Name _________________________________________________ Date _______________________ Period ________
Final Review
This packet is a general overview of the main topics covered in the second semester of Academic Chemistry. All of the class material is NOT
included and students are strongly encouraged to study notes and review previous assignments.
Stoichiometry
1. Hydrogen peroxide is used to clean lead (II) sulfide from oil paintings.
PbS(s) + 4H2O2(aq) → PbSO4(s) + 4H2O(l)
a. How many grams of H2O2 must be used to clean off 0.24 g of PbS?
b. If 0.072 g of H2O form in the reaction, how many grams of PbSO4 must also have been formed?
2. Sodium hydroxide reacts with carbon dioxide according to the following balanced equation:
2NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l)
a. Which is the limiting reactant when 1.85 mol NaOH and 1.00 mol CO2 are allowed to react?
b. How many grams of sodium carbonate can be produced?
3. Ammonia gas, NH3, can be prepared by the reaction of a metal oxide such as calcium oxide with ammonium chloride.
CaO(s) + 2NH4Cl(s) → 2NH3(g) + H2O(g) + CaCl2(s)
If 112 grams of calcium oxide and 224 grams of ammonium chloride are mixed,
a. What is the limiting reactant?
b. What mass of ammonia gas can be produced?
c. If only 16.3 grams of ammonia gas is actually obtained, what is its percent yield?
4. When copper (II) chloride reacts with sodium nitrate, copper (II) nitrate and sodium chloride are formed.
a. Write the balanced equation for the reaction given above:
b. If 15.0 grams of copper (II) chloride react with 20.0 grams of sodium nitrate, how much sodium chloride can
be formed?
c. What is the limiting reactant for the reaction above?
d. If 11.3 grams of sodium chloride are formed in the reaction, what is the percent yield of this reaction?
Light & Electron Configurations
1. Know all the rules for electron configuration.
2. Write the complete electron configuration for the potassium atom.
3. Write the complete electron configuration for the antimony atom.
4. Write the noble gas (shorthand) electron configuration for the magnesium ion.
5. Write the noble gas (shorthand) electron configuration molybdenum atom.
6. Write the noble gas (shorthand) electron configuration for the lead atom.
7. Write the complete electron configuration for the thorium atom.
8. Violet light has a wavelength of 4.10 x 10-12 m. What is the frequency?
9. Green light has a frequency of 6.01 x 1014 Hz. What is the wavelength?
10. Calculate the wavelength of radiation with a frequency of 8.0 x 1014 Hz.
11. A helium laser emits light with a wavelength of 633 nm. What is the frequency of the light?
12. Calculate the energy, in Joules, of a photon of red light whose wavelength is 3.81 x 10-3 nm.
13. Determine the energy, in Joules, of a photon whose wavelength is 4.257 x 10-7 nm.
Bonding
1. For the following molecules: draw the Lewis structure. For the starred (*) molecules, identify the electron pair geometry
& molecular structure.
a. *NO3b. *SiCl4
c. *PCl3
d. SF6
e. *SO2
f. *COF2 (C is central)
g. XeF5+
Solutions
Use the diagram on the right to answer questions #1-4.
1. How much NaNO3 will dissolve in 100 mL of water at 35°C?
2. If 145 g of KI is dissolved at 10°C, will the solution
be saturated, unsaturated, of supersaturated?
3. What temperature is necessary to create a saturated solution
with 15g of KClO3 in 100 mL of water?
4. How much NH4Cl will dissolve in 200 mL of water at 90°C?
5. Predict the products for the following chemical reactions and write the balanced formula equation, complete ionic
equation and the net ionic equation on a separate piece of paper.
a. Barium Chloride(aq) + Sulfuric Acid(aq) →
b. Potassium Phosphate(aq) + Aluminum Nitrate(aq) →
6. Assume you dissolve 45.0 g of camphor, C10H16O, in 334 g of ethanol, C2H5OH. Calculate the mass percent of camphor
in this solution.
7. What is the molarity of a solution when 80.0 grams of NaOH is dissolved in 1.25 L of solution?
8. To what volume, in mL, should you dilute 100. mL of a 5.00 M CaCl2 solution to obtain a 0.750 M CaCl2 solution?
Gases
1. How many moles of gas occupy 98.0 L at a pressure of 2.80 atmospheres and a temperature of 292 K?
2. A balloon is filled with 35.0 L of helium in the morning when the temperature is 20.0°C. By noon the temperature has
risen to 45.0°C. What is the new volume of the balloon?
3. A 35 L tank of oxygen is at 315 K with an internal pressure of 190 atmospheres. How many moles of gas does the tank
contain?
4. A sample of oxygen gas has a volume of 150 mL when its pressure is 440 mmHg. If the pressure is increased to
760 mmHg, what will the new gas volume be?
5. 5.36 liters of nitrogen gas are at -25C and 733 mm Hg. What would be the volume at 128C and 1.5atm?
6. 790. mm Hg of gas is collected over water at 25°C. (Vapor pressure of water is 23.12 mm Hg at 25°C). What is the
partial pressure of the gas collected?
7. A 5.00-L air sample containing H2S at STP is treated with a catalyst to promote the reaction,
2H2S(g) + O2(g) → 2H2O(g) + 2S(s)
If 3.21 g of solid S was collected, calculate the volume of H2S in the original sample.
Thermochemistry
1. Calculate ∆Hrxn for the reaction 2Al(s) + 3Cl2(g) → 2AlCl3(s) from the following data.
2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)
∆H = -1049 kJ
HCl(g) → HCl(aq)
∆H = -74.8 kJ
H2(g) + Cl2(g) → 2HCl(g)
∆H = -1845 kJ
AlCl3(s) → AlCl3(aq)
∆H = -323 kJ
2. A 25.0 gram sample of a solid metal was heated to 100.0C and dropped into a calorimeter containing 90.0 grams of water
at 25.32C. If the final temperature of the water and the metal was 28.78C, calculate the specific heat of the metal.
Specific heat of water is 4.184 J/C•g
3. Given the data in the table below, calculate ∆H°rxn, in kJ, at 25°C:
2SO2(g) + O2(g) → 2SO3(g)
Substance
ΔHf° (kJ/mol)
SO2
-297
O2
0
SO3
-395
Use the information below to answer 4-5.
Csolid= 2.06 J/°C•g
Cliquid= 4.184 J/°C•g
Cgas = 2.02 J/°C•g
Hf = 334 J/g
Hv = 2260 J/g
4. Calculate the number of joules released when 25.0 grams of steam is cooled from 115.0°C to -57.0°C.
5. Calculate the amount of energy used when 33.3 grams of ice at 0.00°C is converted to steam at 150.0°C.
6. Calculate the specific heat of a metal if 45.0 grams of the metal at 100.0C, when placed into 150.0 grams of water at
20.0C, produces a final temperature of 22.5C.
7. The combustion of ethane, C2H4, is an exothermic reaction and releases 1.39 kJ of heat. Calculate the amount of heat
liberated, in kJ, when 4.79 g of C2H4 reacts with excess oxygen.
C2H4(g) + 3O2(g) → 2CO2(g) + H2O(l)
Acids & Bases
Label the Brønsted-Lowry acid, base, conjugate acid, and conjugate base.
1.
HSO4-
+
H2O

H3O+
+
SO42-
2.
HCO3-
+
H2O

OH-
+
H2CO3
3.
HSO4-
+
H3O+

H2O
+
H2SO4
4.
NH3
+
HSO3- 
NH4+
+
SO32-
5. Complete the following table:
pH
[H+]
pOH
5.4 x 10–4
(a)
Acidic,
basic, or
neutral?
7.8 x 10-10
(b)
(c)
[OH–]
10.75
(d)
5.00
6. 50. ml of 0.45 M Sr(OH)2 are required to titrate a 0.75 M H2SO4 sample. What is the volume of the H2SO4?
7. Calculate the [H+] for a solution with a pOH of 8.37.
8. What is the [OH-] of H2SO4 if the [H+] is 9.79 x 10-3 M at 25°C?