Quick questions on Redox reactions - WJEC A-Level Chemistry

The reliable method is to write each half equation, balance it fully, then scale and add. Balance the atoms being oxidised or reduced first, then balance oxygen with water, then hydrogen with $\text{H}^+$, then balance the charge by adding electrons. Multiply the two half equations so the electrons match, then add them and cancel the electrons and any species appearing on both sides. This routine works for any acidified redox reaction, including the dichromate and manganate systems that recur in titrations.

State, in terms of electrons, what happens to a reducing agent. [1 mark]

State the colour change at the end point of an iron(II) versus manganate(VII) titration. [1 mark]

Balance the half equation $\text{Fe}^{2+} \rightarrow \text{Fe}^{3+}$. [1 mark]

State the colour change when acidified dichromate(VI) acts as an oxidising agent. [1 mark]

State the order of steps for balancing an acidified half equation. [1 mark]