General Chemistry Principles, Patterns, and Applications, 2011

8. For each redox reaction, determine the identities of the oxidant, the reductant, the species oxidized, and the
species reduced.
a. H 2 (g) + I 2 (s) → 2HI(g)
b. 2Na(s) + 2H 2 O(l) → 2NaOH(aq) + H 2 (g)
c. 2F 2 (g) + 2NaOH(aq) → OF 2 (g) + 2NaF(aq) + H 2 O(l)
9. For each redox reaction, determine the identities of the oxidant, the reductant, the species oxidized, and the
species reduced.
a. 2Na(s) + Cl 2 (g) → 2NaCl(s)
b. SiCl 4 (l) + 2Mg(s) → 2MgCl 2 (s) + Si(s)
c. 2H 2 O 2 (aq) → 2H 2 O(l) + O 2 (g)
10. Balance each chemical equation. Then identify the oxidant, the reductant, the species oxidized, and the
species reduced. (Δ indicates that the reaction requires heating.)
a. H 2 O(g) + CO(g) → CO 2 (g) + H 2 (g)
b. the reaction of aluminum oxide, carbon, and chlorine gas at 900ºC to produce aluminum
chloride and carbon monoxide
c. HgO(s) → Δ Hg(l) + O 2 (g)
11. Balance each chemical equation. Then identify the oxidant, the reductant, the species oxidized, and the
species reduced. (Δ indicates that the reaction requires heating.)
a. the reaction of water and carbon at 800ºC to produce hydrogen and carbon monoxide
b. Mn(s) + S 8 (s) + CaO(s) → CaS(s) + MnO(s)
c. the reaction of ethylene and oxygen at elevated temperature in the presence of a silver catalyst to produce
ethylene oxide
12.
a. ZnS(s) + H 2 SO 4 (aq) + O 2 (g) → ZnSO 4 (aq) + S 8 (s) + H 2 O(l)
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