QUESTION 8 Identify the oxidation-reduction reactions among the following: 1. Zn(s) + 2HCl(aq) ---------> ZnCl2(aq) + H2(g) 2. 2Mg(s) + O2(g) ----------> 2MgO(s) 3. 2Na(s) + Cl2(g) ----------> 2NaCl D) 1 and 2 only 2 and 3 only All of 1, 2, and 3 1 and 3 only
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In an oxidation-reduction (redox) reaction, one species is oxidized (loses electrons) and another species is reduced (gains electrons). Show more…
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Determine which of the following are oxidation-reduction reactions. For those that are, identify the oxidizing and reducing agents. (a) $3 \mathrm{Zn}(\mathrm{s})+2 \mathrm{CoCl}_{3}(\mathrm{aq}) \longrightarrow 3 \mathrm{ZnCl}_{2}(\mathrm{aq})+2 \mathrm{Co}(\mathrm{s})$ (b) $\mathrm{ICl}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{HCl}(\mathrm{aq})+\mathrm{HIO}(\mathrm{aq})$ $$ \text { (c) } \begin{aligned} 3 \mathrm{HCl}(\mathrm{aq})+\mathrm{HNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{Cl}_{2}(\mathrm{~g})+& \mathrm{NOCl}(\mathrm{g}) \\ &+2 \mathrm{H}_{2} \mathrm{O}(\ell) \end{aligned} $$ (d) $\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \stackrel{\text { heat }}{\longrightarrow} 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{~g})$
Which two of the following reactions are oxidation-reduction reactions? Explain your answer in each case. Classify the remaining reaction. (a) $\mathrm{Zn}(\mathrm{s})+2 \mathrm{NO}_{3}^{-}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow$ $\mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{NO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$ (b) $\operatorname{Zn}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \longrightarrow \mathrm{ZnSO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$ (c) $\mathrm{Ca}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{g})$
Identify each of the following as an oxidation or a reduction reaction: (7.5) a. $\mathrm{Zn}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Zn}(s)$ b. $\mathrm{Al}(s) \longrightarrow \mathrm{Al}^{3+}(a q)+3 e^{-}$ c. $\mathrm{Pb}(s) \longrightarrow \mathrm{Pb}^{2+}(a q)+2 e^{-}$ $\mathbf{d} . \mathbf{C l}_{2}(g)+2 e^{-} \longrightarrow 2 \mathbf{C l}^{-}(a q)$
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