Name___________________________________
Period _______
Spring Final Review
MOLES
1. The gram formula mass of Al2O3 is 101.961
g/mol. What is the mass of 6.02 x 1023
molecules of Al2O3?
101.961 g Al2O3
2. How many molecules are in 9.45 mol of sodium
nitrate, NaNO3?
9.45 𝑚𝑜𝑙 𝑁𝑎𝑁𝑂3 𝑥
6.02𝑥1023 𝑁𝑎𝑁𝑂3
1𝑚𝑜𝑙 𝑁𝑎𝑁𝑂3
24
= 5.69𝑥10 𝑁𝑎𝑁𝑂3
3. How many grams are in 1.58 mol of potassium
nitride, K3N?
1.58 𝑚𝑜𝑙 𝐾3 𝑁 𝑥
131.3 𝑔 𝐾3 𝑁
= 207 𝑔 𝐾3 𝑁
1 𝑚𝑜𝑙 𝐾3 𝑁
4. How many molecules are in 3.47 g of MgCl2?
3.47 𝑔 𝑀𝑔𝐶𝑙2 𝑥
1 𝑚𝑜𝑙 𝑀𝑔𝐶𝑙2 6.02𝑥1023 𝑀𝑔𝐶𝑙2
𝑥
95.21 𝑔 𝑀𝑔𝐶𝑙2
1 𝑚𝑜𝑙 𝑀𝑔𝐶𝑙2
= 2.19𝑥1022 𝑀𝑔𝐶𝑙2
5.
Nicotine is 74.1% carbon, 8.6% hydrogen, and
17.3% nitrogen by mass. What is its empirical
formula?
“Percent by mass, gets to mole, divide by
smallest, multiply ‘til whole”
C5H7N
6. Analysis of a compound gave 26.2% N, 7.5%
H, 66.4% Cl. It’s molecular mass is 160 g/mol.
a. What is its empirical formula?
NH4Cl
STOICHIOMETRY
1. Copper(II)Oxide decomposes to form solid
copper and oxygen gas. If 95.4 g of copper(II)
oxide decomposes, how many grams of oxygen
are formed?
2 CuO 2 Cu + O2
95.4 𝑔 𝐶𝑢𝑂 1 𝑚𝑜𝑙 𝐶𝑢𝑂 1 𝑚𝑜𝑙 𝑂2 32.0 𝑔 𝑂2
𝑥
𝑥
𝑥
1
79.6 𝑔 𝐶𝑢𝑂 2 𝑚𝑜𝑙 𝐶𝑢𝑂 1 𝑚𝑜𝑙 𝑂2
= 19.2 g O2
2. Potassium hydroxide reacts with sulfuric acid in
a double replacement reaction. What is the
mass of water if 19.6 g of KOH reacts with
excess acid?
2 KOH + H2SO4  H2O + K2SO4
19.6 𝑔 𝐾𝑂𝐻 1 𝑚𝑜𝑙 𝐾𝑂𝐻 1 𝑚𝑜𝑙 𝐻2𝑂 18.0 𝑔 𝐻2𝑂
𝑥
𝑥
𝑥
1
56.1 𝑔 𝐾𝑂𝐻 2 𝑚𝑜𝑙 𝐾𝑂𝐻 1 𝑚𝑜𝑙 𝐻2𝑂
=3.14 g H2O
3. If 36.5 g of HCl and 73.0 g of Zn are put
together, and the reaction proceeds as follows:
2 HCl + Zn  ZnCl2 + H2
a. Find the limiting reactant.
36.5 𝑔 𝐻𝐶𝑙 1 𝑚𝑜𝑙 𝐻𝐶𝑙 1 𝑚𝑜𝑙 𝑍𝑛𝐶𝑙2 136.4 𝑔 𝑍𝑛𝐶𝑙2
𝑥
𝑥
𝑥
1
36.5 𝑔 𝐻𝐶𝑙 2 𝑚𝑜𝑙 𝐻𝐶𝑙
1 𝑚𝑜𝑙 𝑍𝑛𝐶𝑙2
73.0 𝑔 𝑍𝑛 1 𝑚𝑜𝑙 𝑍𝑛 1 𝑚𝑜𝑙 𝑍𝑛𝐶𝑙2 136.4 𝑔 𝑍𝑛𝐶𝑙2
𝑥
𝑥
𝑥
1
65.4 𝑔 𝑍𝑛
1 𝑚𝑜𝑙 𝑍𝑛
1 𝑚𝑜𝑙 𝑍𝑛𝐶𝑙2
36.5 g HCl is the limiting reactant
(produces less ZnCl2)
b. Find the mass of ZnCl2 formed.
36.5 g HCl produces 68.2 g ZnCl2
73.0 g Zn produces 152 g ZnCl2
b. What is its molecular formula?
160
53.45
=3
N3H12Cl3
7. What is the percentage composition of silver in
silver nitrate (AgNO3?)
107.87
𝑥100
169.87
= 63.5 % Ag
c. If only 80 g of ZnCl2 is formed find the %
yield. (Actual yield / theoretical yield ) x 100
(80 g / 68.2 g ) x 100 = 117%
Name___________________________________
Period _______
THERMOCHEMISTRY
1. If you burn a 30.0 g Cheeto in a bomb
calorimeter containing 500 g of water (Cp =
4.18 J/g°C), and the temperature increases by
30 degrees Celsius, how many joules of
energy are in the chips?
Q = (500g)(30°C)(4.18 J/g°C )= 62700 J
2. What is the molarity of NaOH in which 19.2 g of
solute is dissolved in 160 ml of solution?
19.2 𝑔 𝑁𝑎𝑂𝐻 1 𝑚𝑜𝑙 𝑁𝑎𝑂𝐻
𝑥
= .48 𝑚𝑜𝑙
1
40.0 𝑔 𝑁𝑎𝑂𝐻
2. The temperature of an 8.0 g sample of metal
changed from 250 to 500 C when it absorbed
420J of heat. What is the specific heat of this
sample?
𝑄
420 𝐽
Cp = 𝑚∆𝑇 = (8.0 𝑔)(25°C) = 2.1 J/g°C
3. How many grams of NaCl would be required to
make 300 ml of a 0.5 M solution of NaCl?
𝑚𝑜𝑙
𝑀= 𝐿
𝑚𝑜𝑙 = 𝑀𝑥𝐿 = 0.5 𝑀 𝑥 0.300 𝐿 = .15 𝑚𝑜𝑙
0.15 𝑚𝑜𝑙 58.8 𝑔 𝑁𝑎𝐶𝑙
𝑥
= 8.85 𝑔 𝑁𝑎𝐶𝑙
1
1 𝑚𝑜𝑙 𝑁𝑎𝐶𝑙
3. True of False
a. __F__Heat moves from a colder object to a
warmer one.
b. __T___∆H refers to a reaction while ∆Hf°
refers to a compound
c. __F___If the heat involved in a chemical
reaction has a negative sign, heat is lost to
the surroundings and the reaction is
endothermic
d. __F___A process that absorbs heat is an
exothermic process.
e. __T___ΔH is zero for a free element (O2,
Na, etc.)
4. Label the following reactions as either
endothermic or exothermic.
a. __Exo____ 2 H2 + O2  2 H2O + energy
b. __Endo____ CO2 + H2O + energy  CH2O
+ O2
c. ___Exo____ CH4 + 2 O2  CO2 + 2 H2O
+energy
5. A hot metal cube is placed into cool water.
Explain what happens to the temperature of the
water and the metal cube?
Heat is lost from the metal cube and gained by the
water. The temperature of the metal cube
decreases as the water temperature increases.
SOLUTIONS
1. What is the molarity of nitric acid in which 6.3 g
of HNO3 is dissolved in 500 ml of solution?
6.3𝑔 𝐻𝑁𝑂3
1 𝑚𝑜𝑙
𝑥
= 0.1 𝑚𝑜𝑙 𝐻𝑁𝑂3
1
63𝑔 𝐻𝑁𝑂3
0.1 𝑚𝑜𝑙 𝐻𝑁𝑂3
= 0.2 𝑀
. 500 𝐿
. 48 𝑚𝑜𝑙
= 3𝑀
. 160 𝐿
4. How many mL of 3.0 M HCl would be needed to
make 2000 ml of 0.5 M HCl?
𝑉1 𝑀1 = 𝑉2 𝑀2
𝑉2 𝑀2
𝑉1 =
𝑀1
(2000 𝑚𝐿) (0.5 𝑀)
𝑉1 =
3.0 𝑀
𝑉1 = 333 𝑚𝐿
5. A lab procedure calls for 3.2L of solution. This
solution is made by adding water to 0.0500 L of
16 M H2SO4. What concentration do you end
up with by doing this?
𝑉1 𝑀1 = 𝑉2 𝑀2
𝑉1 𝑀1
𝑀2 =
𝑉2
(0.0500 𝐿)(16 𝑀)
𝑀2 = (
= 0.25 𝑀
3.2 𝐿
6. How much 1.43 M HCl will be needed to make
1.5 L of 1.2 M HCl?
𝑉1 𝑀1 = 𝑉2 𝑀2
𝑉2 𝑀2
𝑉1 =
𝑀1
(1.5 𝐿)(1.2𝑀)
𝑉1 =
= 1.26 L
1.43 𝑀
7. Which of the following is soluble (Only one is
correct)?
a. Na2CrO4
b. AgBr
c. HgSO4
d. AlPO4
8. You mix Mg(NO3)2 and Na2CO3. Will you get a
precipitate? If so, what is the formula?
a. No.
Name___________________________________
b. Yes, NO3CO3
c. Yes, MgCO3
9. Which of the following reactions will produce a
precipitate? (only one is correct):
a. Ca(OH)2+NaClCaCl2 + NaOH
Period _______
15. At what temperature can NH3 and KNO3 dissolve
the same amount of solute?
a. 43°C
b. 28°C
c. 8°C
d. 24°C
b. AlBr3 + AgClO  AgBr + Al(ClO)3
c. MgBr2 + Al(NO3)3  AlBr3 + Mg(NO3)2
10. All of these can increase the rate at which a
solid dissolves in water except —
a. using smaller crystals of the solid
b. stirring the water
c. increasing the temperature of the water
d. using larger crystals of the solid
11. Which set of conditions would increase the
solubility of salt (solid) in water?
a. Low temperature, small particle size
b. Low temperature, large particle size
c. High temperature, small particle size
d. High temperature, large particle size
12. True or False: Correct the statement if it is
false.
a. ___F__Water is nonpolar.
b. ___T___Water is able to dissolve ionic
compounds due to its slight positive and
negative charges.
c. __F____Water is universal compound
solvent.
d. ___F___Water molecules have strong forces
of interaction due to oxygen hydrogen
bonding.
13. Mr. Philpott prepares an unsaturated solution
of sodium nitrate. This means –
a. That no more sodium nitrate can be
added to the solution
b. That more sodium nitrate can be
added to the solution
c. That there is more than the
maximum amount of sodium nitrate
in the solution.
d. None of the above
14. What happens to a light bulb connected to an
aqueous solution when you have a strong
electrolyte? Weak electrolyte? Nonelectrolyte?
Strong: Bright
Weak: Dim
Non: Off
ACIDS AND BASES
1. Identify the parts of the neutralization reaction
(acid, base, salt, and water):
a. Mg(OH)2 + H2SO4
Base
Acid
b. H3PO4 + NaOH
Acid
 MgSO4 + H2O
Base
Salt
Water
 Na3PO4 + H2O
Salt
Water
2. A solution with a pH of 4 is how many more
times acidic than a solution with a pH of 7?
7-4= 3
103 = 10 x 10 x 10 = 1000
3. A solution with a pH of 14 is how many more
times basic than a solution with a pH of 13?
14-13 = 101 = 10
4. True or False?
_T__Strong acids almost completely dissociate
in water while weak acids partially dissociate in
water.
_F__Strong acids partially dissociate in water
while weak acids almost completely dissociate
in water.
Name___________________________________
_F__Weak acids always have a lower pH than
strong acids.
__F_Strong acids produce hydroxide ions in
solution and weak acids produce hydrogen ions
in solution.
5. What are the pH and pOH of a solution with a
[H+] of 3.64 x 10-7?
pH = -log(H+]
pH = -log(3.64x10-7) = 6.43 = pH
pOH = 14 – pH = 14 - 6.43 = 7.57
6. What is the pOH of a solution in which 0.26
moles of sodium hydroxide (NaOH) was
dissolved in .457 L of water.
𝑀=
0.26 𝑚𝑜𝑙
.457 𝐿
= 0.568 = [𝑂𝐻 − ]
pOH = -log (OH-) = - log(.568) = 0.246
7. Complete the tables below
Acids, Bases,
or Both
Property
Donates protons (H+)
Causes blue litmus paper to
turn red
Electrolytes
Sour taste
Causes red litmus paper to turn
blue
Bitter taste
[ H+] = 1.0 x 10-2
Electron donor
Acid
Acid
Both
Acid
Base
Base
Acid
(Pre-AP only)
Base
Period _______
GAS LAWS
1. True / False
a. __T__ According to the kinetic-molecular
theory, particles of matter are in continual
motion
b. __F__ According to the kinetic-molecular
theory, matter is composed of very large
particles
c. __F__ According to the kinetic-molecular
theory, the total energy of colliding particles
is changing all the time.
2. You are stuck in a room with two horrible
smelling gases. One is a bad smell from a cat’s
litter box due to ammonia, NH3, with a
molecular weight of 17g/mol and the other is
an inexpensive French perfume with a
molecular weight of 170 g/mol. Which gas
molecules will reach your nose first?
a) ammonia
b) inexpensive perfume
c) both
+
[H ]
[OH-]
pH
Acid, Base or
Neutral?
1.00 x
1.00x10
4
Acid
10
10-4
7
1x10-7
1x10-7
Neutral
3. How can you slow down the time it takes the
molecules of ammonia and inexpensive
perfume to reach your nose?
a) increase the temperature of the room
b) decrease the temperature of the room
c) it doesn’t matter
4. 257 mL of oxygen in a gas tube goes from 17°C
to 42°C from being out in the sun. The
pressure in the tube increases from 3.6 atm to
4.5 atm. What is the new volume of the tube?
(3.6)(257)(315)
V2 = (290)(4.5) = 223.32 mL = 220 mL
5. A .450 L sample of fluorine gas is at 27˚C and
216 kPa. How many moles of fluorine gas is
this?
(216)(.450)
n = (8.314)(300) = 0.039 mol
Equations and Conversion Factors
𝟔. 𝟎𝟐 𝒙 𝟏𝟎𝟐𝟑 𝒎𝒐𝒍𝒆𝒄𝒖𝒍𝒆𝒔
𝟏 𝒎𝒐𝒍
pH = -log[H+]
pOH = -log[OH-]
pH + pOH = 14