4.94P - Chemistry: Molecular Nature Of Matter And Change

Question

Predict the product(s) and write a balanced equation for each of the following redox reactions:

$\left(a\right)\mathbf{ }\mathbf{Fe}\left(s\right)\mathbf{+}{\mathbf{HClO}}_{\mathbf{4}}\left(\mathrm{aq}\right)\mathbf{\to }$

$\left(b\right){\mathbf{S}}_{\mathbf{8}}\left(s\right)\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\left(g\right)\mathbf{\to }$

$\left(c\right) {\mathbf{BaCl}}_{\mathbf{2}}\left(l\right)\stackrel{\mathbf{electricity}}{\mathbf{\to }}$

Step-by-Step Solution

Answer

The product and the balanced equation of the given reactions are:

$\text{Fe}\left(\text{s}\right){\text{+HClO}}_{\text{4}}\left(\text{aq}\right)\to \text{Fe}{\left({\text{ClO}}_{\text{4}}\right)}_{\text{2}}\left(\text{aq}\right){\text{+H}}_{\text{2}}\left(\text{g}\right)$

${\text{S}}_{\text{8}}\left(\text{s}\right){\text{+O}}_{\text{2}}\left(\text{g}\right)\to {\text{8SO}}_{\text{2}}\left(\text{g}\right)$

${\mathrm{BaCl}}_2\left(\mathrm{l}\right)\stackrel{\mathrm{electricity}}{\to }\mathrm{Ba}\left(\mathrm{l}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

Determination of the product of equation (a)

The given redox reaction is a displacement reaction.

Iron displaces two hydrogen atoms from ${\mathrm{HClO}}_4$  and $\mathrm{Fe}{\left({\mathrm{ClO}}_4\right)}_2$ forms    

Balanced chemical equation of (a)

The given reaction is:

 $\mathrm{Fe}\left(\mathrm{s}\right)+{\mathrm{HClO}}_4\left(\mathrm{aq}\right)\to$

The balanced reaction is:

$\mathrm{Fe}\left(\mathrm{s}\right)+{\mathrm{HClO}}_4\left(\mathrm{aq}\right)\to \mathrm{Fe}{\left({\mathrm{ClO}}_4\right)}_2\left(\mathrm{aq}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

Determination of the product of equation (b)

The given redox reaction is a combination reaction.

Sulfur combines with oxygen and forms sulfur dioxide.

Balanced chemical equation of (b)

The given reaction is:

 ${\mathrm{S}}_8\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to$

The balanced reaction is:

${\mathrm{S}}_8\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to 8{\mathrm{SO}}_2\left(\mathrm{g}\right)$

Determination of the product of equation (c)

The given redox reaction is a decomposition reaction.

 BaCl₂ decomposes and forms Ba and Cl₂

 

Balanced chemical equation of (c)

The given reaction is:

 ${\mathrm{BaCl}}_2\left(\mathrm{l}\right)\stackrel{}{\to }$

The balanced reaction is:

${\mathrm{BaCl}}_2\left(\mathrm{l}\right)\stackrel{\mathrm{electricity}}{\to }\mathrm{Ba}\left(\mathrm{l}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$