Final Exam Review
Units 5-8
Warm Up
• Go to the blog
• Click on the Day 2 WARM UP Questions
• While you are waiting to begin, review your
stations from yesterday.
Station 1 (Moles Unit 5)
• Complete the below Mole Map:
Volume
Mole
Particles
Mass
Station 1 (Moles Unit 5)
• Complete the below Mole Map:
Volume
Mole
Particles
Mass
Station 1 (Moles Unit 5)
Convert 4.5 g CO2 to
molecules.
a)
b)
c)
d)
6.2x1020 molecules
6.2x1022 molecules
1.2x10-25 molecules
1.2x1025 molecules
Calculate the mass of 4.3L
of oxygen gas.
a)
b)
c)
d)
e)
3.1 grams
6.1 grams
31 g rams
61 grams
138 grams
Station 1 (Moles Unit 5)
Convert 4.5 g CO2 to
molecules.
a)
b)
c)
d)
6.2x1020 molecules
6.2x1022 molecules
1.2x10-25 molecules
1.2x1025 molecules
Calculate the mass of 4.3L
of oxygen gas.
a)
b)
c)
d)
e)
3.1 grams
6.1 grams
31 g rams
61 grams
138 grams
Station 2 (Moles Unit 5)
1. Define molecular formula.
2. Define empirical formula.
3. How do you find empirical formula given the
percent composition? (remember the rhyme)
4. Once you have empirical formula how do you
find molecular formula? What other
information do you need?
Station 2 (Moles Unit 5)
1. The actual formula of the compound
2. The formula of the compound with reduced
subscripts. Its based on the percent
composition.
3. % to grams; gram to mole; divide by smallest;
multiply till whole
4. Find the molar mass of the empirical formula
and compare it to the given molar mass of the
compound (this is the additional information
you need). If different, multiply subscripts by
their quotient.
Station 2 (Moles Unit 5)
A compound consisting of C,
H, and O is found to contain
40.00% C and 6.71% H.
Determine the empirical
formula of the compound.
a)
b)
c)
d)
e)
CH2O
CHO
C2H4O2
C6H12O6
CH2
The molecular mass of the
compound to the left is
calculated to be 180.0
g/mol. Determine the
molecular formula of the
compound.
a)
b)
c)
d)
e)
CH2O
C3H6O3
C2H4O2
C6H12O6
C18H36O18
Station 2 (Moles Unit 5)
A compound consisting of C,
H, and O is found to contain
40.00% C and 6.71% H.
Determine the empirical
formula of the compound.
a)
b)
c)
d)
e)
CH2O
CHO
C2H4O2
C6H12O6
CH2
The molecular mass of the
compound to the left is
calculated to be 180.0
g/mol. Determine the
molecular formula of the
compound.
a)
b)
c)
d)
e)
CH2O
C3H6O3
C2H4O2
C6H12O6
C18H36O18
Station 3 (Stoichiometry Unit 6)
1. What conversion factor do you use to convert
between moles of different elements within
a given reaction?
2. What do you need to make sure is done
before you use the above factor?
3. How do you determine the limiting reactant?
Station 3 (Stoichiometry Unit 6)
1. Mole ratio
2. Balanced equation
3. Solve the stoichiometry problem to find the
mass of the product for each given reactant.
The number that gives you the smallest
answer is the limiting reactant.
Station 3 (Stoichiometry Unit 6)
P4 + 5O2  P4O10
Determine the mass of
tetraphosphorus
decoxide formed if 25.0
g of phosphorus (P4)
and 50.0 g of oxygen
gas are combined.
a)
b)
c)
d)
e)
57.3 grams of P4O10
88.7 grams of P4O10
146 grams of P4O10
25.0 grams of P4O10
50.0 grams of P4O10
Which reactant is limiting
in the example to the left?
a)
b)
c)
d)
25.0 g of P4
50.0g of O2
57.3 g of P4O10
88.7 grams of P4O10
Station 3 (Stoichiometry Unit 6)
P4 + 5O2  P4O10
Determine the mass of
tetraphosphorus
decoxide formed if 25.0
g of phosphorus (P4)
and 50.0 g of oxygen
gas are combined.
a)
b)
c)
d)
e)
57.3 grams of P4O10
88.7 grams of P4O10
146 grams of P4O10
25.0 grams of P4O10
50.0 grams of P4O10
Which reactant is limiting
in the example to the left?
a)
b)
c)
d)
25.0 g of P4
50.0g of O2
57.3 g of P4O10
88.7 grams of P4O10
Station 4 (Heat Unit 7)
1. What is the equation that relates heat to
change in temperature?
2. Define endothermic
3. Define exothermic
Station 4 (Heat Unit 7)
1. Q=mcΔT
2. Endothermic requires heat to be added to
proceed
3. Exothermic releases heat
Station 4 (Heat Unit 7)
• Which of the following
is an endothermic
phase change?
a)
b)
c)
d)
Sublimation
Freezing
Condensation
None of these
• Which of the following
is an exothermic phase
change?
a)
b)
c)
d)
Evaporation
Melting
Deposition
None of these
Station 4 (Heat Unit 7)
• Which of the following
is an endothermic
phase change?
a)
b)
c)
d)
Sublimation
Freezing
Condensation
None of these
• Which of the following
is an exothermic phase
change?
a)
b)
c)
d)
Evaporation
Melting
Deposition
None of these
Station 4 (Heat Unit 7)
How much heat does a 3.0
grams of water absorb as
its temperature increases
from 0C to 5.0C?
a)
b)
c)
d)
88.54 J
3.59 J
20.92 J
62.76 J
A 25 g sample of water is
absorbs 942 J as it is
heated. If the initial
temperature of the water
was 23.5oC, what is the
final temp?
a. 9.01 oC
b. 32.51 oC
c. 157.7 oC
d. 134.15 oC
cice=2.1 J/goC, cwater=4.184 J/goC, csteam=1.7 J/goC
Station 4 (Heat Unit 7)
How much heat does a 3.0
grams of water absorb as
its temperature increases
from 0C to 5.0C?
a)
b)
c)
d)
88.54 J
3.59 J
20.92 J
62.76 J
A 25 g sample of water is
absorbs 942 J as it is
heated. If the initial
temperature of the
ethanol was 23.5oC, what
is the final temp?
a. 9.01 oC
b. 32.51 oC
c. 157.7 oC
d. 134.15 oC
cice=2.1 J/goC, cwater=4.184 J/goC, csteam=1.7 J/goC
Station 5 (Solutions Unit 8)
1. What factors affect the rate of solvation (ie.
the rate at which a solvent dissolves)?
2. Define molarity. What are its units?
3. Define molality. What are its units?
Station 5 (Solutions Unit 8)
1. Agitation (stirring), increasing temperature
(heating), increasing surface area (crushing),
all increase the rate of solvation.
𝑚𝑜𝑙 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
.
𝐿 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
It has units of
𝑚𝑜𝑙 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒
.
𝑘𝑔 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡
It has units of
2. 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 =
mol/L or M.
3. 𝑀𝑜𝑙𝑎𝑙𝑖𝑡𝑦 =
mol/kg or m.
Station 5 (Solutions Unit 8)
What is the volume of
solution if the molarity is
0.45M and 0.15 moles of
solute are dissolved?
a)
b)
c)
d)
e)
0.33 L of solution
0.33 mL of solution
3.00 L of solution
3.00 mL of solution
None of these
Calculate the molarity of a
solution if 1500 g of H2SO4
is dissolve in 5.0L of water.
a.
b.
c.
d.
300 M
0.3 M
3.06 M
0.003 M
Station 5 (Solutions Unit 8)
What is the volume of
solution if the molarity is
0.45M and 0.15 moles of
solute are dissolved?
a)
b)
c)
d)
e)
0.33 L of solution
0.33 mL of solution
3.00 L of solution
3.00 mL of solution
None of these
Calculate the molarity of a
solution if 1500 g of H2SO4
is dissolve in 5.0L of water.
a.
b.
c.
d.
300 M
0.3 M
3.06 M
0.003 M
Station 5 (Solutions Unit 8)
What is the mass of NaOH
needed to prepare a
3500mL solution of
0.66 M NaOH?
a.
b.
c.
d.
2310 g
92.4 g
0.0924 g
2.31 g
What is the volume of a
0.56M solution containing
and 80 grams of NaOH?
a.
b.
c.
d.
3.57 L
35.7mL
142.8 L
14.3 L
Station 5 (Solutions Unit 8)
What is the mass of NaOH
needed to prepare a
3500mL solution of
0.66 M NaOH?
a.
b.
c.
d.
2310 g
92.4 g
0.0924 g
2.31 g
What is the volume of a
0.56M solution containing
and 80 grams of NaOH?
a.
b.
c.
d.
3.57 L
35.7mL
142.8 L
14.3 L
Station 6 (Acid/Base Unit 8)
1. What is the Arrhenius definition of an acid?
2. What is the Arrhenius definition of a base?
3. What is the Bronstead-Lowry definition of an
acid?
4. What is the Bronstead-Lowry definition of a
base?
Station 6 (Acid/Base Unit 8)
1.
2.
3.
4.
Produces H+ ion
Produces OH- ion
H+ ion donor
H+ ion acceptor
Station 6 (Acid/Base Unit 8)
According to the
Arrhenius theory a
substance that releases a
hydrogen ion is classified
as a(n)
a)
b)
c)
d)
Acid
Base
Conjugate Acid
Conjugate Base
Consider the reaction:
NH3(aq) + H2O(l)  NH4+(aq) + OH-(aq)
What species is the
conjugate acid?
a)
b)
c)
d)
NH3
H2O
NH4+
OH-
Station 6 (Acid/Base Unit 8)
According to the
Arrhenius theory a
substance that releases a
hydrogen ion is classified
as a(n)
a)
b)
c)
d)
Acid
Base
Conjugate Acid
Conjugate Base
Consider the reaction:
NH3(aq) + H2O(l)  NH4+(aq) + OH-(aq)
What species is the
conjugate acid?
a)
b)
c)
d)
NH3
H2O
NH4+
OH-
Station 7 (Acid/Base Unit 8)
• What is the pH range for an acid? Base?
• Complete the following map:
[H+]
pH
[OH-]
pOH
Station 7 (Acid/Base Unit 8)
• What is the pH range for an acid? Base?
• Complete the following map:
[H+]
pH
[OH-]
pOH
Station 7 (Acid/Base Unit 8)
If the [H+] is equal to
9.2 x 10 -4 M, it’s a(n)
_________
a) Acid
b) Base
c) Neutral solution
Calculate the [OH-] for a
solution that has [H+] is
equal to 2.0 x 10 -8 M
a.
b.
c.
d.
5.0 x 10-1 M
5.0 x 10-7 M
1.0 x10-7 M
2.0 x 10-7 M
Station 7 (Acid/Base Unit 8)
If the [H+] is equal to
9.2 x 10 -4 M, it’s a(n)
_________
a) Acid
b) Base
c) Neutral solution
Calculate the [OH-] for a
solution that has [H+] is
equal to 2.0 x 10 -8 M
a.
b.
c.
d.
5.0 x 10-1 M
5.0 x 10-7 M
1.0 x10-7 M
2.0 x 10-7 M