Predicting the products of a Redox Reaction Predict whether the following redox reactions will occur: (a)[latex] Hg^{2+}(aq) + Zn(s) \longrightarrow Hg(l) + Zn^{2+}(aq)[/latex] (b) [latex]2 H^{+}(aq) + Cu(s) \longrightarrow H2(g) + Cu^{2+}(aq)[/latex] STRATEGY Look at Table 4.5 to find the relative reactivities of the elements.

(a) Zinc is above mercury in the activity series, so this reaction will occur. (b) Copper is below hydrogen in the activity series, so this reaction will not occur. PRACTICE 4.27 Predict whether the following reaction will occur: [latex]\mathrm{Ca}^{2+}(a q)+\mathrm{Mg}(s) \longrightarrow \mathrm{Ca}(s)+\mathrm{Mg}^{2+}(a q)[/latex] APPLY 4.28 Use the following reactions to arrange the elements A, B, C, and D in order of their strength as a reducing agent from strongest to weakest. [latex]\begin{array}{ll}\mathrm{A}+\mathrm{D}^{+} \longrightarrow \mathrm{A}^{+}+\mathrm{D} & \mathrm{C}^{+}+\mathrm{D} \longrightarrow \mathrm{C}+\mathrm{D}^{+} \\\mathrm{B}^{+}+\mathrm{D} \longrightarrow \mathrm{B}+\mathrm{D}^{+} & \mathrm{B}+\mathrm{C}^{+} \longrightarrow \mathrm{B}^{+}+\mathrm{C}\end{array}[/latex]

Question 4.14: predicting the products of a Redox Reaction Predict whether ...

Chemistry

Predicting the products of a Redox Reaction
Predict whether the following redox reactions will occur:

(a) $Hg^{2+}(aq) + Zn(s) \longrightarrow Hg(l) + Zn^{2+}(aq)$

(b) $2 H^{+}(aq) + Cu(s) \longrightarrow H2(g) + Cu^{2+}(aq)$

STRATEGY

Look at Table 4.5 to find the relative reactivities of the elements.

TABLE 4.5 A Partial Activity Series of the Elements
Oxidation Reaction
	These elements react rapidly with aqueous $H^{+}$ ions (acid) or with liquid	$\begin{Bmatrix} Li\rightarrow Li^{+} + e^{-} \\ K\rightarrow K^{+}+ e^{-} \\ Ba\rightarrow Ba^{2+}+2e^{-}\\Ca\rightarrow Ca^{2+}+2 e^{-}\\Na \rightarrow Na^{+}+e^{-} \end{Bmatrix}$
	These elements react with aqueous $H^{+}$ ions or with stea to release $H_{2}$ gas.	$\begin{Bmatrix} Mg\rightarrow Mg^{2+} + 2e^{-} \\ Al\rightarrow Al^{3+}+ 3e^{-} \\ Mn\rightarrow Mn^{2+}+2e^{-}\\Zn \rightarrow Zn^{2+}+2 e^{-}\\Cr\rightarrow Ca^{3+}+3 e^{-}\\Fe \rightarrow Fe^{2+}+2e^{-} \end{Bmatrix}$
	These elements react with aqueous $H^{+}$ ions to release $H_{2}$ gas.	$\begin{Bmatrix} Co\rightarrow Co^{2+} + 2e^{-} \\ Ni\rightarrow Ni^{2+}+ 2e^{-} \\ Sn\rightarrow Sn^{2+}+2e^{-}\\ \end{Bmatrix}$ $H_{2}\rightarrow 2 H^{+}+2e^{-}$
	These elements do not react with aqueous $H^{+}$ ions to release $H_{2}$ .	$\begin{Bmatrix} Cu\rightarrow Cu^{2+} + 2e^{-} \\ Ag\rightarrow Ag^{+}+ e^{-} \\ Hg\rightarrow Hg^{2+}+2e^{-}\\ Pt\rightarrow Pt^{2+}+2 e^{-}\\ Au\rightarrow Au^{3+}+3 e^{-} \end{Bmatrix}$

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