CHEM 1A  Lecture Quiz 3 • Spring 2014
Name:_________________________________________
Categorize each reaction below as ONE of the following types. Each reaction will only fit in one
category.
A.
B.
C.
D.
E.
Double Replacement
Single Replacement
Synthesis
Decomposition
Combustion
Type of Reaction
1. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O
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2. MgCl2 + H2 → Mg + 2 HCl
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3. 2 B + 3 Cl2 → 2 BCl3
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4. 8 SF6 → S8 + 24 F2
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5. Ca3(PO4)2 + 6 CuCl → 3 CaCl2 + 2 Cu3PO4
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6. CaCO3 → CaO + CO2
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7. 2 Li + 2 HCl → 2 LiCl + H2
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For each of the processes below, write a proper balanced chemical equation in the space
provided.
8. The decomposition of Al(NO3)3 to produce aluminum metal, nitrogen gas and oxygen gas:
_________________________________________________________________________
9. The synthesis of P2O5 from P4(s) and oxygen gas:
_________________________________________________________________________
10. The complete combustion of C5H10O5:
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For each set of reactants below predict the possible products AND balance the equation. If the
reaction is NOT expected to occur, CIRCLE THE REACTANTS. If the reaction IS expected to
occur, CIRCLE THE PRODUCTS.
Hint: A reactivity series is available on the back of this quiz.
11. _______Mg(s) + _______FeCl3(s) → _______________________________________________
12. _______ Br2(l) + _______ AlF3(s) → _______________________________________________
13. Circle ALL of the substances or solutions below that are STRONG electrolytes. PAY ATTENTION TO
THE PHASES.
A. C6H12O6(aq)
B. MgBr2(aq)
C. SO3(g)
D. PbI2(s)
E. Al(NO3)3(aq)
14. How many grams of sodium hydroxide would be needed to produce 250.0 mL of NaOH (aq) solution
with a concentration of 0.25 M? Hint: the molar mass of NaOH is 39.997 g/mol.
15. Consider the reaction below:
3 Mg(OH)2(aq) + 2 H3PO4(aq) → Mg3(PO4)2(s) + 6 H2O(l)
An aqueous solution of phosphoric acid (volume = 10.00 mL) was titrated with a magnesium hydroxide
solution. If 35.91 mL of 0.1299 M Mg(OH)2(aq) was required in the titration, determine the concentration of the
phosphoric acid solution (in mol/L).
For each ion or molecule below, determine the oxidation number for each type of atom
present.
16. ClO4-
Cl:________ O:________
17. CF2H2
F:________ H:________ C:________
18. S2O42-
S:________ O:________
For each reaction below, CIRCLE THE OXIDIZING AGENT, and write a STAR ABOVE THE
REDUCING AGENT.
19.
5 H2C2O4 + 2 MnO4- + 6 H+ → 10 CO2 + 2 Mn2+ + 8 H2O
20.
Cr2O72- + 6 Fe2+ + 14 H+ → 2 Cr3+ + 6 Fe3+ + 7 H2O
Balance the separate, unrelated half reactions below. Label each as an OXIDATION or a
REDUCTION.
Oxidation or Reduction?
21.
Ni2+ → Ni2O3
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22.
S2O32- → S4O62-
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23.
Balance the redox reaction below using the method of half reactions. SHOW YOUR WORK FOR
FULL CREDIT.
Te(s) + NO3- → TeO2(s) + NO(g)
EXTRA CREDIT: (5 points)
Balance the reaction below.
____ S8 + ____ HNO3 + → ____ H2SO4 + ____ NO2 + ____ H2O