Step 1: Understand concept of standard electrode potential.
When multiple redox steps are involved, overall potential is not simple addition but weighted based on electron transfer numbers in each step. Step 2: Break into half reactions.
MnO\(_4^-\) → MnO\(_2\) corresponds to 3 electron change.
MnO\(_2\) → Mn\(^{2+}\) corresponds to 2 electron change. Step 3: Use energy additivity principle.
\[
\Delta G^\circ = -nFE^\circ
\]
Total free energy change is additive, so:
\[
n_{total}E_{total} = n_1E_1 + n_2E_2
\] Step 4: Substitute values.
Total electrons = 5:
\[
5E = 3x + 2y
\] Step 5: Solve for E.
\[
E = \frac{3x + 2y}{5}
\] Step 6: Final conclusion.
Thus standard potential for overall reaction is weighted average based on electrons transferred. Final Answer:
\[
\boxed{\frac{3x + 2y}{5}}
\]