In the given chemical reaction, colors of the Fe$$^{2+}$$ and Fe$$^{3+}$$ ions, are respectively:
$$5Fe^{2+} + MnO_4^- + 8H^+ \rightarrow Mn^{2+} + 4H_2O + 5Fe^{3+}$$

We look at the reaction

$$5\,\text{Fe}^{2+} + \text{MnO}_4^- + 8\text{H}^+ \rightarrow \text{Mn}^{2+} + 4\text{H}_2\text{O} + 5\,\text{Fe}^{3+}$$

This is a redox change in which iron is present in the $$+2$$ and $$+3$$ oxidation states. To answer the question we only need to recall the characteristic solution colours of these two oxidation states of iron.

In aqueous solution the $$\text{Fe}^{2+}$$ ion forms the hexaaqua complex $$[\text{Fe(H}_2\text{O)}_6]^{2+}$$. The transition-metal d-d electronic transitions in this $$d^6$$ ion give a pale green appearance; many standard qualitative-analysis charts describe the colour simply as “green”.

Similarly, the $$\text{Fe}^{3+}$$ ion forms $$[\text{Fe(H}_2\text{O)}_6]^{3+}$$. Because the vacant $$d$$ orbitals lie lower in energy, the absorbed wavelengths shift, and the transmitted light is yellow to brown. In dilute solution the colour is usually noted as “yellow”; in more concentrated solutions it darkens toward brown. For examination purposes “yellow” is the accepted answer.

So the $$\text{Fe}^{2+}$$ ion is green, while the $$\text{Fe}^{3+}$$ ion is yellow.

Looking at the options, option D states “Green, Yellow”, which matches our conclusion.

Hence, the correct answer is Option D.