Using Table $18\mathrm{.}1$ from your book and$/$or the list of standard reduction potentials on the next

page, calculate the standard cell potential for each of the following types of batteries and give

the corresponding overall reaction:

$1.$ A normal AA battery is typically a type of alkaline battery, also known as an alkaline$$

manganese battery. It contains a zinc anode $($negative terminal$),$ a manganese dioxide

cathode $($positive terminal$),$ and an alkaline electrolyte solution. The electrochemical

reactions that take place within the battery involve:

$$ the anode: Zn$($s$)->$ Zn$2+($aq$)+2$e$$

$$ the cathode: MnO$2($s$)+4$H$+($aq$)+2$e$->$ Mn$2+($aq$)+2$H$2$O$($l$)$

$2.$ A normal car battery is typically a lead$$acid battery, which consists of lead dioxide

$($PbO$2)$ as the positive electrode $($cathode$),$ sponge lead $($Pb$)$ as the negative electrode

$($anode$),$ and a sulfuric acid $($H$2$SO$4)$ electrolyte solution. The electrochemical reactions

that occur within the battery involve:

$$ the anode: Pb$($s$)->$ Pb$2+($aq$)+2$e$$

$$ the cathode: PbO$2($s$)+4$H$+($aq$)+$ SO$42($aq$)+2$e$->$ PbSO$4($s$)+2$H$2$O$($l$)$

$3.$ In a lithium$-$ion battery, the electrochemical reactions involve lithium ions $($Li$+)$ moving

between a graphite$-$based anode and a metal oxide cathode, such as cobalt$($III$)$ oxide.

Here are the simplified half$-$reactions that occur during the discharge of a lithium$-$ion

battery:

$$ the anode: Li$($s$)->$ Li$+($aq$)+$ e$$

$$ the cathode: Co$3+($aq$)+$ e$->$ Co$2+($aq$)$