Lawrie Ryan and Roger Norris Solutions for Chapter: Electrochemistry, Exercise 3: Questions

In the chemical reaction, ${\mathrm{CuCl}}_2 + \mathrm{Fe} \to {\mathrm{FeCl}}_2 + \mathrm{Cu}$

i. Which species gains electrons?

ii Which species loses electrons?

iii Which species is the oxidising agent?

iv Which species is the reducing agent?

In the chemical reaction, $\mathrm{Cu} + {\mathrm{Br}}_2 \to {\mathrm{Cu}}^{2+}+2{\mathrm{Br}}^{-}$

i. Which species gains electrons?

ii Which species loses electrons?

iii Which species is the oxidising agent?

iv Which species is the reducing agent?

In the chemical reaction, ${\mathrm{PbO}}_2 + {\mathrm{SO}}_2 \to {\mathrm{PbSO}}_4$

i. Which species gains electrons?

ii Which species loses electrons?

iii Which species is the oxidising agent?

iv Which species is the reducing agent?

Construct full redox equation for the following pair of half-equations. The reaction of iodide ions with hydrogen peroxide:
$$\begin{gathered} {\mathrm{I}}^{-}\to \frac{1}{2}{\mathrm{I}}_2+ {\mathrm{e}}^{-} \\ {\mathrm{H}}_2{\mathrm{O}}_2 + 2{\mathrm{H}}^{+}+2{\mathrm{e}}^{-} \to 2{\mathrm{H}}_2\mathrm{O} \end{gathered}$$
 

Construct full redox equation for the following pair of half-equations. The reaction of chloride ions with acidified manganese(IV) oxide:
$$\begin{gathered} {\mathrm{Cl}}^{-}\to \frac{1}{2}{\mathrm{Cl}}_2 + {\mathrm{e}}^{-} \\ {\mathrm{MnO}}_2 + 4{\mathrm{H}}^{+} + 2{\mathrm{e}}^{-} \to {\mathrm{Mn}}^{2+} + 2{\mathrm{H}}_2\mathrm{O} \end{gathered}$$

Construct full redox equation for the following pair of half-equations. The reaction of acidified ${\mathrm{MnO}}_4^{-}$ ions with ${\mathrm{Fe}}^{2+}$ ions:
$$\begin{gathered} {\mathrm{Fe}}^{2+}\to {\mathrm{Fe}}^{3+} +{\mathrm{e}}^{-} \\ {\mathrm{MnO}}_4^{-} +8{\mathrm{H}}^{+} +5{\mathrm{e}}^{-} \to {\mathrm{Mn}}^{2+}+ 4{\mathrm{H}}_2\mathrm{O} \end{gathered}$$