Chapter 17: Problem 71
An oxidizing agent causes the (oxidation/reduction) of another species, and the oxidizing agent itself is (oxidized/reduced).
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
For each of the following oxidation-reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a. \(2 \mathrm{K}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{K}_{2} \mathrm{O}(s)\) b. \(\mathrm{H}_{2}(g)+\mathrm{S}(s) \rightarrow \mathrm{H}_{2} \mathrm{S}(g)\) c. \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightarrow 2 \mathrm{NH}_{3}(g)\) d. \(2 \mathrm{Hg}(l)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{Hg}_{2} \mathrm{Cl}_{2}(s)\)
Which electrode in a galvanic cell is the anode? Which is the cathode?
Balance each of the following oxidation-reduction reactions, which take place in acidic solution, by using the "half-reaction" method. a. \(\mathrm{Al}(s)+\mathrm{H}^{+}(a q) \rightarrow \mathrm{Al}^{3+}(a q)+\mathrm{H}_{2}(g)\) b. \(\mathrm{S}^{2-}(a q)+\mathrm{N O}_{3}^{-}(a q) \rightarrow \mathrm{S}(s)+\mathrm{N O}(g)\) c. \(\mathrm{I}_{2}(a q)+\mathrm{Cl}_{2}(a q) \rightarrow \mathrm{IO}_{3}^{-}(a q)+\mathrm{HCl}(g)\) d. \(\mathrm{A s O}_{4}^{-}(a q)+\mathrm{S}^{2-}(a q) \rightarrow \mathrm{A s O}_{3}^{-}(a q)+\mathrm{S}(s)\)
In each of the following reactions, identify which element is oxidized and which is reduced. a. \(2 \mathrm{Al}(s)+6 \mathrm{HCl}(a q) \rightarrow 2 \mathrm{AlCl}_{3}(a q)+3 \mathrm{H}_{2}(g)\) b. \(2 \mathrm{HI}(g) \rightarrow \mathrm{H}_{2}(g)+\mathrm{I}_{2}(s)\) c. \(\mathrm{Cu}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{CuSO}_{4}(a q)+\mathrm{H}_{2}(g)\)
For each of the following oxidation-reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a. \(6 \mathrm{Na}(s)+\mathrm{N}_{2}(g) \rightarrow 2 \mathrm{Na}_{3} \mathrm{N}(s)\) b. \(\mathrm{Mg}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{MgCl}_{2}(s)\) c. \(2 \mathrm{Al}(s)+3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{AlBr}_{3}(s)\) d. \(4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\)
What do you think about this solution?
We value your feedback to improve our textbook solutions.
