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Date: ____________
Period: _______
Chemistry Student Learning Objective Review Part 3
Unit 7: Chemical Reactions Chapter 11
1. Define/describe the following types of reactions
a. Synthesis
b. Decomposition
c. Single Replacement
d. Double Replacement
e. Neutralization
f. Combustion
2. Identifying types of reactions shown below (DO NOT BALANCE REACTOINS)
Equation
Type of Reaction
1. N2 + H2 → NH3
1. __________________________
2. KClO3 → KCl + O2
2. __________________________
3. C8H18 + O2 → CO2 + H2O
3. __________________________
4. NaCl + F2 → NaF + Cl2
4. __________________________
5. AgNO3 + MgCl2 → AgCl + Mg(NO3)2
5. __________________________
6. CH4 + O2 → CO2 + H2O
6. __________________________
7. Sr(OH)2 + HI → SrI2 + H2O
7. __________________________
8. C3H6 + O2 → CO2 + H2O
8. __________________________
9. FeCl3 + NaOH → Fe(OH)3 + NaCl
9. __________________________
10. Na + H2O → NaOH +H2
10. __________________________
11. NaOH +HCl → NaCl + H2O
11. __________________________
12. Ag2O → Ag + O2
12. __________________________
13. S8 + O2 → SO3
13. __________________________
14. K + MgBr2 → KBr + Mg
14. __________________________
3. Balance the following reactions and identify the type of reaction (show balancing work)
a)
___Na +
NaNO3 
b)
___N2 +
O2
Na2O +
___N2O5
N2
Type: __________________________
Type: __________________________
c) _____H3PO4 + ____Ca(OH)2_____Ca3(PO4)2 + _____H2OType: __________________________
d) ____AlCl3 + ____Na2CO3____Al2(CO3)3 + _____NaCl
Type: __________________________
e) _____AlCl3 _____Al + _____Cl2
Type: __________________________
f)
Type: __________________________
_____ C2H6 + _____ O2 → _____ CO2 + _____ H2O
4. What are the 7 diatomic elements?
5. Turn the following word equations into skeleton equations (don’t balance # of atoms)
a) When solid potassium nitrate is heated, it forms solid potassium nitrite and oxygengas.
b) When dissolved sodium hydroxide reacts with sulfuric acid aqueous sodium sulfate and
water are formed.
c) zinc metal and oxygen gas react to produce zinc oxide
d) Sodium phosphate and calcium chloride react to form calcium phosphate and sodium
chloride.
e) sodium chloride and lead (II) nitrate produce lead (II) chloride and sodium nitrate
f) In a blast furnace, iron (III) oxide and carbon monoxide gas produce carbondioxide gas and
iron.
Unit 8& 9: Chemical Quantities Chapter 10& 12
6. Find the percent composition for the following problems, show ALL calculations.
a. Percent composition of Chromium in Sn(Cr2O7)2
b. Percent composition of oxygen in calcium acetate
c. Percent composition of Strontium in Sr3N2
7. Define and give example of:
a. Empirical formula
b. Molecular formula
8. Empirical/Molecular formula practice
a. What is empirical formula for C4H10?
b. What is empirical formula for C12H22O2?
c. A compound with an empirical formula of C4H4O and a molar mass of 136 grams per mole.
What is the molecular formula of this compound?
d. Empiricalformula is C2H4NO. If its molar mass is 116.1 g/mol, what is the molecular
formula?
9. Complete the following stoichiometric equalities
a. _________ mole = ___________ liters
c. _________ mole = _________ grams
b. _________ mole = ____________ particles
d. _________ mole = ________ molecules
10. Complete the following conversions showing ALL work with units (including molar mass
calculations).
4P(s) + 5O2(g) →2P2O5(s)
a. If you have 56.7 g of oxygen how many liter of oxygen do you have?
b. When 276.6 g of phosphorous is reacted with excess oxygen how many grams of P2O5 did
you produce?
C2H4+ 3O2→ 2CO2 + 2H2O
c. If you produced 46.56 grams of water how many grams of oxygen did your react?
d. If 12.5 g of C2H4 is reacted with 12.5 g O2 how many grams of CO2 did you produce?
e. 5.75 grams of Iron react with 6.05 grams of Chlorine producing 14.50 grams Iron (III)
Chloride.
i. Write a balanced chemical equation for the reaction above
ii. Determine the limiting reactant.
iii. Calculate the theoretical yield of Iron (III) Chloride
iv. Determine the percent yield of Iron (III) Chloride.
f. 12.5 grams of Iodine react with 11.9 grams of Chlorine producing 19.5 grams Iodine
Trichloride.
i. Write a balanced chemical equation for the reaction above
ii. Determine the limiting reactant.
iii. Calculate the theoretical yield of Iodine Trichloride.
iv. Determine the percent yield of Iodine Trichloride.