Question

Write two balanced half-reactions for this redox equation:

Fe + Cl2 → FeCl3

Answer 1

First we need to write a balance equation for this redox reaction

`2Fe _(_s_) + 3Cl_2_(_g_) ==> 2FeCl_3_(_a_q_)`

In the above reaction
`Fe` on reactant side has oxidation state 0, while on the product side it has an oxidation state of +3. On the other hand,
`Cl_2` has oxidation state of 0 on reactant side and an oxidation state of -1 on product side.

The metal
`Fe` loses electrons to form
`Fe^3^+` ion and is oxidized. So we write an oxidation half reaction.

`2Fe _(_s_) ==> 2Fe^3^+_(_a_q_) + 6e^-`

and the
`Cl_2` molecule gains electrons to form
`Cl^-` ions and is reduced. The reduction half reaction is

`3Cl_2_(_g_) + 6e^- ==> 6Cl^-_(_a_q_)`.