Question

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

$\left(\mathit{a}\right)\mathit{S}\mathit{r}\left(\mathit{s}\right)\mathbf{+}\mathit{B}{\mathit{r}}_{\mathbf{2}}\left(\mathit{l}\right)\mathbf{\to }$

$\left(\mathit{b}\right)\mathit{A}{\mathit{g}}_{\mathbf{2}}\mathit{O}\left(\mathit{s}\right)\stackrel{\mathbf{\Delta }}{\mathbf{\to }}$

$\left(\mathit{c}\right)\mathit{M}\mathit{n}\left(\mathit{s}\right)\mathbf{+}\mathit{C}\mathit{u}{\left(\mathit{N}{\mathit{O}}_3\right)}_{\mathbf{2}}\left(\mathit{a}\mathit{q}\right)\mathbf{\to }$

Short answer

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

(a)$Sr\left(s\right)+B{r}_2\left(l\right)\to SrB{r}_2\left(s\right)$

(b)$2A{g}_{2}O\left(s\right)\stackrel{\Delta }{\to }4Ag\left(s\right)+O_2\left(g\right)$

(c)$Mn\left(s\right)+Cu{\left(N{O}_3\right)}_2\left(aq\right)\to Mn{\left(N{O}_3\right)}_2\left(aq\right)+Cu\left(s\right)$

Step-by-step solution

Determine the product of the equation (a) 

The given redox reaction is a combination reaction.

Strontium combines with bromine and forms strontium bromide.

It is a reaction of metal-non metal which produce ionic compound.

The given reaction is:

$Sr\left(s\right)+B{r}_2\left(l\right)\to$

The balanced reaction is:

$Sr\left(s\right)+B{r}_2\left(l\right)\to SrB{r}_2\left(s\right)$

Determine the product of the equation (b)

The given redox reaction is a decomposition reaction.

Silver oxide decomposes and forms silver and oxygen

The given reaction is:

$A{g}_{2}O\left(s\right)\stackrel{\Delta }{\to }$

The balanced reaction is:

$2A{g}_{2}O\left(s\right)\stackrel{\Delta }{\to }4Ag\left(s\right)+O_2\left(g\right)$

Determine the product of the equation (c)

The given redox reaction is a displacement reaction.

The given reaction is:

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

The balanced reaction is:

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