy
b)
overall enthalpy change
c)
thermal activity
d)
activation energy
14.
In a chemical sample undergoing a chemical change, typically all of the particles are moving fast enough and colliding just right for the reactants to completely change to products.
a)
true
b)
false
15.
if 2 moles of tri-carbon octa-hydride were burned in oxygen, how many water molecules would you make?
a)
2
b)
4
c)
6
d)
8
16.
meth-, eth-, _________, but-, __________, ________, hept-, __________, non-, dec-:
are all of the first 10 organic prefixes in alkanes, alkenes, and alkynes.
are all of the first 10 organic prefixes in alkanes, alkenes, and alkynes.
a)
oct-, pent-, hex-, prop-
b)
hex-, oct-, pent-, prop-
c)
prop-, hex-, pent-, oct-
d)
prop-, pent-, hex-, oct-
17.
When 2 moles of butane is burned in the presence of oxygen, how much carbon dioxide would you expect?
a)
2 moles
b)
6 moles
c)
8 moles
d)
1 mole
18.
When 2 moles of C4H10 are burned in oxygen, how many moles of water would you expect to be produced?
a)
1
b)
4
c)
8
d)
10
19.
Which of the following statements is true?
a)
transition states can be isolated
b)
intermediates can never be isolated
c)
enzymes are not used up in the chemical reaction
d)
enthalpy is the same as free energy
20.
enthalpy is:
a)
stored energy
b)
motion energy
c)
free energy
d)
internal energy
21.
entropy is:
a)
internal energy
b)
temperature
c)
disorder
d)
enthalpy
22.
the first law of thermodynamics states that energy
a)
is always getting bigger
b)
is always used to make a chemical system more disordered
c)
is never created nor destroyed
d)
is infinite is amount
23.
The natural order of the universe is to always be getting:
a)
more stored energy
b)
more enthalpy
c)
more entropy
d)
more order to chemicals
24.
When 2 moles of hydrogen combine chemically with 1 mole of oxygen, then we expect to get how much water?
a)
1 mole
b)
2 moles
c)
3 moles
d)
4 moles
25.
When the forward rate of a chemical reaction equals the reverse rate of a chemical reaction, we would call this:
a)
static
b)
blananced
c)
spontaneous
d)
at equilibrium
26.
What factors affect kinetics:
a)
concentration of reactants
b)
temperature
c)
presence of a catalyst
d)
all of the above
27.
Kinetics would measure the rate of:
a)
the disappearance of reactant
b)
the appearance of product
c)
temperature change
d)
two of the other answers are correct
28.
For chemical reactants to "actually react," they must:
a)
be in the correct orientation
b)
have received enough activation energy
c)
go through breaking bonds and remaking other bonds
d)
all of the above
29.
How many liters would you need to make 1.00 Molar solution, if you have 6.00 moles of sodium hydroxide Na(OH) (aq)?
a)
2
b)
3
c)
4
d)
6
30.
How many grams would you need of H(+) to make 2 Molar solution in 3 Liters of water? Again, H(+) is about 1 gram/mole.
a)
6
b)
3
c)
2
d)
1
31.
What is the molarity of 3 moles of HCl in 3 Liters of solution?
a)
1 M
b)
2 M
c)
3 M
d)
.5 M
32.
What is the molarity of 650. mL containing 63.0 grams of NaCl?
a)
2.40 M
b)
.860 M
c)
1.70 M
d)
.540 M
33.
Which sweet tea would you expect to be the sweetest from the following concentrations re: sugar solute in the tea?
a)
1.0 M
b)
2.0 M
c)
3.0 M
d)
5.0 M
34.
The higher the concentration of solution, the less amount of solute it has in it?
a)
true
b)
false
35.
What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution?
a)
.488 M
b)
7.67 moles
c)
7.67 M
d)
.00767 M
36.
Which of the following options has the most NaCl in it? Keep in mind: 58.44 grams = 1.0 mole.
a)
100. mL of 1.8 M solution
b)
50.0 mL of 4.1 M solution
c)
9.35 grams
d)
1.0 moles
37.
How many grams are in 7.80 grams of NaCl?
a)
452 g
b)
460 g
c)
462 g
d)
476 g
38.
What is the molar mass of glucose: C6H12O6?
a)
180.18 g/ mol
b)
180.12 g/mol
c)
180.24 g/mol
d)
180.06 g/mol
39.
N2 + 3H2 --> 2NH3
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
1
b)
2
c)
3
d)
6
40.
What are the first things you do when solving stoichiometry problems?
a)
balance the equation and Identify the known and unknown quantities
b)
panic
c)
write the unbalanced equation
d)
take a nap
41.
How many grams are in 1.0 moles of diatomic oxygen?
a)
16
b)
32
c)
6.02 x 1023
d)
1.0 mole
42.
What is the molar mass in g/mol of CH4 to four significant digits?
a)
16.04
b)
16.05
c)
16.07
d)
16.08
43.
Mole ratio is the ratio of:
a)
the asked for substance formula over the given's substance formula
b)
the given's substance formula over the asked for's substance formula
c)
the molar mass of the given's substance formula
d)
a ratio of the dark side to the force
44.
In the ideal gas law equation: PV=nRT, the R is a:
a)
ratio
b)
radius
c)
reaction rate constant
d)
gas constant
45.
Pressure is the force of:
a)
inhibition
b)
catalyst action
c)
collision of particles
d)
average kinetic energy
46.
temperature is:
a)
absolute motion energy
b)
average force of collision
c)
average kinetic energy
d)
measured in atm
47.
pressure x volume can be thought of as:
a)
pressure
b)
reaction rate
c)
disorder
d)
energy
48.
nRT can be thought of as:
a)
pressure
b)
reaction rate
c)
disorder
d)
energy
49.
Heat flows:
a)
from cold to hot
b)
from lower average kinetic energy to higher
c)
from hot to cold
d)
from low to high pressure
50.
What is the name for SiO2?
a)
silica oxide
b)
silicon oxide
c)
silicon di-oxide
d)
mono silicon di-oxide
51.
What main imf (intermolecular force of attraction) exists between molecules of a HCl sample?
a)
dispersion forces
b)
hydrogen bonding
c)
dipole-dipole
d)
ion-dipole
52.
What main imf exists between particles of a Cl2 sample?
a)
ion-dipole
b)
hydrogen bonding
c)
dipole-dipole
d)
dispersion forces
53.
Imf's are forces that exist:
a)
between atoms within a molecule
b)
between neighboring molecules
54.
Which is not an imf?
a)
molecular covalent bonding
b)
ion-dipole
c)
dipole-dipole
d)
hydrogen bonding
55.
What are the main imf's between water molecules?
a)
dispersion forces
b)
hydrogen bonding
c)
dipole-dipole
d)
ion-dipole
56.
What type of imf is between adjacent molecules despite their polarity?
a)
ion-dipole
b)
dipole-dipole
c)
dispersion forces
d)
hydrogen bonding
57.
What is the unit for molar mass?
a)
g
b)
g/mol
c)
moles/ liter
d)
L x atm/mol x K
58.
A--> B
If you are doing stoichiometry and converting from mass in grams of a reactant substance to mass in grams of a product substance, what will your pathway follow for conversion:
If you are doing stoichiometry and converting from mass in grams of a reactant substance to mass in grams of a product substance, what will your pathway follow for conversion:
a)
grams A--> moles A --> grams B
b)
grams A -->moles B --> grams B
c)
grams A --> grams B
d)
grams A--> moles A --> moles B --> grams B
59.
What generally increases due to stronger imf's?
a)
non-ideal gas behavior
b)
higher melting points
c)
higher boiling points
d)
all of the above
60.
An imf for 2 polar molecules near each other
a)
dispersion
b)
dipole-dipole
c)
hydrogen bonding
d)
ion-dipole
61.
An imf specifically between one molecule that has hydrogen and another that has N, O, or F?
a)
hydrogen bonding
b)
ion-dipole
c)
dipole-dipole
d)
dispersion forces
62.
Imf type existing because of temporary dipoles formed due to electron windows momentarily opening up:
a)
dispersion
b)
dipole-dipole
c)
H-bonding
d)
ion-dipole
63.
A chemical bond is made of how many electrons?
a)
1
b)
2
c)
4
d)
6
64.
Which of the following are not diatomic molecules?
a)
N2
b)
O2
c)
H2
d)
S2
65.
Increasing the concentration of reactants could:
a)
slow down the reaction
b)
speed up the reaction
c)
lower the pressure of the system
66.
If you double the concentration of one of the reactants, and the initial reaction rate also doubles, what is the reaction order?
a)
0
b)
1st
c)
2nd
67.
What is the mole ratio of water to hydrogen in the formation of water from oxygen and hydrogen?
a)
1 mol water / 1 mol hydrogen
b)
1 mol hydrogen / 1 mol water
c)
2 mol water / 2 mol hydrogen
68.
In stoichiometry what number helps you relate the amount of one chemical to the amount of another chemical?
a)
number of moles
b)
molar mass
c)
molarity
d)
mole ratio
69.
What do opposite charges do at short distances?
a)
attract
b)
repel
c)
just sit there
70.
What is the alternative quantity used in kinetics problems when (aq) is not appropriate?
a)
temperature of a gas
b)
pressure of a gas
c)
number of moles of a gas
71.
In a proposed reaction mechanism, what is the rate determining step?
a)
1st elementary reaction
b)
2nd step
c)
slow step
d)
fast step
72.
What vertical group is stable on the Periodic Table?
a)
group 1 a, the alkali metals
b)
group 2 a, the alkaline earth metals
c)
group 7 a, the halogens
d)
group 8 a, the noble gases
73.
Where does salt solute go when it dissolves in water?
a)
to the bottom of the container
b)
to the cell phone every student is using
c)
in between the solvent's particles
d)
to the top of the container
74.
What area of the Periodic Table has the strongest Coulombic Force of attraction?
a)
bottom left corner
b)
upper left corner
c)
top right corner
d)
top right corner, not including group 8a
75.
The SI unit for energy is:
a)
calorie
b)
grams/mole
c)
joule
d)
newton
76.
When speaking of bond energy, we usually measure in:
a)
calories
b)
joules
c)
kilo-joules
d)
electric potential
77.
Which state has the most motion energy and involves colliding and spreading?
a)
solid
b)
liquid
c)
gas
d)
(aq)
78.
(aq) stands for:
a)
solid
b)
liquid
c)
gas
d)
water solution
79.
What type of reaction starts at a lower energy for the reactants and ends with a higher energy of the products?
a)
endothermic
b)
exothermic
c)
dynamic
d)
eagle souring
80.
In an exothermic reaction:
a)
more bonds are made than broken
b)
more bonds are broken than made
c)
energy is taken into the system more than released from the system
81.
In an exothermic reaction, significant enthalpy of the reactants is released as:
a)
temperature
b)
pressure
c)
heat
82.
What is STP?
a)
a liquid for your car
b)
standard temperature and pressure
c)
220K
d)
2 of the other answers is correct
83.
What is standard temperature in Celsius?
a)
0 K
b)
0 C
c)
28 C
d)
298 K
84.
How do I convert from Celsius to Kelvin?
a)
add 32
b)
add 273
c)
subtract 273
85.
In a gas sample at a certain temperature, all particles are moving at the same speed?
a)
true
b)
false
86.
How are temperature and pressure related?
a)
directly proportional
b)
inversely proportional
87.
A closed system:
a)
allow matter to flow between the chemical system and the environment
b)
does not allow energy to flow between the chemical system and its environment
c)
does not allow particles to flow between the chemical system and its environment
88.
When temperature increases, what happens to the rate constant for a chemical reaction?
a)
goes up
b)
goes down
c)
stays constant
89.
When free energy is negative, the chemical reaction:
a)
stays constant in its enthalpy
b)
is spontaneous
c)
is non-spontaneous
d)
undergoes heating
90.
Roughly what is the molar mass in g/mole for
Ca (CO3)?
Ca (CO3)?
a)
28
b)
50
c)
100
d)
112
91.
Mass cannot be created nor destroyed is known as the:
a)
law of definited proportions
b)
newton's 3rd aw
c)
law of definite proportions
d)
law of conservation of mass
92.
What is the most electronegative (hungry for electrons) element on the Periodic Table?
a)
H
b)
N
c)
O
d)
F
93.
What is the systematic name for PCl3?
a)
phosphorus chloride
b)
tri-phosphorus mono-chloride
c)
phosphorchloride
d)
phosphorus tri-chloride
94.
Delta G=?
a)
delta H
b)
temperature x delta S
c)
delta H + T x delta S
d)
delta H - T x delta S
95.
0 degrees Celsius is the temperature of:
a)
liquid water freezing
b)
boiling point of water
c)
melting point of ice
d)
liquid water freezing and the melting point of ice
96.
At what temperatures and pressures can the effect of intermolecular forces be minimized?
a)
high T, low P
b)
high P, low T
c)
low T, low P
d)
low T, low P
97.
What does the decimal number on the Periodic Table represent when doing stoichiometry?
a)
atomic number
b)
size
c)
mole ratio
d)
molar mass
98.
When doing stoichiometry, what is the conversion factor you multiply by when converting from grams of a substance to moles of that same substance?
a)
g/mol
b)
mole ratio
c)
mol/g
d)
none of the above
99.
When dissolving a substance into a solvent, what must be higher in value and more stable physical blend?
a)
imf's between the solute particles
b)
imf's between the solvent particles
c)
imf's between the solute and solvent particles
100.
Other than concentration, what affects chemical behavior significantly and more than the others?
a)
pressure
b)
temperature
101.
In our steel wool demonstration, what happens to the mass of the solid undergoing oxidation and combustion?
a)
it increases
b)
it decreases
c)
it remains constant
102.
In our "layering of solutions" lab, what imf results from us adding NaCl and keeps the yellow and blue blend non-uniform, and how can we prevent the layering and return all the polar substances to a uniform green color?
a)
hydrogen bonding; heating it up
b)
ion-dipole; heating it up
c)
dipole-dipole; heating it up
d)
dispersion forces; cooling it down
103.
What tool is most accurate for measuring the volume of a liquid?
a)
beaker
b)
flask
c)
test tube
d)
graduated cylinder
104.
How many sig figs are in: .0120 g
a)
1
b)
2
c)
3
d)
4
105.
12.011 g/mol of carbon x 2.00 moles = ? g
a)
24.022 g
b)
24.02 g
c)
24.0 g
d)
24 g
106.
The slope of a kinetics curve would look like what if it were to show Time (s) vs Reactant M/s?
a)
positive in slope
b)
horizontal in slope
c)
negative in slope
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