Question dfa6b

Jun 9, 2017

Here's what I get.

Explanation:

In a silver oxide-zinc battery, the positive electrode (cathode) consists of $\text{Ag"_2"O}$ and added graphite to improve conductivity.

The negative electrode (anode) is $\text{Zn}$ powder mixed with a gelling agent and an electrolyte that is usually aqueous ($\text{KOH}$). The two half-cells are separated by a permeable combination of layers of plastic membrane, treated cellophane, and absorbent fibres.

The top cup is made of laminated layers of copper, tin, steel, and nickel, and the bottom cup is nickel-plated steel.

An insulating gasket prevents contact between the two cups.

The silver is reduced at the cathode from $\text{Ag(I)}$ to $\text{Ag}$, and the zinc is oxidized from $\text{Zn}$ to $\text{Zn(II)}$.

The equations for the half-cell reactions and the overall cell reaction are:

$\textcolor{w h i t e}{m m m m m m m m m m m m m m m m m m m m m m m m m m m m} {E}^{\circ} \text{/V}$
At the anode: color(white)(m)"Zn" + 2"OH"^"-" → "Zn(OH)"_2 + 2"e"^"-";color(white)(mmmml) +1.245
At the cathode: "Ag"_2"O" + "H"_2"O" +2"e"^"-"– → "2Ag" + 2"OH"^"-";color(white)(ll) +0.34
Overall: color(white)(mmml)"Ag"_2"O" + "Zn" + "H"_2"O" → "2Ag" + "Zn(OH)"_2; +1.68#