# Question 12c06

Dec 21, 2016

Here's how I worked it out.

#### Explanation:

The cell is

The cell reactions are:

color(white)(m)2×["MnO"_4^"-""(aq)" +"8H"^"+""(aq)" + "5e"^"-" → "Mn"^"2+""(aq)" + "4H"_2"O(l)"]
color(white)(mmmmmmmmmmmll)5×["2I"^"-""(aq)" →"I"_2"(s)" + "2e"^"-" ]#
$\text{2MnO"_4^"-""(aq)" + "10I"^"-""(aq)" + "16H"^"+""(aq)" → "2Mn"^"2+""(aq)" +"5I"_2"(s)" + "8H"_2"O(l)}$

Cell notation is a shorthand way of expressing a reaction in an electrochemical cell.

• The anode (oxidation) half-reaction is written on the left, and the cathode half-reaction goes on the right.
• The two half-reactions are separated by two bars or slashes representing a salt bridge.
• Individual solid, liquid, or aqueous phases within each half-cell are separated by a single bar.
• The reactants in each half cell are always written first, followed by the products.
• The state of each phase (usually s, l, g, or aq) is included after the species name.

Thus, the cell notation for this cell is

$\text{C(s) | " "I"^"-""(aq)"| "I"_2"(s) ""||"color(white)(l)"H"^"+""(aq), MnO"_4^"-""(aq), Mn"^"2+""(aq) | C(s)}$