Question

Write a half balanced equation for the oxidation that occurs in the operating cell

Answer 1

`\text{ Mg}_(\left(s\right))\text{ }\rightarrow\text{ Mg}_(\left(aq\right))\text{ + 2e}^-`

Step-by-step explanation:

Here, we want to write a balanced half-cell reaction for oxidation

Firstly, we have to identify the species being reduced (they are the ones that undergo oxidation)

Oxidation usually involves the loss of electrons. From what we can see, Magnesium lost 2 electrons to become positively charged

Thus, we have the oxidation half-reaction as:

`Mg\placeholder{⬚}_(\left(s\right))\rightarrow\text{Mg}^(2+)\text{ + 2e}^-`