Question

Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:

$\left(\mathit{a}\right)\mathit{S}\mathit{b}\left(\mathit{s}\right)\mathbf{+}\mathit{C}{\mathit{l}}_{\mathbf{2}}\left(\mathit{g}\right)\mathbf{\to }\mathit{S}\mathit{b}\mathit{C}{\mathit{l}}_{\mathbf{3}}\left(\mathit{s}\right)$

$\left(\mathit{b}\right)\mathit{A}\mathit{s}{\mathit{H}}_{\mathbf{3}}\left(\mathit{g}\right)\mathbf{\to }\mathit{A}\mathit{s}\left(\mathit{s}\right)\mathbf{+}{\mathit{H}}_{\mathbf{2}}\left(\mathit{g}\right)$

$\left(\mathit{c}\right)\mathit{Z}\mathit{n}\left(\mathit{s}\right)\mathbf{+}\mathit{F}\mathit{e}{\left(\mathit{N}{\mathit{O}}_3\right)}_{\mathbf{2}}\left(\mathit{a}\mathit{q}\right)\mathbf{\to }\mathit{Z}\mathit{n}{\left(\mathit{N}{\mathit{O}}_3\right)}_{\mathbf{2}}\left(\mathit{a}\mathit{q}\right)\mathbf{+}\mathit{F}\mathit{e}\left(\mathit{s}\right)$

Short answer

The classification of the given reactions are:

(a) Combination reaction

(b) Decomposition reaction

(c) Displacement reaction

Step-by-step solution

Write balanced reaction of equation (a)

The given reaction is:

$Sb\left(s\right)+C{l}_2\left(g\right)\to SbC{l}_3\left(s\right)$

The balanced reaction is:

$2Sb\left(s\right)+3C{l}_2\left(g\right)\to 2SbC{l}_3\left(s\right)$

The given redox reaction is a combination reaction.

In this reaction,$\text{Sb}$and$C{l}_2$combines and forms$SbC{l}_3.$

Write balanced reaction of equation (b) 

The given reaction is:

$As{H}_3\left(g\right)\to As\left(s\right)+H_2\left(g\right)$

The balanced reaction is:

$2As{H}_3\left(g\right)\to 2As\left(s\right)+3H_2\left(g\right)$

The given redox reaction is a decomposition reaction.

In this reaction, ${\text{AsH}}_{\text{3}}$ decomposes and forms $\text{As}$and $H_2.$

Write balanced reaction of equation (c)

The given reaction is:

$Zn\left(s\right)+Fe{\left(N{O}_3\right)}_2\left(aq\right)\to Zn{\left(N{O}_3\right)}_2\left(aq\right)+Fe\left(s\right)$

The balanced reaction is:

$Zn\left(s\right)+Fe{\left(N{O}_3\right)}_2\left(aq\right)\to Zn{\left(N{O}_3\right)}_2\left(aq\right)+Fe\left(s\right)$

The given redox reaction is a displacement reaction.

The$\text{Zn}$atom replaces iron atom from $Fe{\left(N{O}_3\right)}_2$ and forms $Zn{\left(N{O}_3\right)}_2.$