Quick questions on Balancing redox half-equations: TCE Chemistry (Tasmania)

Use this order for each half-equation:

Many TASC redox reactions occur in acidic solution, but some are in basic conditions. The simplest approach is to balance the equation first as if it were acidic (using $\text{H}^+$ and $\text{H}_2\text{O}$), then neutralise the $\text{H}^+$ by adding the same number of $\text{OH}^-$ to both sides. The $\text{H}^+$ and $\text{OH}^-$ on one side combine to form water, and you cancel any water that then appears on both sides. The result is a half-equation containing $\text{OH}^-$ and $\text{H}_2\text{O}$ but no $\text{H}^+$, appropriate for a basic medium.

Each balanced half-equation is exactly the reaction that occurs at one electrode of an electrochemical cell: the oxidation half is the anode reaction and the reduction half is the cathode reaction. The number of electrons in the half-equation is the same number used in Faraday's law calculations and in finding standard cell potentials. Building the skill of writing clean half-equations therefore pays off directly in the electrochemistry and electrolysis questions later in Unit 3.